# ... (1) State one way in which she could increase the rate of reaction.... (1)

Save this PDF as:

Size: px
Start display at page:

Download "... (1) State one way in which she could increase the rate of reaction.... (1)"

## Transcription

1 Q1. A student does an experiment to examine the rate of reaction between magnesium and dilute hydrochloric acid. She adds 25 cm³ of the acid to a weighed amount of the metal. The reaction produces hydrogen gas. Magnesium + hydrochloric acid magnesium + hydrogen chloride She collects the gas and measures the volume collected at one minute intervals. All the metal reacted but there was some acid left unreacted. Her results are shown on the graph. (a) The diagram shows part of the apparatus she used for the experiment. Complete the diagram to show how the student could collect the hydrogen produced and measure the volume after each minute. Page 1 of 50

2 (b) (i) When is the rate of reaction at its fastest? State one way in which she could increase the rate of reaction. (c) (i) What is the total volume of hydrogen collected in the experiment?... cm³ State one way in which she could increase the final volume of hydrogen collected. (Total 6 marks) Q2. Marble chips (calcium carbonate) react with dilute hydrochloric acid. calcium + hydrochloric calcium + carbon + water carbonate acid chloride dioxide A student wanted to find out if the size of the marble chips made a difference to how fast the reaction took place. (a) What readings should she take? Page 2 of 50

3 (b) She repeated the experiment but this time used the same mass (10g) of large marble chips. In both experiments there was some marble left in the flask when the reaction stopped. These are the results of the two experiments. TIME (minutes) Loss in mass (g), using small chips Loss in mass (g), using large chips (i) Explain the loss in mass in the two experiments. What difference does the size of the chips make? (c) A chemical reaction occurs when reacting particles collide with sufficient energy. The reaction between marble and hydrochloric acid is faster if the acid is at a higher temperature. Explain why. (3) (Total 7 marks) Q3. Some students were investigating how fast hydrogen gas is released in the reaction between magnesium and dilute hydrochloric acid. To begin with they used 0.1 g of magnesium ribbon. Next, they repeated the experiment using 0.1 g of magnesium powder. In each case, they used enough acid to react with all the metal. Page 3 of 50

4 (a) Their results are shown on the graph below. Hydrogen is produced in both the reactions. Use the information on the graph to describe two other ways in which the two reactions are similar (b) Describe one way in which the reactions are different. (Total 3 marks) Page 4 of 50

5 Q4. The diagram represents the particles in a piece of reactive metal. The piece of reactive metal is added to dilute hydrochloric acid. (a) (i) Which particle will probably react first? Choose from: a particle inside the piece; a particle at the centre of a face; a particle on one of the corners. Explain the reason for your choice. (b) The reaction can be speeded up by making changes to the hydrochloric acid or the solid. (i) State two ways to speed up the reaction by changing the hydrochloric acid. In each case explain in terms of particles why the reaction is faster Page 5 of 50

6 Zn + HCl ZnC1 2 + H 2 What change can you make to the piece of solid to speed up the reaction? Explain in terms of the particles why the reaction is able to speed up. (Total 8 marks) Q5. The graph shows the volume of gas given off during an experiment using hydrogen peroxide solution and manganese oxide. Draw, on the axes above, a graph to show the result you would expect if the volume of hydrogen peroxide solution had been the same, but it was twice as concentrated. (Total 3 marks) Q6. Zinc powder normally reacts slowly with hydrochloric acid. (a) Balance the symbol equation for the reaction. Page 6 of 50

7 The graph shows the results from a reaction of 1.0 g of zinc powder with 20 cm 3 of dilute hydrochloric acid. It gives off a gas and forms zinc chloride, ZnCl 2. Some unreacted zinc is left at the end. (b) Copper powder is a good catalyst for the reaction of zinc with hydrochloric acid. (i) A mixture of 10 cm 3 of the same dilute hydrochloric acid and 1.0 g of copper powder was added to 1.0 g of zinc powder. What is the maximum volume of gas which could be given off?... cm 3 (iii) Draw a graph, on the axes above, for an experiment where 20 cm 3 of the same dilute hydrochloric acid was added to 1.0 g of copper powder mixed with 1.0 g of zinc powder. Give two other ways the reaction described in part (i) could be made to go faster (c) Copper powder can be formed by adding copper sulphate solution to the mixture of zinc powder and acid. (i) Why does zinc react with copper sulphate solution to produce copper? Page 7 of 50

8 Write the word equation for the reaction. (Total 8 marks) Q7. Many indigestion tablets contain calcium carbonate as their only active ingredient. Calcium carbonate neutralises some of the hydrochloric acid in the stomach. Two different indigestion tablets, X and Y, were separately reacted with excess hydrochloric acid. The volume of gas given off in each reaction was measured every minute. The results are shown in the graph. (i) Which tablet, X or Y, contained most calcium carbonate?... Explain the reason for your answer. Which tablet, X or Y, reacted faster with hydrochloric acid?... Explain the reason for your answer. Page 8 of 50

9 (iii) Explain the shape of the graph for tablet X between 3 and 5 minutes. (Total 3 marks) Q8. The flow diagram shows how to make ammonia and nitric acid from the nitrogen in the air. (a) A fertiliser is made by neutralising ammonia with nitric acid. What is the name of this fertiliser? (b) In the flow diagram, why are two different catalysts used? Page 9 of 50

