The transfer of heat could be due to a physical change or a chemical change. There are three laws of chemical thermodynamics.
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1 Thermodynamics The transfer of heat could be due to a physical change or a chemical change. There are three laws of chemical thermodynamics.
2 What is the difference between a scientific law and theory? The first law of thermodynamics: Energy and matter can be neither created nor destroyed; only transformed from one form to another. The energy and matter of the universe is constant. The second law of thermodynamics: In any spontaneous process there is always an increase in the entropy of the universe. The entropy is increasing. The third law of thermodynamics: The entropy of a perfect crystal at 0 K is zero. There is no molecular motion at absolute 0 K.
3 The energy that flows into or out of a system because of a difference in temperature between the thermodynamic system and its surrounding. Symbolized by "q". When heat is evolved by a system, energy is lost and "q is negative (- ). When heat is absorbed by the system, the energy is added and "q" is positive (+).
4 Heat can flow in one of two directions: Exothermic To give off heat; energy is lost from the system: (- q) Endothermic To absorb heat; energy is added to the system: (+q)
5 If the heat transfer involves a chemical reaction then q is called: The heat energy (ΔH; enthalpy) required to return a system to the given temperature at the completion of the reaction. q = ΔH at constant pressure The heat of reaction can be specific to a reaction like: HEAT OF COMBUSTION The quantity of heat energy given off when a specified amount of substance burns in oxygen.
6 SPECIFIC HEAT: The quantity of heat required to raise the temperature of one gram of a substance by one degree Celsius (or one Kelvin). q = C p x m x ΔT
7 Heat energy is usually measured in either Joules, given by the unit (J), and kilojoules (kj) or in calories, written shorthand as (cal), and kilocalories (kcal). Food Calories are noted with a capital C, Calorie (Cal). 1 cal = J 1 Cal = 1,000 cal NOTE: This conversion correlates to the specific heat of water which is 1 cal/g o C or J/g o C.
8 Determine the energy (in kj) required to raise the temperature of g of water from 20.0 o C to 85.0 o C? m = g q = m x Cp x ΔT ΔT = T f - T i = o C = 65.0 o C Cp (H 2 O) = J/ g - o C q = (100.0 g) x (4.184 J/g- o C) x (65.0 o C) q = J (1 kj / 1000J) = 27.2 kj Determine the specific heat of an unknown metal that required 2.56 kcal of heat to raise the temperature of g from 15.0 o C to o C?
9 Determine the energy (in kj) required to raise the temperature of g of water from 20.0 o C to 85.0 o C? m = g q = m x Cp x ΔT ΔT = T f - T i = o C = 65.0 o C Cp (H 2 O) = J/ g - o C q = (100.0 g) x (4.184 J/g- o C) x (65.0 o C) q = J (1 kj / 1000J) = 27.2 kj Determine the specific heat of an unknown metal that required 2.56 kcal of heat to raise the temperature of g from 15.0 o C to o C? Cp = 92.3 kcal /g - o C
10 The law of conservation of energy (the first law of thermodynamics), when related to heat transfer between two objects, can be stated as: The heat lost by the hot object = the heat gained by the cold object - q hot = q cold
11 Assuming no heat is lost, what mass of cold water at 0.00 o C is needed to cool g of water at 97.6 o C to 12.0 o C? - m h x Cp h x ΔT h = m c x Cp c x ΔT c - [(100.0g) (1 cal/g o C) ( o C)] = m (1 cal/g o C) ( o C) 8560 cal = m (12.0 cal/g) m = 8560 cal / (12.0 cal/g) m = 713 g
12 PRACTICE PROBLEMS 1. Iron metal has a specific heat of J/g o C. How much heat is transferred to a 5.00 g piece of iron, initially at 20.0 o C, when it is placed in a beaker of boiling water at 1 atm? 2. How many calories of energy are given off to lower the temperature of g of iron from o C to 35.0 o C? 3. If 3.47 kj were absorbed by 75.0 g H 2 O at 20.0 o C, what would be the final temperature of the water? 4. A 100. g sample of water at 25.3 o C was placed in a calorimeter g of lead shots (at 100 o C) was added to the calorimeter and the final temperature of the mixture was 34.4 o C. What is the specific heat of lead? 5. A 17.9 g sample of unknown metal was heated to o C. It was then added to g of water in an insulted cup. The water temperature rose from o C to o C. What is the specific heat of the metal in J/g o C?
