# Question Bank. Calorimetry

Save this PDF as:

Size: px
Start display at page:

## Transcription

1 Calorimetry 1. Define the term heat. Ans. It is the sum total of kinetic and potential energy of all the molecules of a given substance. 2. Name the SI unit of heat. Ans. Joule (J) is the SI unit of heat. 3. Define temperature : Ans. The average kinetic energy of all the molecules of a given substance is called temperature. 4. State the SI unit of temperature. Ans. Kelvin (K) is the SI unit of temperature. 5. The temperature of a substance rises by 25 C. How much is the rise on kelvin scale and why? Ans. The rise on kelvin scale is 25 K. It is because, rise in temperature in C = rise in temperature in kelvin. 6. What is a calorimeter? Why is it made of copper? Give two reasons. Ans. A copper vessel along with copper stirrer used in the measurement of heat energy is called calorimeter. Calorimeter is made from copper because, (i) it takes the temperature of the contents within it very quickly. (ii) it has a very low specific heat capacity and hence takes very little amount of heat energy from the contents within it. 1

2 7. (a) Define : (i) Calorie, (ii) Kilocalorie. (b) How many calories are in one kilocalorie? (c) How many joules of energy are in : (i) one calorie, (ii) one kilocalorie? (d) State the SI unit for measuring heat energy. Ans. (a) (i) Calorie : It is the amount of heat energy required to raise the temperature of 1 g of water through 1 C. (ii) Kilocalorie : It is the amount of heat energy required to raise the temperature of 1 kg of water, through 1 C. (b) 1000 calories = 1 kilocalorie (c) (i) 1 calorie = 4.2 J (ii) 1 kilocalorie = 4200 J (d) The SI unit for measurement of heat energy is joule. 8. State three factors, which determine the heat absorbed by a cold body. Ans. (i) Heat absorbed is directly proportional to the mass of the body. (ii) Heat absorbed is directly proportional to the specific heat capacity of the body. (iii) Heat absorbed is directly proportional to the rise in temperature of the body. 2

3 9. (a) Define the following terms : (i) specific heat capacity (ii) thermal capacity or heat capacity. (b) State the SI units of : (i) specific heat capacity (ii) thermal capacity. (c) Which material is calorimeter made of? Ans.(a) (i) The amount of heat energy required to raise the temperature of one kg of a substance through 1 K is called its specific heat capacity. (ii) The amount of heat energy required to raise the temperature of a given mass of a substance through 1 K is called its thermal capacity. (b) (i) The SI unit of specific heat capacity is J kg 1 K 1. (ii) The SI unit of thermal capacity is JK 1. (c) Calorimeter is made from copper. Recently copper has been replaced by aluminium. 10. Specific heat capacity of water is 4200 Jkg 1 k 1. What do you understand by the statement? Ans. From the above statement, it implies that, if the temperature of 1 kg of water is raised through 1 K, then the amount of heat energy required to do so is 4200 J. 3

4 11. The thermal capacity of a vessel is 428 J K 1. What do you understand by the statement? Ans. From the above statement, it implies that, if the temperature of the given vessel is raised through 1 K, then heat energy required to do so is 428 K. 12. The heat capacity of a vessel is 42 J C 1. How much heat energy is required to raise its temperature from 10 C to 20 C? Ans. Rise in temperature = (20 10) C = 10 C Heat energy required to raise its temperature through 10 C = Heat capacity Rise in temperature = 42 J C 1 10 C = 420 J. 13. Some amount of heat energy is supplied to two liquids A and B. The liquid A shows a greater rise in temperature. What can you say about heat capacity of A as compared to that of B? Ans. Heat capacity of A is less than that of B. 14. Why is the base of cooking pan made thick and heavy? Ans. Cooking pans are made from metals such as copper, brass, stainless steel, etc. They have low specific heat capacity and hence rapidly attain the temperature of flame used for heating. This in turn can burn the food. To avoid burning of food the base is made heavy and thick, so that the temperature within the pan is less than the flame and hence the food cooks without burning. 4

5 15. A substance of mass m 1, specific heat capacity c 1 at a temperature T 1 is mixed with another substance of mass m 2, specific heat capacity c 2 at a lower temperature T 2. Deduce the expression for the final temperature of the mixture. State any assumption made, if any. Ans. Let the final temperature of mixture be T Rise in temperature (θ R) = (T T 2 ) Fall in temperature (θ f) = (T 1 T) Now, heat gained by substance at lower temp. = Heat lost by substance at higher temp. m 2 c 2 (T T 2 ) = m 1 c 1 (T 1 T) m 2 c 2 T m 2 c 2 T 2 = m 1 c 1 T 1 m 1 c 1 T m 2 c 2 T + m 1 c 1 T = m 1 c 1 T 1 + m 2 c 2 T 2 (m 2 c 2 + m 1 c 1 )T = m 1 c 1 T 1 + m 2 c 2 T 2 T = mct + m ct mc + mc Why are hot water bottles very efficient for fomentation? Ans.Water has the highest sp. heat capacity of 4.2 Jg 1 C 1. Furthermore, its temperature does not rise beyond 100 C, under normal conditions. Thus, it can store large amount of heat energy at quite a bearable temperature and hence it is ideal for fomentation purposes. 5

6 17. What are land and sea breezes? Explain how are they caused in the coastal regions. Ans. Local winds which blow from the sea to the land during the day-time and from the land to the sea during night-time are called sea and land breezes. Formation of sea breeze : Specific latent heat capacity of land is about five time less, as compared to water. Thus, when the sun shines equally on the sea, as well as on the land, the land gets comparatively hot as compared to the sea. The air above the land gets hot and hence, rises, thereby causing a drop in pressure. To make up for the drop in pressure, the cold air from the sea, blows towards the land, thereby giving rise to sea breeze. Formation of land breeze : At night the sea water, as well as the land radiate heat energy. However, the land radiates heat energy, at much faster rate as compared to the sea, owing to its five times less specific heat capacity, as compared to the sea water. Thus, on the whole, the sea is comparatively warmer as compared to the land. The air above the sea gets warm and rises up. This causes a fall in pressure. To make up for this fall in pressure, the cold air from the land blows towards the sea, thereby giving rise to land breeze. 6

7 18. Discuss the role of high specific heat capacity of water, with reference to the climate in coastal regions. Ans. The climate in coastal regions remains moderate due to the blowing in of the cold air from sea during day-time (sea breeze) and blowing out of the cold air from land to sea (land breeze), during night-time. The land and sea breeze are formed as under : Write here formation of land and sea breeze as in Q Why is water used as a coolant in motor-car radiators? Ans. Water has the highest specific heat capacity of 4.2 Jg 1 C 1 and its temperature does not rise beyond 100 C. Thus, it can absorb large amount of heat from a working engine, which is then radiated out through the radiator. Thus, on this low temperature the engine works efficiently. 20. Why is water sprayed on roads in the evening in hot summer? Ans.Water has the highest specific heat capacity of 4.2 Jg 1 C 1. Thus, water absorbs large amount of heat from the roads, but its own temperature does not rise much. Thus, on the whole the roads get cooled. 21. Why the temperature in hot summer falls sharply, after a sharp shower? Ans. Water has the highest specific heat capacity of 4.2 Jg 1 C 1. Thus, when there is a sharp shower, the water evaporates. In doing so, it absorbs large amount of heat from surroundings, hence temperature falls sharply. 7