10 (c) What happens to catalysts at the end of a reaction? (d) Explain why catalysts are used in many industrial chemical reactions. (e) Explain, in terms of collisions between molecules, why a high pressure is used in the reaction between nitrogen and hydrogen. (Total 7 marks) Q9. Hydrogen peroxide slowly decomposes into water and oxygen. hydrogen peroxide water + oxygen The reaction can be speeded up by adding manganese dioxide. (a) (i) What do we call a substance that speeds up a chemical reaction without being changed itself? Give two other ways of increasing the rate of this reaction. 1 2 Page 10 of 50

11 (b) The diagram shows how the rate of this reaction can be measured. As the hydrogen peroxide decomposes, the mass of the flask and its contents decreases. Why does this decrease in mass take place? (Total 4 marks) Q10. The flow diagram shows some stages in the manufacture of the fertiliser ammonium nitrate (NH 4 NO 3 ). (a) The elements needed to make ammonia (NH 3 ) are obtained from natural gas and air. Which element is obtained from the air? Page 11 of 50

12 (b) The word equation for the formation of nitrogen monoxide is: ammonia + oxygen nitrogen monoxide + water The platinum catalyst needs to be heated only at the start of the reaction. Suggest why. (c) Name the liquid A that reacts with nitrogen dioxide (NO 2 ) to produce nitric acid (HNO 3 ). (d) Describe how ammonium nitrate (NH 4 NO 3 ) can be made from two of the products shown in the flow diagram. (Total 5 marks) Q11. Marble is a rock that contains mainly calcium carbonate. This reacts with hydrochloric acid. calcium carbonate + hydrochloric acid calcium chloride + water + carbon dioxide The rate of this reaction was followed by measuring the mass of carbon dioxide formed. Page 12 of 50

13 Two 10 g samples of marble, A and B, were each reacted with 50 cm 3 of dilute hydrochloric acid, at different temperatures. The mass of carbon dioxide formed in each reaction was recorded and plotted to produce the graph below. Each reaction stopped when no more carbon dioxide was formed. In both experiments some marble was left unreacted when the reaction stopped. (a) Explain how you can tell which sample, A or B, reacted faster with the dilute hydrochloric acid. (b) The faster rate of reaction was caused by using a higher temperature. Explain, in terms of particles, why a higher temperature causes a faster rate of reaction. (3) (Total 5 marks) Page 13 of 50

14 Q12. Calcium carbonate reacts with nitric acid to produce carbon dioxide. CaCO 3 + 2HNO 3 Ca(NO 3 ) 2 + H 2 O + CO 2 A 10 g lump of calcium carbonate was reacted with 20 cm 3 of dilute nitric acid. When the reaction was finished, some of the calcium carbonate was left unreacted. The graph shows the volume of carbon dioxide made in each minute for sixteen minutes. (a) The volume of carbon dioxide made in each minute decreases until it remains steady at 83 cm 3. Explain why (b) Draw a graph line, on the axes above, for an experiment where 20 cm 3 of the same dilute nitric acid was reacted with 10 g of powdered calcium carbonate. Page 14 of 50

15 (c) Give one way of changing the rate of this reaction (other than using powdered calcium carbonate) (Total 5 marks) Q13. This item appeared in the Wolverhampton Express and Star on October 31st, Read the passage and answer the questions that follow. Fumes scare at factory Workers were forced to flee a factory after a chemical alert. The building was evacuated when a toxic gas filled the factory. It happened when nitric acid spilled on to the floor and mixed with magnesium metal powder. (a) The equation which represents the reaction between magnesium and nitric acid is: Mg (s) + 4HNO 3(aq) Mg(NO 3 ) 2(aq) + 2H 2 O + 2NO 2(g) Give the formula of the toxic gas that was produced.... (b) Explain, in terms of particles, how the toxic gas was able to fill the factory quickly (c) The reaction of nitric acid with magnesium metal powder is more dangerous than if the acid had fallen on to the same mass of magnesium bars. Explain why Page 15 of 50

16 (d) (i) Water was sprayed on to the magnesium and nitric acid to slow down the reaction. Explain, in terms of particles, why the reaction would slow down. Explain why it is better to add alkali, rather than just add water to the spillage. (Total 7 marks) Q14. Soap can be made by reacting fats with sodium hydroxide solution. fat + sodium hydroxide soap + glycerol The diagram shows a laboratory experiment to make soap. Page 16 of 50

17 From the information in the diagram, give two factors which increase the rate of this reaction. In each case explain, in terms of particles, why the rate of reaction increases. Factor Reason Factor Reason (Total 7 marks) Q15. Dilute hydrochloric acid reacts with sodium carbonate. The word equation for this reaction is: sodium carbonate + hydrochloric acid sodium chloride + water + carbon dioxide (a) The diagram shows apparatus used by student X to investigate this reaction. (i) Name the piece of apparatus labelled A.. Page 17 of 50