13 PRACTICE PROBLEMS 1. Iron metal has a specific heat of J/g o C. How much heat is transferred to a 5.00 g piece of iron, initially at 20.0 o C, when it is placed in a beaker of boiling water at 1 atm? 180. J 2. How many calories of energy are given off to lower the temperature of g of iron from o C to 35.0 o C? 3. If 3.47 kj were absorbed by 75.0 g H 2 O at 20.0 o C, what would be the final temperature of the water? 4. A 100. g sample of water at 25.3 o C was placed in a calorimeter g of lead shots (at 100 o C) was added to the calorimeter and the final temperature of the mixture was 34.4 o C. What is the specific heat of lead? 5. A 17.9 g sample of unknown metal was heated to o C. It was then added to g of water in an insulted cup. The water temperature rose from o C to o C. What is the specific heat of the metal in J/g o C?
14 PRACTICE PROBLEMS 1. Iron metal has a specific heat of J/g o C. How much heat is transferred to a 5.00 g piece of iron, initially at 20.0 o C, when it is placed in a beaker of boiling water at 1 atm? 180. J 2. How many calories of energy are given off to lower the temperature of g of iron from o C to 35.0 o C? 3. If 3.47 kj were absorbed by 75.0 g H 2 O at 20.0 o C, what would be the final temperature of the water? 1.23 x 10 3 cal 4. A 100. g sample of water at 25.3 o C was placed in a calorimeter g of lead shots (at 100 o C) was added to the calorimeter and the final temperature of the mixture was 34.4 o C. What is the specific heat of lead? 5. A 17.9 g sample of unknown metal was heated to o C. It was then added to g of water in an insulted cup. The water temperature rose from o C to o C. What is the specific heat of the metal in J/g o C?
15 PRACTICE PROBLEMS 1. Iron metal has a specific heat of J/g o C. How much heat is transferred to a 5.00 g piece of iron, initially at 20.0 o C, when it is placed in a beaker of boiling water at 1 atm? 180. J 2. How many calories of energy are given off to lower the temperature of g of iron from o C to 35.0 o C? 3. If 3.47 kj were absorbed by 75.0 g H 2 O at 20.0 o C, what would be the final temperature of the water? 1.23 x 10 3 cal 31.1 o C 4. A 100. g sample of water at 25.3 o C was placed in a calorimeter g of lead shots (at 100 o C) was added to the calorimeter and the final temperature of the mixture was 34.4 o C. What is the specific heat of lead? 5. A 17.9 g sample of unknown metal was heated to o C. It was then added to g of water in an insulted cup. The water temperature rose from o C to o C. What is the specific heat of the metal in J/g o C?
16 PRACTICE PROBLEMS 1. Iron metal has a specific heat of J/g o C. How much heat is transferred to a 5.00 g piece of iron, initially at 20.0 o C, when it is placed in a beaker of boiling water at 1 atm? 180. J 2. How many calories of energy are given off to lower the temperature of g of iron from o C to 35.0 o C? 3. If 3.47 kj were absorbed by 75.0 g H 2 O at 20.0 o C, what would be the final temperature of the water? 1.23 x 10 3 cal 31.1 o C 4. A 100. g sample of water at 25.3 o C was placed in a calorimeter g of lead shots (at 100 o C) was added to the calorimeter and the final temperature of the mixture was 34.4 o C. What is the specific heat of lead? 1.28 J/g o C 5. A 17.9 g sample of unknown metal was heated to o C. It was then added to g of water in an insulted cup. The water temperature rose from o C to o C. What is the specific heat of the metal in J/g o C?
17 PRACTICE PROBLEMS 1. Iron metal has a specific heat of J/g o C. How much heat is transferred to a 5.00 g piece of iron, initially at 20.0 o C, when it is placed in a beaker of boiling water at 1 atm? 180. J 2. How many calories of energy are given off to lower the temperature of g of iron from o C to 35.0 o C? 3. If 3.47 kj were absorbed by 75.0 g H 2 O at 20.0 o C, what would be the final temperature of the water? 1.23 x 10 3 cal 31.1 o C 4. A 100. g sample of water at 25.3 o C was placed in a calorimeter g of lead shots (at 100 o C) was added to the calorimeter and the final temperature of the mixture was 34.4 o C. What is the specific heat of lead? 1.28 J/g o C 5. A 17.9 g sample of unknown metal was heated to o C. It was then added to g of water in an insulted cup. The water temperature rose from o C to o C. What is the specific heat of the metal in J/g o C? J/g o C
18 GROUP STUDY PROBLEMS 1. A g metal bar requires kj to change its temperature from 22.0 o C to o C. What is the specific heat of the metal in J/g o C? 2. How many joules are required to lower the temperature of g of iron from 75.0 o C to 25.0 o C? 3. If 40.0 kj were absorbed by g H 2 O at 10.0 o C, what would be the final temperature of the water? 4. A 250 g of water at o C is mixed with ml of water at 5.0 o C. Calculate the final temperature of the mixture. 5. A 400 g piece of gold at o C is dropped into 15.0 L of water at 22.0 o C. The specific heat of gold is J/g o C or cal/ g o C. Calculate the final temperature of the mixture assuming no heat is lost to the surroundings.
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