8 22. Why do sandy soils get heated up quickly as compared to wet soils? Ans. The specific heat capacity of the sand is about five times less than that of the water. Thus, when sun shines equally on sandy soil and the wet soil, the sandy soil gets heated up rapidly as compared to the wet soil. It is because, water absorbs large amount of heat energy, but its temperature does not rise sufficiently. 23. Why is water considered the best liquid for quenching thirst? Ans. Water has the highest specific heat capacity of 4.2 Jg 1 C 1 and hence it can absorb large amount of heat energy, without rising in temperature sufficiently. Thirst is the natural signal, when body produces more heat energy than required. Thus, water is ideal for quenching thirst, because it can absorb large amount of heat energy. 24. Why is it advisable to pour cold water over burns, caused on the human body, by hot solids? Ans. Water has the highest specific heat capacity of 4.2 Jg 1 C 1. Thus, it can extract large amount of heat energy rapidly from the site of burn and hence gives a lot of relief. 8

9 25. Why does a wise farmer waters his fields, if the forecast says it is going to be frost? Ans. The frost can seriously damage the leaves and fruits of the plants. When a farmer waters his fields, during night, this water gives large amount of heat energy, because 1 g of water will liberate 4.2 J of energy for every 1 C fall in temperature. Thus, the air around the field is saturated with heat energy and its temperature does not fall below 0 C. Thus, no frost is formed. 26. Why are big tubs of water kept in underground cellars for storing fresh fruit and vegetables in cold countries? Ans. During sub-zero temperatures, the water within the cells of fruits and vegetables freezes and hence damages them. To avoid such a damage the huge water tubs are kept. The water gives off 4200 J of heat energy for every one kg for 1 C fall in temperature. Thus, it does not allow the temperature of cellar to fall below 0 C, and hence, their is no damage to fresh fruits or vegetables. 27. Define the following terms : (i)fusion (ii) Melting point Ans. Fusion : The process of changing of a solid in liquid state, at some fixed temperature, by the absorption of heat from some external source is called fusion. Melting point : It is the temperature at which a solid changes into liquid state. 9

10 28. What do you understand by the following terms : (i) latent heat of fusion? (ii) specific latent heat of fusion? (iii) specific latent heat of fusion of ice? (iv) state the value of sp. latent heat of fusion of ice in : (1) the SI system (2) calories? Ans. (i) Latent heat of fusion : It is the amount of heat energy required to change a given mass of solid at its m.p. into its liquid state, without any rise in temperature. (ii) Specific latent heat of fusion : It is the amount of heat energy required to change 1 kg of solid, at its melting point, into its liquid state, without any rise in temperature. (iii) Specific latent heat of fusion of ice : It is the amount of heat energy required to change 1 kg of ice at 0 C, into 1 kg of water at 0 C, without any rise in temperature. (iv) Specific latent heat of fusion of ice is (i) 336,000 Jkg 1 in the SI system (ii) 80 calories g 1 in CGS system. 10

11 29. Bottled drinks are cooled more effectively, when surrounded by lumps of ice than iced water. Or Why do bottled soft drinks get cooled more quickly by ice cubes than by iced water. Ans. Every 1 kg of ice at 0 C absorbs 336,000 J of heat energy to form water at 0 C. As ice can extract 336,000 J of heat energy, more than water at 0 C, therefore, it cools the bottled drinks more effectively. 30. Why does atmospheric temperature fall after a hailstorm? Ans. Ice has the highest sp. latent heat of fusion of 336,000 Jkg 1. Thus, when the hail melts, it absorb large amount of heat energy from the surroundings. Thus, the atmospheric temperature drops. 31. Why does weather become pleasant when it starts freezing in cold countries? Ans. Ice has the highest sp. latent heat of fusion of 336,000 Jkg 1. Thus, every 1 kg of water at 0 C, on freezing releases 336,000 J of heat energy. As enormous amount of heat energy is released in atmosphere, therefore weather becomes pleasant. 32. Why does it gets warm during a snow storm? Ans. Same as Q

12 33. Why does it become bitterly cold when ice melts in cold countries? Ans. Same as Q Specific latent heat of fusion of lead is Jkg 1. What do you understand by the statement? Ans. It means one kg of lead at its melting point, on solidification at the same temperature will release J of heat energy. 35. Given figure shows variation in temperature with time when some wax cools from liquid phase to solid phase. (i) In which part of the curve the wax is in liquid phase? (ii) What does the part QRS represent? (iii) At which point on the curve, the wax will be in the liquid as well as solid phase? (iv) In which part of curve the wax is in solid phase. Ans. (i) Wax is in liquid phase in region PQ. (ii) QRS represents change in state of liquid wax to solid wax at constant temperature. (iii) At point R the wax will be in the solid as well as liquid phase. (iv) Wax is in the solid phase in region ST. 12

13 36. 1 kg of ice at 0 C is heated at a constant rate and its temperature is recorded after every 30 s, till steam is formed at 100 C. Draw a temperature-time graph to represent the change of phase. Ans. 37. The melting point of naphthalene, a crystalline solid, is 80 C and room temperature is 30 C. Liquid naphthalene at 100 C is cooled down to room temperature. Draw a temperature-time graph to represent cooling curve. Ans. 38. Ice-cream appears colder to mouth than water at 0 C. Give a reason. Ans. Ice has the highest sp. latent heat of fusion, i.e., 336 Jg 1. Thus, every one gram of ice on melting in mouth extracts out 336 J of extra heat energy, as compared to water at 0 C. Thus, ice-cream appears colder than water at 0 C. 13

14 39. What do you understand by the following terms? (i) Boiling, (ii) Boiling point. Ans. (i) Boiling : The process of rapid change of a liquid into gaseous state, without any change in temperature, and by the absorption of heat energy from an external source is called boiling. (ii) Boiling point : The constant temperature at which a liquid rapidly changes to its gaseous state is called boiling point. 40. Graph shows change of phases of a substance on temperature-time graph. (a)what do parts AB, BC, and CD represent? (b)what is the melting point of substance? (c) What is the boiling point of substance? Ans.(a) (i) AB represents the solid being heated still it attains a temp T1. (ii) BC represents changes in the state of solid to liquid at constant temperature. (iii) CD represents the liquid being heated till it attains a temperature of T3. (b) The melting point of the substance is T1. (c) The boiling point of the substance is T2. 14

15 Numerical Problems 1. Calculate the amount of heat energy required to raise the temperature of 100 g of copper from 20 C to 70 C (sp. heat capacity of copper = 390 J kg 1 K 1) Ans. Mass of copper (m) = 100 g = 0.1 kg Rise in temperature (θ R ) = (70 20) = 50 C Sp. heat capacity of copper (c) = 390 J kg 1 K 1 Heat required = mcθ R = 390 J kg 1 C 1 = 0.1 kg 390 J kg 1 C 50 C = 1950 J J of heat energy is supplied to raise the temperature of 0.5 kg of lead from 20 C to 40 C. Calculate the specific heat capacity of lead. Ans. Mass of lead (m) = 0.5 kg Rise in temperature (θ R ) = (40 20) C = 20 C Heat required (H) = 1300 J H = mc θ R c = H 1300J mθ 0.5 kg 20 C R = 130 J kg 1 C 1 15