18 NaCO 3 NaCl Na 2 CO 3 Na 2 Cl Use the Data Sheet to help you choose the correct formula from the list for: sodium carbonate,... sodium chloride.... (b) The diagram below shows a different apparatus used by student Y to investigate the same reaction. (i) Name the pieces of apparatus labelled B and C. B... C... Both students X and Y used the same volume of acid concentration of acid temperature mass of sodium carbonate Use information from the diagrams to explain why the reaction that student Y carried out was faster.... Page 18 of 50

19 (c) The results obtained by student Y were plotted as shown below. (i) Student Y repeated the experiment exactly as before but used warmer acid. This made the reaction faster. On the graph draw a line for this faster reaction. Explain, in terms of particles, why the rate of the reaction is faster when warmer acid is used.... (3) (Total 12 marks) Page 19 of 50

20 Q16. Calcium carbonate reacts with dilute hydrochloric acid as shown in the equation below. CaCO 3 (s) + 2HCl(aq) CaCl 2 (aq) + H 2 O(l) + CO 2 (g) The rate at which this reaction takes place can be studied by measuring the amount of carbon dioxide gas produced. The graph below shows the results of four experiments, 1 to 4. In each experiment the amount of calcium carbonate, the volume of acid and the concentration of the acid were kept the same but the temperature of the acid was changed each time. The calcium carbonate was in the form of small lumps of marble. (a) Apart from altering the temperature, suggest two ways in which the reaction of calcium carbonate and hydrochloric acid could be speeded up (b) Which graph, 1 to 4, shows the results of the experiment in which the acid had the highest temperature? Experiment... Explain fully how you know. Page 20 of 50

21 (c) (i) In experiment 2, how does the rate of reaction after one minute compare with the rate of reaction after two minutes? Explain, as fully as you can, why the reaction rate changes during experiment 2. (Total 7 marks) Q17. Calcium tablets are taken to build and maintain strong bones and teeth. (a) These tablets react with hydrochloric acid in the stomach. CaCO 3 ( ) + 2HCl(aq) CaCl 2 ( ) + H 2 O( ) + CO 2 ( ) (i) Add all these missing state symbols to the balanced chemical equation. The calcium salt that is formed is absorbed during digestion. What is the name of the calcium salt? Page 21 of 50

22 (b) The volume of carbon dioxide produced by one calcium tablet in the stomach can be found as shown. The volume of carbon dioxide was recorded every 30 seconds until the reaction stopped. Time in seconds Volume of gas in cm (i) Complete the graph of these results. (3) Describe one way in which this reaction can be made to go faster. Page 22 of 50

23 2H 2 O O 2 (iii) A calculation, using the mass of this tablet, showed that 80 cm 3 of carbon dioxide would be produced if the tablet was pure calcium carbonate. What do the results show about the purity of the tablet? Explain your answer by calculating the purity of this tablet. (3) (Total 10 marks) Q18. This question is about rates of reaction. (a) Hydrogen peroxide (H 2 O 2 ) decomposes very slowly at room temperature. (i) Complete the balanced chemical equation for this reaction by writing in the formula of the missing product. The decomposition is much faster if manganese oxide is mixed with the hydrogen peroxide. Complete the sentence. Manganese oxide acts as a... for decomposition of hydrogen peroxide. (b) In an experiment 1g of manganese oxide was mixed with 50 cm 3 of hydrogen peroxide solution. The results show the volume of oxygen collected during six minutes. Time in minutes Volume of oxygen in cm Page 23 of 50

24 (i) Draw a graph of these results. (3) How long did it take for the decomposition to stop? (iii) Why did the decomposition stop? (c) In a second experiment water had been added to the hydrogen peroxide solution. Again 50 cm 3 of this hydrogen peroxide solution was mixed with 1g of manganese oxide. (i) For this second experiment, sketch, on the same grid, a graph line you would expect to get. In this second experiment, why would the rate of reaction be different to the first experiment? (Total 10 marks) Page 24 of 50

25 Q19. Mountaineers can warm their food in self-heating, sealed containers. (a) The water is allowed to react with the lime. The heat from the reaction warms the food. What type of reaction causes a rise in temperature?... (b) Some students investigated the effect of adding different sized lumps of lime to water. The results of their investigation are shown. Temperature in C Time in minutes Large lumps of lime Small lumps of lime Powdered lime What do these results show? Give an explanation for your answer Page 25 of 50

26 (c) Suggest and explain one disadvantage of using powdered lime to heat food (Total 5 marks) Q20. A student studied the effect of temperature on the rate of reaction between hydrochloric acid and sodium thiosulphate. The student mixed 50 cm 3 of a sodium thiosulphate solution and 5 cm 3 of hydrochloric acid in a flask. The flask was placed over a cross. The student timed how long after mixing the cross could no longer be seen. (a) (i) Balance the chemical equation for this reaction. Na 2 S 2 O 3 (aq) + HCl(aq) NaCl(aq) + H 2 O(l) + SO 2 (g) + S(s) What causes the cross to be seen no longer? Page 26 of 50

27 (b) A graph of the results is shown. (i) What effect does temperature have on the rate of this reaction? Explain why temperature has this effect on the rate of reaction. (Total 5 marks) Q21. Hydrogen peroxide, H 2 O 2, is often used as a bleach. It decomposes forming water and oxygen. (a) (i) Write the balanced chemical equation for the decomposition of hydrogen peroxide. (3) Give a test for oxygen. Test... Result of test... Page 27 of 50

28 (b) The rate of decomposition of hydrogen peroxide at room temperature is very slow. Manganese oxide is a catalyst which can be used to speed up the decomposition. Complete the sentence. A catalyst is a substance which speeds up a chemical reaction. At the end of the reaction, the catalyst is... (c) Two experiments were carried out to test if the amount of manganese oxide, MnO 2 affected the rate at which the hydrogen peroxide decomposed. (i) Complete the diagram to show how you could measure the volume of oxygen formed during the decomposition. Page 28 of 50

29 The results are shown in the table. Time in minutes Volume of gas in cm 3 using 0.25 g MnO Volume of gas in cm 3 using 2.5 g MnO Draw a graph of these results. The graph for 0.25 g MnO 2 has been drawn for you. (3) (iii) Explain why the slopes of the graphs become less steep during the reaction.... Page 29 of 50

30 (iv) The same volume and concentration of hydrogen peroxide solution was used for both experiments. What two other factors must be kept the same to make it a fair test? (Total 15 marks) Q22. (a) Indigestion tablets called antacids can be taken to react with excess hydrochloric acid in the stomach. A student investigated two different antacid tablets labelled X and Y. (i) Both tablets, X and Y, contained calcium carbonate. Give the chemical symbol for each of the three elements in calcium carbonate. (3) Name the gas formed when calcium carbonate reacts with hydrochloric acid. (b) The student first reacted tablet X and then tablet Y, with 100 cm 3 of a hydrochloric acid solution. The student measured the volume of gas produced during the first five minutes. The results are shown in the table. Time in minutes Volume of gas in cm 3 Tablet X Volume of gas in cm 3 Tablet Y Page 30 of 50

31 (i) Draw a graph of the results for tablet Y. (A graph of the results for tablet X has been drawn for you.) (3) Tablet X contains less calcium carbonate than tablet Y. How do the results show this? (iii) Explain why the rate of reaction slows down for both tablets. (Total 10 marks) Page 31 of 50

32 Q23. A student studied the reaction between dilute hydrochloric acid and an excess of calcium carbonate. calcium carbonate + hydrochloric acid calcium chloride + water + carbon dioxide The student measured the volume of carbon dioxide produced in the experiment. The results are shown on the graph. (a) After how many minutes had all the acid been used up?... minutes (b) The student wrote this conclusion for the experiment: The reaction gets slower and slower as the time increases. Explain why the reaction gets slower. Your answer should be in terms of particles. Page 32 of 50

33 (c) A second experiment was carried out at a higher temperature. All other factors were the same. Draw a line on the graph above to show the results that you would expect. (Total 5 marks) Q24. Solutions A and B are colourless. When they are mixed, they react and turn blue after a period of time. A student investigated how temperature affected the rate of reaction between solutions A and B. The rate was measured by timing how long the mixture took to turn blue. The results are shown in the table. Temperature in C Time taken to turn blue, in seconds Page 33 of 50

34 (a) (i) Draw a graph for these results. (3) Use your graph to find how long it takes the solution to turn blue at 40 C. Time =... s (b) (i) How does the rate of reaction change as the temperature is increased? Page 34 of 50

35 Explain, in terms of particles, why temperature has this effect on the rate of reaction. To gain full marks in this question you should write your ideas in good English. Put them into a sensible order and use the correct scientific words. (3) (c) State one variable that must be kept constant to make this experiment a fair test. (Total 9 marks) Q25. Copper sulfate (CuSO 4 ) is a salt that has many uses. An aqueous solution of copper sulfate can be made by reacting copper oxide (CuO) with an acid. (a) (i) Name this acid.... Write a balanced symbol equation, including state symbols, for this reaction.. (b) Copper oxide reacts much faster with acid at 40 C than at 20 C. Explain why in terms of particles (Total 5 marks) Page 35 of 50

36 Q26. A student investigated the rate of reaction between marble and hydrochloric acid. The student used an excess of marble. The reaction can be represented by this equation. CaCO 3 (s) + 2HC1 (aq) CaC1 2 (aq) + H 2 O (l) + CO 2 (g) The student used the apparatus shown in the diagram. The student measured the mass of the flask and contents every half minute for ten minutes. The results are shown on the graph. Use the graph to answer the questions. (a) (b) Complete the graph opposite by drawing a line of best fit. Why did the mass of the flask and contents decrease with time? Page 36 of 50

37 (c) After how many minutes had all the acid been used up?... minutes (d) The student repeated the experiment at a higher temperature. All other variables were kept the same as in the first experiment. The rate of reaction was much faster. (i) Draw a line on the graph to show what the results for this second experiment might look like. Why does an increase in temperature increase the rate of reaction? (3) (Total 8 marks) Q27. Sodium thiosulfate solution reacts with hydrochloric acid. As the reaction takes place the solution slowly turns cloudy. The diagram shows a method of measuring the rate of this reaction. A student used this method to investigate how changing the concentration of the sodium thiosulfate solution affects the rate of this reaction. The student used different concentrations of sodium thiosulfate solution. All the other variables were kept the same. Page 37 of 50