16 3. Find the time taken by a 500 W heater to raise the temperature of 50 kg of a material of specific heat capacity 960 J kg 1 K 1 from 18 C to 38 C. Assume all heat energy supplied by the heater is given to the material. Ans. Power of the heater (P) = 500 W = 500 Js 1 Let the time for which the heater works = t Energy supplied by the heater = P t Rise in temperature of the material = 500 J s 1 t (θ R ) = (38 18) = 20 C = 20 K Mass of the material (m) = 50 kg sp. heat capacity of the material (c) = 960 J kg 1 K 1 Heat energy absorbed by the material = mcθ R = 50 kg 960 J kg 1 K 1 20 K = J Energy supplied by the heater = Heat energy absorbed by the material 500 J s 1 t = J t = J Js = 1920 s = min = 32 min 16

17 4. An electric heater of power 600 W raises the temperature of 4.0 kg of a liquid from 10.0 C to 15.0 C in 100 s. Calculate : (i) heat capacity of 4.0 kg of liquid, (ii) the specific heat capacity of liquid. Ans. Power of heater (P) = 600 W = 600 Js 1 Time (t) = 100 s Energy supplied by heater = P t = 600 Js s = J Rise in temperature (θ R ) = ( ) C = 5 C = 5 K (i) For 5 K rise in temperature energy required = J For 1 K rise in temperature energy required = J 5K = JK 1 Heat capacity of liquid = JK 1 (ii) Specific heat capacity of liquid = Heat capacity Mass JK 4.0 kg 1 1 = 3000 Jkg K 17

18 5. A piece of iron of mass 2.0 kg has thermal capacity 966 J C 1. Find : (i) the heat energy needed to raise it to 15 C and (ii) its sp. heat capacity in SI unit. Ans. (i) Thermal capacity = 966 J C 1 = 966 JK 1 Rise in temperature = 15 C = 15 K Heat energy required to warm iron = Thermal capacity Rise in temperature = 966 JK 1 15 K = J (ii) Specific heat capacity of iron = Thermal capacity Mass of iron 966 JK kg Jkg K kg of lemon squash at 30 C is placed in a refrigerator, which can remove heat at an average of 30 Js 1. How long will it take to cool lemon squash to 5 C? (sp heat capacity of lemon squash is 4200 J kg 1 C 1). Ans. Mass of lemon squash (m) = 0.5 kg sp. heat capacity of lemon squash (c) = 4200 Jkg 1 C 1 Fall in temperature (θ f) = (30 5) C = 25 C Heat extracted by refrigerator (H) = mcθ f = 0.5 kg 4200 Jkg 1 C 1 25 C = J 18

19 Rate of extraction of heat = 30 Js 1 Time in which lemon squash cools = Js 1 = 1750 s 60 = 1750 s = min g mass of a certain metal at 83 C is immersed in 300 g water at 30 C. The final temperature is 33 C. Calculate the specific heat capacity of the metal. (Assume that specific heat capacity of water is 4.2 Jg 1K 1). Ans. DATA Substances Metal Water Mass 200 g 300 g Sp. heat capacity? 4.2 Jg 1K 1 Initial temp. 83 C 30 C Final temp. = 33 C θ R = (33 30) θ f = (83 33) = 3 C = 3 K = 50 C = 50 K Heat lost by metal = mcθ f = 200 g c 50 K Heat gained by water = mcθ R = 300 g 4.2 Jg 1K 1 3 K = 3780 J Heat lost = Heat gained 19

20 200 g c 50 K = 3780 J c = 3780 J gk = Jg 1K 1 8. You are required to make a water bath of 40 kg, at 40 C, by mixing hot water at 100 C and cold water at 15 C. Calculate the ratio of hot and cold water, which should be mixed. Ans. Let the mass of cold water = x. Mass of hot water = (40 kg x). Substance Mass S.H.C Initial temp. Cold water x 4200 Jkg 1 C 1 15 C Hot water 40 kg x 4200 Jkg 1 C C Heat lost by hot water = Heat gained by cold water. mc θf = mc θr. (40 x) = x (40 x) 12 = 5x. 480 = 17x x = Mass of cold water = kg. = kg. Mass of hot water = ( ) = kg. 20 Final temp. = 40 C θr = (40 15) = 25 C θf = (100 40) = 60 C Mass of hot water : Mass of cold water = : = 1 : 2.4.

21 9. Temperature of 600 g cold water rose by 15 C, when 300 g of hot water at 50 C was added to it. What is the initial temp. of cold water? Ans. Substance Mass S.H.C Initial temp. Final temp. =? (x) Cold water Hot water 600 g 300 g 4.2 Jg 1 C Jg 1 C 1? 50 C θr = 15 C θf = (50 C x) Heat lost by hot water = Heat gained by cold water (50 x) = (50 x) = 30 x = 20 C (Final temp.) Initial temp. of water = (Final temp. θr) = (20 15) = 5 C g of hot water at 80 C is added to 400 g of cold water, when the temperature of cold water rises by 18 C. Calculate the initial temperature of cold water. Ans. Proceed as in Q 9. [Ans. 26 C] 21

22 11. Some amount of heat is given out to 120 g of water and its temperature rises by 10 K. When same amount of heat is given to 60 g of oil, its temperature rises by 40 K. The specific heat capacity of water is 4200 Jkg 1 K 1. Calculate : (i) amount of heat in joules given to water. (ii) specific heat capacity of oil. Ans. (i) Heat absorbed by water = mcθr = = 5040 J. (ii) Heat absorbed by water = Heat absorbed by oil 5040 J = 60 g c 40. c = = 2100 Jkg 1K A metal drill of power 500 W, drills a hole in a metal cube of mass 0.25 kg in 6.5s. The specific heat capacity of lead is 130 J kg 1 C 1. (i) How much heat is generated by metal drill in one second? (ii) Calculate the heat generated in 6.5 s. (iii) If t C, is the rise in temperature of metal cube, state the amount of heat energy absorbed by it in terms of t. (iv) Write down an equation and calculate the value of t. 22

23 Ans.(i) Energy generated by drill in 1 s = P t = s = 500 J. (ii) Energy generated by drill in 6.5 s = = 3250 J. (iii) Energy absorbed by metal = mcθr = t = 32.5 t. (iv) Energy absorbed by metal = Energy generated by drill 32.5 t = 3250 t = = 100 C. 13. An electric heater is of power 1000 W. It heats 0.4 kg of water for 2 minutes. The specific heat capacity of water is 4200 J kg 1K 1. (i) How much heat is liberated by heater in 1 s? (ii) How much heat is liberated by heater in 2 minutes? (iii) If θ C, is the rise in temperature of water, state the amount of heat energy absorbed by it, in terms of θ. (iv) Write down an equation and calculate the value of θ. Ans. Proceed as in Q. 12. [Ans. (i) 1000 J; (ii) 120,000 J; (iii) 1680 θ; (iv) C] 14. A copper calorimeter, weighing 57.5 g, contains 60 g of water at 12 C. 55 g of iron nails at 100 C, are dropped into the calorimeter and stirred rapidly. The final temperature attained by the calorimeter and its contents is 20 C. Calculate the specific heat capacity of iron. (Sp. heat capacity of copper is 0.4 Jg 1 C 1 and that of water is 4.2 Jg 1 C 1. 23