38 The results are shown on the graph below. (a) (i) Draw a line of best fit on the graph. Suggest two reasons why all of the points do not lie on the line of best fit. 1 2 (b) (i) In a conclusion to the investigation the student stated that: The rate of this reaction is directly proportional to the concentration of the sodium thiosulfate solution. How does the graph support this conclusion? Page 38 of 50

39 Explain, in terms of particles, why the rate of reaction increases when the concentration of sodium thiosulfate is increased. (Total 6 marks) Q28. The following steps show how to use a type of glue. Step 1 Measure out equal amounts of the liquids from tubes A and B. Step 2 Mix the liquids to make the glue. Put a thin layer of the glue onto each of the surfaces to be joined. Step 3 Assemble the pieces to be joined and then hold them together with tape. Step 4 Leave the glue to set. (a) When liquids A and B are mixed a chemical reaction takes place. (i) This reaction is exothermic. State how the temperature of the mixture will change as the glue is mixed. Page 39 of 50

40 When the glue sets it forms a giant covalent structure. Explain why substances with giant covalent structures have high melting points. (b) The time taken for the glue to set at different temperatures is given in the table below. Temperature in C Time taken for the glue to set 20 3 days 60 6 hours 90 1 hour Explain, in terms of particles, why increasing the temperature changes the rate of the reaction which causes the glue to set. (Total 5 marks) Page 40 of 50

41 Q29. A student investigated the rate of reaction between marble and hydrochloric acid. The student used an excess of marble. The reaction can be represented by this equation: CaCO 3 (s) + 2HCl(aq) CaCl 2 (aq) + H 2 O(l) + CO 2 (g) The student used the apparatus shown in the diagram. The student measured the mass of the flask and contents for ten minutes. The results are shown on the graph. Use the graph to answer the questions. (a) (i) Complete the graph by drawing a line of best fit. Use the graph to find the mass of the flask and contents after 1.8 minutes.... grams Page 41 of 50

42 (iii) The rate of reaction can be measured by the steepness of the graph line. Describe, as fully as you can, how the rate of reaction changes with time in this experiment. (b) The mass of the flask and contents decreased during the experiment. Use the equation for this reaction to help you explain why. (c) A balance is used to measure the mass of the apparatus. (i) Which balance, A, B, or C, has the highest resolution? Balance A Balance B Balance C The balance with the highest resolution is balance The balance used for this experiment should have a high resolution. Explain why. Page 42 of 50

43 (d) The student repeated the experiment using powdered marble instead of marble chips. The rate of reaction between the marble and hydrochloric acid particles was much faster with the powder. Explain why. (Total 11 marks) Q30. The picture shows a lump of phosphate rock. Rob Lavinsky, irocks.com CC-BY-SA-3.0 [CC-BY-SA-3.0], via Wikimedia Commons Phosphoric acid is made by adding sulfuric acid to phosphate rock. (a) The rate of reaction between sulfuric acid and phosphate rock can be increased if the mixture is heated to a higher temperature. Explain, in terms of particles, why an increase in temperature increases the rate of reaction. Page 43 of 50

44 (b) State one other way in which the rate of reaction between sulfuric acid and phosphate rock can be increased. (Total 3 marks) Q31. The symbol equation for the decomposition of hydrogen peroxide is: 2H 2 O 2 2H 2 O + O 2 (a) This reaction is exothermic. What is an exothermic reaction? (b) A student measured the volume of oxygen produced by 50 cm 3 of hydrogen peroxide. Page 44 of 50

45 The graph shows the results. (i) Use the graph to describe the changes in the rate of the reaction from 0 to 35 seconds. (3) What was the total volume of oxygen gas collected?... cm 3 (iii) The student had calculated that the hydrogen peroxide used should produce 25 cm 3 of oxygen. Calculate the percentage yield of oxygen. Answer =... Page 45 of 50

46 (c) An increase in the temperature of the hydrogen peroxide increases the rate of the reaction. Use your knowledge of particles to explain why. (3) (Total 10 marks) Q32. Sodium thiosulfate solution reacts with hydrochloric acid. As the reaction takes place the solution slowly turns cloudy. The diagram shows a method of measuring the rate of this reaction. A student used this method to study how changing the concentration of the sodium thiosulfate solution alters the rate of this reaction. The student used different concentrations of sodium thiosulfate solution. All the other variables were kept the same. The results of the experiments are shown on the graph below. (a) (i) Draw a line of best fit on the graph. Page 46 of 50

47 Suggest two reasons why all of the points do not lie on the line of best fit. Concentration of sodium thiosulfate solution in mol per dm 3 (b) (i) In a conclusion to the experiment the student stated that: The rate of this reaction is directly proportional to the concentration of the sodium thiosulfate. How does the graph support this conclusion? Page 47 of 50

48 Explain, in terms of particles, why the rate of reaction increases when the concentration of sodium thiosulfate is increased. (Total 6 marks) Q33. A student investigated the reaction between magnesium and hydrochloric acid. The equation for the reaction is: Mg(s) magnesium + 2 HCl(aq) hydrochloric acid MgCl2(aq) magnesium chloride + H2(g) hydrogen (a) Give two observations the student could make during the reaction Page 48 of 50