24 Ans. Substance Mass S.H.C Initial temp. Final temp. = 20 C Calorimeter 57.5 g 0.4 Jg 1 C 1 12 C θr = (20 12) = 8 C Cold water Iron 60 g 55 g 4.2 Jg 1 C 1? 12 C 100 C θf = (100 20) = 80 C Heat gained by calorimeter = mcθr = = 184 J Heat gained by cold water = mcθr = = 2016 J Heat lost by iron = mcθf = 55 c 80 = 4400 cg C. Heat lost by iron = Heat gained by calorimeter + Heat gained by water cg C = ( ) = 2200 J c = = 0.5 Jg 1 C A molten metal weighing 150 g, is kept at its melting point, at 800 C. When allowed to solidify at the same temperature, it gives off 7500 J of heat energy. What is the specific latent heat of fusion of metal? If its specific heat capacity is 200 Jkg 1 K 1, how much additional heat will it give out in cooling to 50 C? 24

25 Ans. (i) Heat given off by metal during change of state = mass sp. latent heat of metal 7500 J = 150 g sp. latent heat of fusion of the metal. Sp. latent heat of fusion of the metal = = 50 Jg l (ii) Heat given off by metal on cooling = mcθf = [800 ( 50)] J = 25,500 J. 16. A solid weighing 200 g, is kept at its melting point at 0 C. When allowed to melt at the same temperature, it absorbs J of heat energy. Calculate the specific latent heat of fusion of solid. If its specific heat capacity is 4200 Jkg 1K 1, how much additional heat will it absorb in attaining a temperature of 80 C? Ans Proceed as in [Ans. (i) 336 Jg l, (ii) J] 17. One kg of molten lead at its melting point 327 C, is dropped in 1 kg of water at 20 C. Assuming no heat is lost to surroundings, calculate final temperature of water. [Sp. heat capacity of lead and water is 130 Jkg 1 K 1 and 4200 Jkg 1 K 1 respectively. Sp. latent heat of fusion of lead = J kg 1] 25

26 Ans. Substance Mass S.H.C/S.L.H Lead Water 1 kg 1 kg 130 Jkg 1 C 1 /27000 Jkg Jkg 1 C 1 Initial temp. 327 C 20 C Final temp. =? (x) θ R = (x 20 C) θf = (327 C x) Heat lost by lead to change its state = ml = = J. Heat lost by solid lead from 327 C to final temp. = mcθf = (327 x). Heat gained by water = mcθr = (x 20). Heat gained = Heat lost (x 20) = 130 (327 x) x = x x = x = C kg of molten metal at its melting point 420 C, is dropped into 2 kg of water at 25 C. Assuming no heat is lost to surroundings, calculate the final temperature of water.[sp. heat capacity of metal and water are 250 Jkg 1 K 1 and 4200 Jkg 1 K 1 respectively. Sp. latent heat of fusion of metal = Jkg 1] Ans. Proceed as Q : 17 [Ans C] 26

27 19. A block of lead of mass 1 kg at 27 C was heated in a furnace, till it melts completely. Find the quantity of heat required : (i) To bring the lead block to its melting point, (ii) To completely melt the lead block at its melting point. [m.p of lead = 327 C; sp. heat capacity of lead = 130 Jkg 1 K 1 and sp. latent heat of fusion of lead = 26,000 Jkg 1]. Ans.(i) Heat required to bring the lead to its melting point = mcθr = (327 27) = J (ii) Heat required to melt lead = ml = 1 26,000 = 26,000 J. 20. A block of a metal of mass 0.8 kg at 20 C is heated in a furnace, till it completely melts. Find the quantity of heat required : (i) to bring the metal to its melting point, (ii) to completely melt the metal at its melting point [m.p of metal = 420 C; sp. heat capacity of metal 250 Jkg 1 K 1 and sp. latent heat of fusion of metal = Jkg 1] Ans. Proceed as Q : 19 [Ans. (i) 80,000 J, (ii) J] 21. A refrigerator converts 100 g of water at 20 C to ice at 10 C in 73.5 minutes. Calculate the average rate of heat extraction from water in watts. [Specific heat capacity of ice = 2100 Jkg 1 K 1; sp. heat capacity of water is 4200 J kg 1 K 1 and sp. latent heat of fusion of ice is 336,000 Jkg 1]. Ans. Heat lost by water at 20 C to attain temp. of 0 C = mcθf = kg C = 8400 J 27

28 Heat lost by water at 0 C to form ice at 0 C = mlice = kg 336,000 Jkg 1 = J Heat lost by ice to attain temp. of 10 C = mcθf = kg 2100 J 10 C = 2100 J kg. C Total heat lost= ( ) J = 44,100 J 44,100 J Rate of extraction of heat = = 10 Js 1 = 10 W s 22. A cooling machine freezes 1.2 kg of water at 20 C, into ice at 40 C in 12 minutes. Calculate the average rate of extraction of heat energy in watts. [S.H.C of ice = 2100 Jkg 1 K 1, S.H. C of water = 4200 Jkg 1 K 1, S.L.H of ice = Jkg 1] Ans. Proceed as in Q. 21 [Ans. 336 W] 23. An ice cube of mass 30 g, is dropped in 200 g of water at 30 C, such that all the ice melts. Calculate final temperature of water. [Latent heat of ice = 80 cal g 1; Specific heat capacity of water = 1 cal g 1 C 1] Ans. Substance Mass S.H.C/S.L.H Initial temp. Final temp. =? (x) Ice Water 30 g 200 g 80 cal g 1 1 cal g 1 C 1 0 C 30 C θr = (x 0) = x θf = (30 x) 28

29 Heat gained by ice to form water at 0 C = ml = = = 2400 calories Heat gained by water at 0 C to attain temp. x = mcθr = 30 1 x = 30x. Heat lost by water at 30 C = mcθf = (30 x) = x. Heat gained = Heat lost x = x. 230 x = 3600 x = C g of ice cubes are placed in 500 g of water at 40 C, such that all the ice melts. Calculate final temperature of water. [Latent heat of ice = 80 cal g 1; specific heat capacity of water = 1 cal g 1 C 1] Ans. Proceed as in Q. 23 [Ans C] g of ice at 0 C absorbs 5460 J of heat energy to melt and change to water at 50 C. Calculate the specific latent heat of fusion of ice. Specific heat capacity of water is 4200 J kg 1 K 1. Ans.Mass of ice = 10 g. Heat absorbed by ice to form water at 0 C = m Lice = 10 g Lice Rise in temperature (θ R ) = (50 0) = 50 C. Heat absorbed by water at 0 C to attain temp. of 50 C = mcθr = = 2100 J Total heat absorbed by ice = 10 g Lice J 29

30 Also total heat absorbed by ice = 5460 J 10 g Lice J = 5460 J 10 g Lice = ( ) J = 3360 J Lice = 3360 J 10 g = 336 Jg How much heat is released when 5.0 g of water at 20 C changes to ice at 0 C? [Take sp. heat capacity of water = 4.2 J g 1 C 1, specific latent heat of fusion of ice = 336 Jg 1] Ans. Fall in temperature (θ ) f = (20 0) = 20 C. Heat lost by water to attain temp. of 0 C = mcθf = = 420 J Heat lost by water to form ice at 0 C = mlice = = 1680 J Total amount of heat released by water = ( ) J = 2100 J 27. In an experiment, 17 g of ice is used to bring down the temperature of 40 g of water at 34 C to its freezing point. The specific heat capacity of water is 4.2 J kg 1 K 1. Calculate the specific latent heat of ice. State one assumption made in the above calculation. 30

31 Ans. Fall in temperature of water (θ ) f = (34 0) = 34 C Heat lost by water = mcθ f = = 5712 J Heat gained by ice to form water at 0 C = mlice = 17 g Lice. Heat gained by ice = Heat lost by water 17 g Lice = 5712 J Lice = 5712 J 17 g = 336 Jg Find the result of mixing 10 g of ice at 10 C with 10 g of water at 10 C. [sp. heat capacity of ice = 2.1 Jg 1K 1; sp. latent heat of ice = 336 Jg 1 and specific heat capacity of water = 4.2 J g 1 K 1] Ans. Let the amount of ice which melts = x g Heat gained by ice at 10 C to form ice at 0 C = mc θ R = = 210 J Heat gained by ice at 0 C to melt= mlice = x 336 Total heat gained = 210 J + 336x Heat lost by water at 10 C = mc θ R = = 420 J Heat gained = Heat lost 210 J x = 420 J 336x = ( ) = 210 J x = = g Thus, g of ice melts. 31

32 29. What will be the result of mixing 400 g of copper chips at 500 C with 500 g of crushed ice at 0 C. [sp. heat capacity of copper = 0.42 Jg 1K 1 and sp. latent heat of fusion of ice = 340 Jg 1]. Ans. Let the amount of ice which melts = x g Heat absorbed by ice on melting = mlice = x 340 Fall in temperature of copper chips (θ f ) = (500 0) = 500 C Heat given out by copper chips = mcθf = = J Heat absorbed by ice = Heat given out by copper chips x 340 = x = = g Thus, g of ice will melt. 32

### Specific Heat Capacity and Latent Heat Mixed Questions

Specific Heat Capacity and Latent Heat Mixed Questions 1. 12 000 J of heat energy raises the temperature of a 2kg block of a metal from 20 0 C to 30 0 C. What is the specific heat capacity of the metal?

### Temperature Scales. temperature scales Celsius Fahrenheit Kelvin

Ch. 10-11 Concept Ch. 10 #1, 3, 7, 8, 9, 11 Ch11, # 3, 6, 11 Problems Ch10 # 3, 5, 11, 17, 21, 24, 25, 29, 33, 37, 39, 43, 47, 59 Problems: CH 11 # 1, 2, 3a, 4, 5, 6, 9, 13, 15, 22, 25, 27, 28, 35 Temperature

### state and explain how the internal energy and the absolute (kelvin) temperature are related....

6 N08/4/PHYSI/SP2/ENG/TZ0/XX+ A2. This question is about ideal gases. (a) State what is meant by an ideal gas....... For an ideal gas define internal energy. state and explain how the internal energy and

### L A T E N T H E A T O F F U S I O N

Class Date Name Partner(s) L A T E N T H E A T O F F U S I O N Materials LoggerPro Software and Real Time Physics Thermodynamics Experiment Files Stainless Steel Temperature Probes (2) Styrofoam Cup Film

### Instruction Manual and Experiment Guide F. Basic Calorimetry Set TD-8557A

Instruction Manual and Experiment Guide 012-03060F Basic Calorimetry Set TD-8557A Al Cu W Table of Contents Introduction......................................................................... 1 Notes

### Kinetic Molecular Theory. A theory is a collection of ideas that attempts to explain certain phenomena.

Kinetic Molecular Theory A theory is a collection of ideas that attempts to explain certain phenomena. A law is a statement of specific relationships or conditions in nature. After centuries of questioning

### Specific Heat Capacity The use of an equation

CHAPTER 29 Specific Heat Capacity The use of an equation Definition If 1 kg of water and 1 kg of paraffin are heated in turn for the same time by the same heater, the temperature rise of the paraffin is

### Name Date Class THERMOCHEMISTRY. SECTION 17.1 THE FLOW OF ENERGY HEAT AND WORK (pages 505 510)

17 THERMOCHEMISTRY SECTION 17.1 THE FLOW OF ENERGY HEAT AND WORK (pages 505 510) This section explains the relationship between energy and heat, and distinguishes between heat capacity and specific heat.

### Calorimetry - Specific Heat and Latent Heat

Chapter 3 Calorimetry - Specific Heat and Latent Heat Name: Lab Partner: Section: 3.1 Purpose The purpose of this experiment is to study the relationship between heat and temperature. Calorimetry will

### Miscellaneous Heat Problems

Miscellaneous Heat Problems 1. Given that the specific heat capacity of water is eleven times that of copper, calculate the mass of copper at a temperature of 100 C required to raise the temperature of

### Version PREVIEW Heat Chap. 11 sizemore (13756) 1

Version PREVIEW Heat Chap. 11 sizemore (13756) 1 This print-out should have 25 questions. Multiple-choice questions may continue on the next column or page find all choices before answering. Discharge

### Energy Matters Heat. Changes of State

Energy Matters Heat Changes of State Fusion If we supply heat to a lid, such as a piece of copper, the energy supplied is given to the molecules. These start to vibrate more rapidly and with larger vibrations

### PHYSICS 220 LAB #9: CALORIMETRY

Name: Partners: PHYSICS 220 LAB #9: CALORIMETRY If you pour cold cream into a hot cup of coffee, the mixture comes to an intermediate equilibrium temperature. If you put a piece of ice in a glass of water,

### Chapter 17. Quantity of Heat. A PowerPoint Presentation by Paul E. Tippens, Professor of Physics Southern Polytechnic State University

Chapter 17. Quantity of Heat A PowerPoint Presentation by Paul E. Tippens, Professor of Physics Southern Polytechnic State University 2007 Photo Vol. 05 Photodisk/Getty FOUNDRY: It requires about 289 Joules

February 3, 2012 1. Pick up your calculations and your lab sheet. 2. Have your temperature calculations out. 1. The average daytime temperature on Venus is 453 C. What is this temperature in degrees Fahrenheit

### 3.3 Phase Changes Charactaristics of Phase Changes phase change

When at least two states of the same substance are present, scientists describe each different state as a phase. A phase change is the reversible physical change that occurs when a substance changes from

### Energy in Thermal Processes: The First Law of Thermodynamics

Energy in Thermal Processes: The First Law of Thermodynamics 1. An insulated container half full of room temperature water is shaken vigorously for two minutes. What happens to the temperature of the water?