49 (b) In this question you will be assessed on using good English, organising information clearly and using specialist terms where appropriate. The student investigated how the rate of this reaction changed when the concentration of hydrochloric acid was changed. Write a plan the student could use. In your plan you should: describe how you would carry out the investigation and make it a fair test describe the measurements you would make. (6) (Total 8 marks) Page 49 of 50

50 Page 50 of 50

### Q1. A student studied the reaction between dilute hydrochloric acid and an excess of calcium carbonate.

Q. A student studied the reaction between dilute hydrochloric acid and an excess of calcium carbonate. calcium carbonate + hydrochloric acid calcium chloride + water + carbon dioxide The student measured

### Section B: Some Essential Background Chemistry

Section B: Some Essential Background Chemistry Soluble and insoluble salts The importance of knowing whether a salt is soluble or insoluble in water You will remember that acids react with carbonates to

### Chenistry C2 question booklet part 1

Chenistry C2 question booklet part 94 minutes 94 marks Page of 34 Q. The diagram represents a carbon atom. (a) Use words from the box to answer the questions. electron neutron nucleus proton (i) What is

### MOLE CONVERSION PROBLEMS. 2. How many moles are present in 34 grams of Cu(OH) 2? [0.35 moles]

MOLE CONVERSION PROBLEMS 1. What is the molar mass of MgO? [40.31 g/mol] 2. How many moles are present in 34 grams of Cu(OH) 2? [0.35 moles] 3. How many moles are present in 2.5 x 10 23 molecules of CH

### Experiment 17-Chemical Reactions Lab

Since the Middle Ages, when ancient physicians attempted to find a magical substance that would cure all diseases, humans have been fascinated with chemical reactions. In order to effectively describe

### Topic 1 National Chemistry Summary Notes. Rates of Reaction

Chemical Reactions Topic 1 National Chemistry Summary Notes Rates of Reaction LI 1, 2 and 3 We know a chemical reaction has taken place when we notice one or more of the following things happening: Colour

### F321. CHEMISTRY A Atoms, Bonds and Groups ADVANCED SUBSIDIARY GCE. Monday 23 May 2011 Afternoon. Duration: 1 hour

ADVANCED SUBSIDIARY GCE CHEMISTRY A Atoms, Bonds and Groups F321 *F318510611* Candidates answer on the question paper. OCR supplied materials: Data Sheet for Chemistry A (inserted) Other materials required:

### Stoichiometry Review

Stoichiometry Review There are 20 problems in this review set. Answers, including problem set-up, can be found in the second half of this document. 1. N 2 (g) + 3H 2 (g) --------> 2NH 3 (g) a. nitrogen

### THIS IS A NEW SPECIFICATION

THIS IS A NEW SPECIFICATION ADVANCED SUBSIDIARY GCE CHEMISTRY A Atoms, Bonds and Groups F321 *CUP/T73721* Candidates answer on the question paper OCR Supplied Materials: Data Sheet for Chemistry A (Inserted)

### Chapter 16: Tests for ions and gases

The position of hydrogen in the reactivity series Hydrogen, although not a metal, is included in the reactivity series because it, like metals, can be displaced from aqueous solution, only this time the

### Q1. The chart shows the processes involved in the manufacture of nitric acid from ammonia.

Q. The chart shows the processes involved in the manufacture of nitric acid from ammonia. (a) Complete the word equation for the reaction that takes place in the first reaction vessel. ammonia +... nitrogen

### Chemistry: Chemical Equations

Chemistry: Chemical Equations Write a balanced chemical equation for each word equation. Include the phase of each substance in the equation. Classify the reaction as synthesis, decomposition, single replacement,

### Potassium + Chlorine. K(s) + Cl 2 (g) 2 KCl(s)

Types of Reactions Consider for a moment the number of possible chemical reactions. Because there are millions of chemical compounds, it is logical to expect that there are millions of possible chemical

### EXPERIMENT 5: CHEMICAL REACTIONS AND EQUATIONS

PURPOSE EXPERIMENT 5: CHEMICAL REACTIONS AND EQUATIONS To perform and observe simple chemical reactions. To identify the products of chemical reactions and write balanced equations for those reactions.

### WRITING CHEMICAL FORMULA

WRITING CHEMICAL FORMULA For ionic compounds, the chemical formula must be worked out. You will no longer have the list of ions in the exam (like at GCSE). Instead you must learn some and work out others.

### IB Chemistry. DP Chemistry Review

DP Chemistry Review Topic 1: Quantitative chemistry 1.1 The mole concept and Avogadro s constant Assessment statement Apply the mole concept to substances. Determine the number of particles and the amount

### SCH 4C1 Unit 2 Problem Set Questions taken from Frank Mustoe et all, "Chemistry 11", McGraw-Hill Ryerson, 2001

SCH 4C1 Unit 2 Problem Set Questions taken from Frank Mustoe et all, "Chemistry 11", McGraw-Hill Ryerson, 2001 1. A small pin contains 0.0178 mol of iron. How many atoms of iron are in the pin? 2. A sample

### Syllabus OC18 Use litmus or a universal indicator to test a variety of solutions, and classify these as acidic, basic or neutral

Chemistry: 9. Acids and Bases Please remember to photocopy 4 pages onto one sheet by going A3 A4 and using back to back on the photocopier Syllabus OC18 Use litmus or a universal indicator to test a variety

### Friday 23 May 2014 Morning

Friday 23 May 2014 Morning AS GCE CHEMISTRY A F321/01 Atoms, Bonds and Groups *1168266380* Candidates answer on the Question Paper OCR supplied materials: Data Sheet for Chemistry A (inserted) Other materials

### Chapter 8 - Chemical Equations and Reactions

Chapter 8 - Chemical Equations and Reactions 8-1 Describing Chemical Reactions I. Introduction A. Reactants 1. Original substances entering into a chemical rxn B. Products 1. The resulting substances from

### Instructions Answer all questions in the spaces provided. Do all rough work in this book. Cross through any work you do not want to be marked.