### UNIT 6a TEST REVIEW. 1. A weather instrument is shown below.

UNIT 6a TEST REVIEW 1. A weather instrument is shown below. Which weather variable is measured by this instrument? 1) wind speed 3) cloud cover 2) precipitation 4) air pressure 2. Which weather station

### Heat Transfer. Thermal energy

Thermal energy Heat Transfer Thermal energy is the total kinetic energy of the molecules of a substance. It is the energy needed to raise the temperature of a substance to its actual temperature from absolute

### Chapter 18 Temperature, Heat, and the First Law of Thermodynamics. Problems: 8, 11, 13, 17, 21, 27, 29, 37, 39, 41, 47, 51, 57

Chapter 18 Temperature, Heat, and the First Law of Thermodynamics Problems: 8, 11, 13, 17, 21, 27, 29, 37, 39, 41, 47, 51, 57 Thermodynamics study and application of thermal energy temperature quantity

### Chapter 4: Transfer of Thermal Energy

Chapter 4: Transfer of Thermal Energy Goals of Period 4 Section 4.1: To define temperature and thermal energy Section 4.2: To discuss three methods of thermal energy transfer. Section 4.3: To describe

### FXA 2008. Candidates should be able to : Define and apply the concept of specific heat capacity. Select and apply the equation : E = mcδθ

UNIT G484 Module 3 4.3.3 Thermal Properties of Materials 1 Candidates should be able to : Define and apply the concept of specific heat capacity. Select and apply the equation : E = mcδθ The MASS (m) of

### Chemistry 51 Chapter 2 ENERGY & HEAT

ENERGY & HEAT Energy is defined as the capacity of matter to do work. There are two types of energy: 1. Potential (stored) 2. Kinetic (moving) Energy possesses many forms (chemical, electrical, thermal,

### Procedure. Day 1 - Calibration of the Calorimeter. (Part I) The Heat Capacity of the Calorimeter.

Thermochemistry Experiment 10 Thermochemistry is the study of the heat energy involved in chemical reactions and changes of physical state. Heat energy is always spontaneously transferred from hotter to

### Lead/Tin Solder Lab. 1. Select a labeled cup(s) and sign your names on the table of lead/tin percentages.

Lead/Tin Solder Lab 1. Select a labeled cup(s) and sign your names on the table of lead/tin percentages. 2. Mass out 50 grams total of your assigned lead and tin alloy. 3. Melt the metals together in an

### Chapter 10: Temperature and Heat

Chapter 10: Temperature and Heat 1. The temperature of a substance is A. proportional to the average kinetic energy of the molecules in a substance. B. equal to the kinetic energy of the fastest moving

### 1. Have your Specific Heat Lab/Calculations out from FRIDAY. 1. Review Energy test corrections due by Friday.

February 6, 2012 1. Have your Specific Heat Lab/Calculations out from FRIDAY. 2. YOU NEED YOUR BOOK! Agenda: 1. Review Energy test corrections due by Friday. 2. Review Specific Heat check calculations,

### Physics 101: Lecture 25 Heat

Final Physics 101: Lecture 25 Heat Today s lecture will cover Textbook Chapter 14.1-14.5 Physics 101: Lecture 25, Pg 1 Internal Energy Energy of all molecules including Random motion of individual molecules»

### Chapter 10 Study Questions

Chapter 10 Study Questions Multiple Choice Identify the letter of the choice that best completes the statement or answers the question. 1. Which of the following temperatures is the lowest? a. 100ºC c.

### Chapter 16 Temperature and Heat

The determination of temperature has long been recognized as a problem of the greatest importance in physical science. It has accordingly been made a subject of most careful attention, and, especially

### Chapter 10 Temperature and Heat

Chapter 10 Temperature and Heat What are temperature and heat? Are they the same? What causes heat? What Is Temperature? How do we measure temperature? What are we actually measuring? Temperature and Its

### HNRS 227 Fall 2008 Chapter 4. Do You Remember These? iclicker Question. iclicker Question. iclicker Question. iclicker Question

HNRS 227 Fall 2008 Chapter 4 Heat and Temperature presented by Prof. Geller Do You Remember These? Units of length, mass and time, and metric Prefixes Density and its units The Scientific Method Speed,

### Latent Heat Calculations

Latent Heat Calculations What heat quantities are needed to change a substance from a liquid to a gas? How much energy is needed to melt a solid to a liquid? Is it the same for each substance? Let s look

### Final Exam. Wednesday, December 10. 1:30 4:30 pm. University Centre Rooms

16.102 Final Exam Wednesday, December 10 1:30 4:30 pm University Centre Rooms 210 224 30 questions, multiple choice The whole course, equal weighting Formula sheet provided 26 Lab and Tutorial Marks Final

### Energy. Work. Potential Energy. Kinetic Energy. Learning Check 2.1. Energy. Energy. makes objects move. makes things stop. is needed to do work.

Chapter 2 Energy and Matter Energy 2.1 Energy Energy makes objects move. makes things stop. is needed to do work. 1 2 Work Potential Energy Work is done when you climb. you lift a bag of groceries. you

### Use tongs and wear goggles when removing the samples from the pot of boiling water. Protect your eyes against accidental splashes!

Calorimetry Lab Purpose: Students will measure latent heat and specific heat. PLEASE READ the entire handout before starting. You won t know what to do unless you understand how it works! Introduction:

### PARADISE VALLEY COMMUNITY COLLEGE PHYSICS 101 - INTRODUCTION TO PHYSICS LABORATORY. Calorimetry

PARADISE VALLEY COMMUNITY COLLEGE PHYSICS 101 - INTRODUCTION TO PHYSICS LABORATORY Calorimetry Equipment Needed: Large styrofoam cup, thermometer, hot water, cold water, ice, beaker, graduated cylinder,

### Energy Changes in Chemical Reactions. System loses heat (negative); gains heat (positive) Describe the difference between the two.

Energy Changes in Chemical Reactions Most reactions give off or absorb energy Energy is the capacity to do work or supply heat. Heat: transfer of thermal (kinetic) energy between two systems at different

### thermo practice test

Name: ate: 1. If only the respective tempreatures of two objects are known, what additional information can be determined?. how much heat the objects contain 3. ase your answer(s) to the following question(s)

### PHYS 1020 Final Exam. Seating (from exam listing on Aurora) Brown Gym. Gold Gym

PHYS 1020 Final Exam Monday, December 17, 6-9 pm The whole course 30 multiple choice questions Formula sheet provided Seating (from exam listing on Aurora) Brown Gym A - SIM Gold Gym SIN - Z 27 Week of

### Specific Heat Capacity

Specific Heat Capacity Specific Heat Capacity The amount of energy it takes to heat up 1 gram of a substance by 1 C What heats up faster, metal or water? Calorie Energy changes can also be measured in

### Calculating Work. Thermodynamics. Isobaric Process. Isochoric (isovolumetric) Work from Graph: Example 1 2/27/2012. Chapter 15

Pressure (X105 N/m2) Pressure (X105 N/m2) 2/27/2012 Thermodynamics Chapter 15 Calculating Work Work = area under Pressure vs. Volume graph W = Fd F = PA W=PAd W = P V Calculus link V 2 W = - p dv V 1 Isochoric

### Physics Notes Class 11 CHAPTER 11 THERMAL PROPERTIES OF MATTER

1 P a g e Physics Notes Class 11 CHAPTER 11 THERMAL PROPERTIES OF MATTER The branch dealing with measurement of temperature is called thremometry and the devices used to measure temperature are called

### 1 Btu = kcal = 1055 J.

Heat Problems. How much heat in joules) is required to raise the temperature of 30.0 kg of water from C to 9 C?. To what temperature will 7700 J of heat raise 3.0 kg of water that is initially at 0.0 C?

### Copper, Zinc and Brass (an alloy of Cu and Zn) have very similar specific heat capacities. Why should this be so?

Thermal Properties 1. Specific Heat Capacity The heat capacity or thermal capacity of a body is a measure of how much thermal energy is required to raise its temperature by 1K (1 C). This will depend on

### Specific Heats of Metals

Johnson 1 Cameron Johnson Jun Li Physics 222 March 6, 2013 Specific Heats of Metals Abstract The purpose of this lab is to determine the specific heat of various types of metals by adding a known amount

### Chemistry Thermochemistry Lesson 10 Lesson Plan David V. Fansler

Chemistry Thermochemistry Lesson 10 Lesson Plan David V. Fansler The Flow of Energy-Heat Objectives: Explain the relationship between energy and heat; Distinguish between heat capacity and specific heat.

### 2. Room temperature: C. Kelvin. 2. Room temperature:

Temperature I. Temperature is the quantity that tells how hot or cold something is compared with a standard A. Temperature is directly proportional to the average kinetic energy of molecular translational

### Experiment 4-Heat of Fusion and Melting Ice Experiment

Experiment 4-Heat of Fusion and Melting Ice Experiment In this lab, the heat of fusion for water will be determined by monitoring the temperature changes while a known mass of ice melts in a cup of water.

### Level 1 Physics, 2011

90939 909390 1SUPERVISOR S Level 1 Physics, 2011 90939 Demonstrate understanding of aspects of heat 2.00 pm hursday Thursday 2 November 2011 Credits: Four Achievement Achievement with Merit Achievement

### Temperature & Heat. Overview

Temperature & Heat Overview Temperature vs Heat What is temperature (degrees)? A measure of the average kinetic energy of the particles in an object What is heat (joules)? That energy transferred between

### SPECIFIC HEAT. Roster Number: Pre-Lab Questions Page Instructor: 2. Define specific heat, water equivalent and heat capacity of a body.

SPECIFIC HEAT Name: Class: Roster Number: Pre-Lab Questions Page Instructor: 1. List the symbol and at least two units for specific heat.,, 2. Define specific heat, water equivalent and heat capacity of

### Calorimetry Lab - Specific Heat Capacity

Introduction Calorimetry Lab - Specific Heat Capacity Experience tells us that if a hot piece of metal is added to water, the temperature of the water will rise. If several different metals having the

### Specific Heat Capacity and Latent Heat Questions A2 Physics

1. An electrical heater is used to heat a 1.0 kg block of metal, which is well lagged. The table shows how the temperature of the block increased with time. temp/ C 20.1 23.0 26.9 30.0 33.1 36.9 time/s

### Calorimetry: Determining the Heat of Fusion of Ice and the Heat of Vaporization of Liquid Nitrogen - Chemistry I Acc

Calorimetry: Determining the Heat of Fusion of Ice and the Heat of Vaporization of Liquid Nitrogen - Chemistry I Acc O B J E C T I V E 1. Using a simple calorimeter, Determine the heat of fusion of ice

### Physics 142: Lecture 10 Today s Agenda. Review: Specific Heat. Review: Units of Heat. Review: Internal Energy of Ideal Gas

Physics 142: Lecture 10 Today s Agenda Heat: Phase Change and Latent Heat Heat Transfer (time permitting) Examples Suggested problems for CH11: 23, 46, 49, 0, 1, 78 Review: Internal Energy of Ideal Gas

### Unit 2 Lesson 3 Thermal Energy and Heat Essential Question: What is the relationship between heat and temperature?

Big Idea: Energy exits in different forms and can change from one form to another, but energy is always conserved. Unit 2 Lesson 3 Thermal Energy and Heat Essential Question: What is the relationship between

### Name: Class: Date: 10. Some substances, when exposed to visible light, absorb more energy as heat than other substances absorb.

Name: Class: Date: ID: A PS Chapter 13 Review Modified True/False Indicate whether the statement is true or false. If false, change the identified word or phrase to make the statement true. 1. In all cooling

### Built to specifications:

Experiment: Heat of Fusion (H f ) for Water Minneapolis Community and Technical College v.5.10 I. Introduction The heat of fusion (H f ) is the amount of energy required to melt or freeze a substance and

### Heat and Temperature. Temperature Scales. Thermometers and Temperature Scales

Heat and Temperature Thermometers and Temperature Scales The mercury-based one you see here relies on the fact that mercury expands at a predictable rate with temperature. The scale of the thermometer

### Chapter 4 Practice Quiz

Chapter 4 Practice Quiz 1. Label each box with the appropriate state of matter. A) I: Gas II: Liquid III: Solid B) I: Liquid II: Solid III: Gas C) I: Solid II: Liquid III: Gas D) I: Gas II: Solid III:

### Heat Capacity. A formula can be used to find the energy needed to heat 1g of a specific substance by 1 C. E = mc T

Heat Capacity Heat Capacity- the amount of heat required to raise the temperature of an object by 1 C. This definition applies only to objects that are made of a mixture of several substances. Pure substances,

### Name Chemistry / / Melting/Freezing/Boiling & Condensing

Name Chemistry / / Melting/Freezing/Boiling & Condensing As a substance melts, freezes, boils or condenses, heat is either absorbed or released. But, as this change in state occurs, there is no change

### Phys222 W11 Quiz 1: Chapters 19-21 Keys. Name:

Name:. In order for two objects to have the same temperature, they must a. be in thermal equilibrium.

### Page 1. Name:

Name: 1) Which process requires the addition of energy to water? A) vaporization of water B) condensation of water C) freezing of water D) cooling of water 2) According to the Earth Science Reference Tables,

### Chapter 21: Temperature, Heat & Expansion. Review from the Video:

Chapter 21: Temperature, Heat & Expansion Review from the Video: Temperature is the average kinetic energy of one molecule Heat is energy in motion (flows from hot to cold) Thermal energy is the total

### 3 Thermal physics ESSENTIAL IDEAS. Molecular theory of solids, liquids and gases

3 Thermal physics ESSENTIAL IDEAS Thermal physics deftly demonstrates the links between the macroscopic measurements essential to many scientific models with the microscopic properties that underlie these

### Type: Single Date: Homework: READ 12.8, Do CONCEPT Q. # (14) Do PROBLEMS (40, 52, 81) Ch. 12

Type: Single Date: Objective: Latent Heat Homework: READ 12.8, Do CONCEPT Q. # (14) Do PROBLEMS (40, 52, 81) Ch. 12 AP Physics B Date: Mr. Mirro Heat and Phase Change When bodies are heated or cooled their

### HW#13a Note: numbers used in solution steps are different from your WebAssign values. Page 1 of 6

Note: numbers used in solution steps are different from your WebAssign values. Page 1 of 6 1. Walker3 16.P.006. One day you notice that the outside temperature increased by 24 F between your early morning

### HEAT OF FUSION MECHANICAL EQUIVALENT OF HEAT AND PART A. HEAT OF FUSION

HEAT OF FUSION AND MECHANICAL EQUIVALENT OF HEAT CAUTION: Please handle thermometers gently. Broken mercury-filled thermometers should be taken to Rm. B-31 for disposal as mercury is very toxic. If a red-liquid

### Chemistry Energy Worksheet

Chemistry Energy Worksheet Answer Key Energy Storage & Transfer Mechanisms 1. Indicate how most of the energy is stored in each of the objects. Energy is often stored in most of the six mechanism, but

### Heats of Transition, Heats of Reaction, Specific Heats, and Hess s Law

Heats of Transition, Heats of Reaction, Specific Heats, and Hess s Law GOAL AND OVERVIEW A simple calorimeter will be made and calibrated. It will be used to determine the heat of fusion of ice, the specific

### PHYSICS EXPERIMENTS (HEAT)

PHYSICS EXPERIMENTS (HEAT) In the matter of physics, the first lessons should contain nothing but what is experimental and interesting to see. A pretty experiment is in itself often more valuable than

### 20 Specific Heat of an Unknown Metal

Lab Activity 20 SPECIFIC HEAT OF AN UNKNOWN METAL LAB ACTIVITY 20 Specific Heat of an Unknown Metal Purpose Measure the specific heat of a metal object and identity the metal based on its specific heat.