GCSE CHEMISTRY Higher Tier Chemistry 1H H Specimen 2018 Time allowed: 1 hour 45 minutes Materials For this paper you must have: a ruler a calculator the periodic table (enclosed). Instructions Answer all

### General Chemistry Lab Experiment 6 Types of Chemical Reaction

General Chemistry Lab Experiment 6 Types of Chemical Reaction Introduction Most ordinary chemical reactions can be classified as one of five basic types. The first type of reaction occurs when two or more

### HIGHER TIER CHEMISTRY MINI-MOCK UNIT 2 [C2.1, C2.2&C2.3, C2.4, C2.5, C2.6 and C2.7] (a) Name particles X and Y.

HIGHER TIER CHEMISTRY MINI-MOCK UNIT 2 [C2., C2.2&C2.3, C2.4, C2.5, C2.6 and C2.7] C2. Structure and Bonding Questions Q. The diagram shows a model of part of the giant lattice of a metal. (a) Name particles

### CHEMICAL REACTIONS AND REACTING MASSES AND VOLUMES

CHEMICAL REACTIONS AND REACTING MASSES AND VOLUMES The meaning of stoichiometric coefficients: 2 H 2 (g) + O 2 (g) 2 H 2 O(l) number of reacting particles 2 molecules of hydrogen react with 1 molecule

### Balancing Chemical Equations Worksheet

Balancing Chemical Equations Worksheet Student Instructions 1. Identify the reactants and products and write a word equation. 2. Write the correct chemical formula for each of the reactants and the products.

### THIS IS A NEW SPECIFICATION

THIS IS A NEW SPECIFICATION ADVANCED SUBSIDIARY GCE CHEMISTRY A Atoms, Bonds and Groups F321 * OCE / 1 9 2 3 2* Candidates answer on the Question Paper OCR Supplied Materials: Data Sheet for Chemistry

### Chemistry 12 Worksheet 1-1 - Measuring Reaction Rates

Chemistry 12 Worksheet 1-1 - Measuring Reaction Rates 1. A chemist wishes to determine the rate of reaction of zinc with hydrochloric acid. The equation for the reaction is: Zn (s) + 2HCl (aq) oh 2(g)

### Q1. Hydrogen chloride (HCl) can be made by the reaction of hydrogen (H 2) with chlorine (Cl 2).

Q. Hydrogen chloride (HCl) can be made by the reaction of hydrogen (H 2) with chlorine (Cl 2). (a) The diagrams represent molecules of hydrogen and chlorine. Draw a similar diagram to represent a molecule

### Draw a ring around the correct answer to complete each sentence. 11. Ammonia can be reacted with an acid to produce the salt ammonium nitrate.

Q. This question is about salts of ammonia and salts of lead. (a) Ammonia dissolves in water to make an alkaline solution. Draw a ring around the correct answer to complete each sentence. The ph of a solution

### Experiment 9 - Double Displacement Reactions

Experiment 9 - Double Displacement Reactions A double displacement reaction involves two ionic compounds that are dissolved in water. In a double displacement reaction, it appears as though the ions are

### Coimisiún na Scrúduithe Stáit State Examinations Commission

2015. M33 Coimisiún na Scrúduithe Stáit State Examinations Commission LEAVING CERTIFICATE EXAMINATION, 2015 CHEMISTRY ORDINARY LEVEL TUESDAY, 16 JUNE AFTERNOON 2.00 TO 5.00 400 MARKS Answer eight questions

### Experiment 5. Chemical Reactions A + X AX AX A + X A + BX AX + B AZ + BX AX + BZ

Experiment 5 Chemical Reactions OBJECTIVES 1. To observe the various criteria that are used to indicate that a chemical reaction has occurred. 2. To convert word equations into balanced inorganic chemical

### CHAPTER 9. ANS: a. ANS: d. ANS: c. ANS: a. ANS: c

CHAPTER 9 1. Which one of the following is the acid in vinegar? a. acetic acid b. citric acid c. muriatic acid d. ascorbic acid 2. Which is a basic or alkaline substance? a. gastric fluid b. black coffee

### Chapter 3. Stoichiometry: Ratios of Combination. Insert picture from First page of chapter. Copyright McGraw-Hill 2009 1

Chapter 3 Insert picture from First page of chapter Stoichiometry: Ratios of Combination Copyright McGraw-Hill 2009 1 3.1 Molecular and Formula Masses Molecular mass - (molecular weight) The mass in amu

### Cambridge International Examinations Cambridge International General Certificate of Secondary Education

Cambridge International Examinations Cambridge International General Certificate of Secondary Education *0123456789* CHEMISTRY 0620/03 Paper 3 Theory (Core) For Examination from 2016 SPECIMEN PAPER 1 hour