### Electricity and Energy

Lesmahagow High School National 5 Physics Electricity and Energy Summary Notes Throughout the Course, appropriate attention should be given to units, prefixes and scientific notation. tera T 10 12 x 1,000,000,000,000

### Temperature and Heat. Chapter 17. PowerPoint Lectures for University Physics, Twelfth Edition Hugh D. Young and Roger A. Freedman

Chapter 17 Temperature and Heat PowerPoint Lectures for University Physics, Twelfth Edition Hugh D. Young and Roger A. Freedman Lectures by James Pazun Modified by P. Lam 6_17_2012 Topics for Chapter 17

### Chapter 15 Temperature, Heat, and Expansion

Chapter 15 Temperature, Heat, and Expansion Although the temperature of these sparks exceeds 2000ºC, the heat they impart when striking my skin is very small. Temperature and heat are different concepts.

### THERMOCHEMISTRY & DEFINITIONS

THERMOCHEMISTRY & DEFINITIONS Thermochemistry is the study of the study of relationships between chemistry and energy. All chemical changes and many physical changes involve exchange of energy with the

### Electrical Equivalent of Heat Apparatus

Name Class Date Electrical Equivalent of Heat Equipment Needed Temperature Sensor Current Sensor Voltage Sensor Electrical Equivalent of Heat Apparatus Balance Digital Multimeter Low Voltage Power Supply

### Q = mc T f T i ) Q = mc T)

Problem Solving with Heat Heat is quite a complex concept. Heat can be effected by how much of the substance there is, what temperature the substance is at, and what the substance is. We need a unit define

### Temperature. Temperature

Chapter 8 Temperature Temperature a number that corresponds to the warmth or coldness of an object measured by a thermometer is a per-particle property no upper limit definite limit on lower end Temperature

### Test 5 Review questions. 1. As ice cools from 273 K to 263 K, the average kinetic energy of its molecules will

Name: Thursday, December 13, 2007 Test 5 Review questions 1. As ice cools from 273 K to 263 K, the average kinetic energy of its molecules will 1. decrease 2. increase 3. remain the same 2. The graph below

### q = (mass) x (specific heat) x T = m c T (1)

Experiment: Heat Effects and Calorimetry Heat is a form of energy, sometimes called thermal energy, which can pass spontaneously from an object at a high temperature to an object at a lower temperature.

### Thermodynamics is the study of heat. It s what comes into play when you drop an ice cube

Chapter 12 You re Getting Warm: Thermodynamics In This Chapter Converting between temperature scales Working with linear expansion Calculating volume expansion Using heat capacities Understanding latent

### Specific Heat Capacity & Calorimetry

Unit: Thermal Physics Knowledge/Understanding: specific heat capacity calorimetry Skills: solve calorimetry (specific heat) problems Notes: Different objects have different abilities to hold heat. For

### Exam 4 -- PHYS 101. Name: Class: Date: Multiple Choice Identify the choice that best completes the statement or answers the question.

Name: Class: Date: Exam 4 -- PHYS 101 Multiple Choice Identify the choice that best completes the statement or answers the question. 1. A steel tape measure is marked such that it gives accurate measurements

### Heat evolved by the reaction = Heat absorbed by the water + Heat absorbed by the bomb

ENERGY OF A PEANUT AN EXPERIMENT IN CALORIMETRY 2011, 2010, 2002, 1995, by David A. Katz. All rights reserved. Reproduction permitted for educational use provided original copyright is included. INTRODUCTION:

### Topic Page Contents Page

Heat energy (11-16) Contents Topic Page Contents Page Heat energy and temperature 3 Latent heat energy 15 Interesting temperatures 4 Conduction of heat energy 16 A cooling curve 5 Convection 17 Expansion

### Temperature and Heat

Temperature and Heat Foundation Physics Lecture 2.4 26 Jan 10 Temperature, Internal Energy and Heat What is temperature? What is heat? What is internal energy? Temperature Does a glass of water sitting

### Temperature and. Chapter 5: Temperature and Heat. Thermometer. Bimetallic Strip and Thermal Expansion. Temperature Scales Celsius, Kelvin, Fahrenheit

Temperature Chapter 5 Chapter 5: Temperature and Heat Temperature and Homework: All questions Heat on the Multiple- Choice and the odd-numbered questions on Exercises sections at the end of the chapter.

### Chapter 10 Temperature and Heat

Chapter 10 Temperature and Heat GOALS When you have mastered the contents of this chapter, you will be able to achieve the following goals: Definitions Define each of the following terms, and use it an

### Problem Set 9 Due: see website for due date Chapter 12: Thermal Properties of Matter Q12.1: Solution Q12.4. Reason: Q12.20: Solution Q12.20.

Problem Set 9 Due: see website for due date Chapter 1: Thermal Properties of Matter Questions: 4, 0, 1, 5 Exercises & Problems: 9, 16, 5, 54, 57, 6, 80, 8, 98 Q1.1: If you buy a sealed bag of potato chips

### Specific Heat (Temperature Sensor)

43 Specific Heat (Temperature Sensor) Thermodynamics: Calorimetry; specific heat Equipment List DataStudio file: 43 Specific Heat.ds Qty Items Part Numbers 1 PASCO Interface (for one sensor) 1 Temperature

### The specific heat capacity of a material is defined as the energy needed to raise the temperature of 1 kg of the material by 1 o C.

High Demand Questions QUESTIONSHEET 1 The specific heat capacity of a material is defined as the energy needed to raise the temperature of 1 kg of the material by 1 o C. material iron aluminium copper

### Evaporation. Evaporation. Boiling. Saturation curve. Enthalpy. Steam tables and how to read them

dwells on the fundamental constituents of the universe, the forces they exert on one another, and the results produced by these forces. Here, we understand water molecules, what happens when they are heated,

### IB PHYSICS HL REVIEW PACKET: THERMODYNAMICS (2) (3)

NAME IB PHYSICS HL REVIEW PACKET: THERMODYNAMICS 1. This question is about gases and specific heat capacity. (a) State what is meant by an ideal gas.......... An ideal gas occupies a volume of 1.2 m 3

### Second Law of Thermodynamics

Thermodynamics T8 Second Law of Thermodynamics Learning Goal: To understand the implications of the second law of thermodynamics. The second law of thermodynamics explains the direction in which the thermodynamic

Adca Training Part 1 This presentation is only a guideline, that can only be completed by a trained personnel. (This document s total or partial use and/or reproduction is only allowed if the reference