### Advanced Subsidiary Unit 1: The Core Principles of Chemistry

Write your name here Surname Other names Edexcel GCE Centre Number Chemistry Advanced Subsidiary Unit 1: The Core Principles of Chemistry Candidate Number Thursday 13 January 2011 Morning Time: 1 hour

### AP Chem Unit 1 Assignment 3 Chemical Equations

Symbols used in chemical equations: Symbol Meaning + used to separate one reactant or product from another used to separate the reactants from the products - it is pronounced "yields" or "produces" when

### ATOMS. Multiple Choice Questions

Chapter 3 ATOMS AND MOLECULES Multiple Choice Questions 1. Which of the following correctly represents 360 g of water? (i) 2 moles of H 2 0 (ii) 20 moles of water (iii) 6.022 10 23 molecules of water (iv)

### The relationship between the concentration of a reactant and the rate of reaction with respect to that reactant can be shown using rate time graphs.

The effect of concentration on rate Student sheet To study The relationship between the concentration of a reactant and the rate of reaction with respect to that reactant can be shown using rate time graphs.

### Worksheet # 11. 4. When heated, nickel (II) carbonate undergoes a decomposition reaction. Write a balanced equation to describe this reaction

Worksheet # 11 1. A solution of sodium chloride is mixed with a solution of lead (II) nitrate. A precipitate of lead (II) chloride results, leaving a solution of sodium nitrated. Determine the class of

### Programme in mole calculation

Programme in mole calculation Step 1 Start at the very beginning Atoms are very small indeed! If we draw a line 1 metre long, 6,000,000,000 (6 billion) atoms could be lined end to end. So a scientist cannot

### ? I have some understanding but I need to revise this some more

1 I am confident that I understand this and I can apply this to problems? I have some understanding but I need to revise this some more I don t know this or I need help because I don t understand it National

### Experiment 8 - Double Displacement Reactions

Experiment 8 - Double Displacement Reactions A double displacement reaction involves two ionic compounds that are dissolved in water. In a double displacement reaction, it appears as though the ions are

### 1. Read P. 368-375, P. 382-387 & P. 429-436; P. 375 # 1-11 & P. 389 # 1,7,9,12,15; P. 436 #1, 7, 8, 11

SCH3U- R.H.KING ACADEMY SOLUTION & ACID/BASE WORKSHEET Name: The importance of water - MAKING CONNECTION READING 1. Read P. 368-375, P. 382-387 & P. 429-436; P. 375 # 1-11 & P. 389 # 1,7,9,12,15; P. 436

### Learn Chemistry. Starter for Ten 7. Kinetics. Registered Charity Number 207890

Learn Chemistry Starter for Ten 7. Kinetics Developed by Dr Kristy Turner, RSC School Teacher Fellow 2011-2012 at the University of Manchester, and Dr Catherine Smith, RSC School Teacher Fellow 2011-2012

### Thursday 23 May 2013 Morning

Thursday 23 May 2013 Morning AS GCE CHEMISTRY A F321/01 Atoms, Bonds and Groups *F314600613* Candidates answer on the Question Paper OCR supplied materials: Data Sheet for Chemistry A (inserted) Other

### Chemistry *P42864A0120* P42864A. Unit: KCH0/4CH0 Paper: 2C. Thursday 16 January 2014 Afternoon Time: 1 hour. Instructions. Information.

Write your name here Surname Other names Pearson Edexcel Certificate Pearson Edexcel International GCSE Chemistry Unit: KCH0/4CH0 Paper: 2C Centre Number Candidate Number Thursday 16 January 2014 Afternoon

### Module Seven Including Liquids and Solutions in Stoichiometric Calculations. Chem 170. Stoichiometric Calculations. Module Seven

Chem 170 Stoichiometric Calculations Module Seven Including Liquids and Solutions in Stoichiometric Calculations DePauw University Department of Chemistry and Biochemistry Page 1 Introduction to Module

### 0.786 mol carbon dioxide to grams g lithium carbonate to mol

1 2 Convert: 2.54 x 10 22 atoms of Cr to mol 4.32 mol NaCl to grams 0.786 mol carbon dioxide to grams 2.67 g lithium carbonate to mol 1.000 atom of C 12 to grams 3 Convert: 2.54 x 10 22 atoms of Cr to

### EDEXCEL INTERNATIONAL GCSE CHEMISTRY EDEXCEL CERTIFICATE IN CHEMISTRY ANSWERS SECTION C

EDEXCEL INTERNATIONAL GCSE CHEMISTRY EDEXCEL CERTIFICATE IN CHEMISTRY ANSWERS SECTION C Chapter 16 1. Burn sulfur in air to give sulfur dioxide. S(s) + O 2 (g) ----> SO 2 (g) Pass this with more air over

### Question Bank Electrolysis

Question Bank Electrolysis 1. (a) What do you understand by the terms (i) electrolytes (ii) non-electrolytes? (b) Arrange electrolytes and non-electrolytes from the following substances (i) sugar solution

### MOLES AND MOLE CALCULATIONS

35 MOLES ND MOLE CLCULTIONS INTRODUCTION The purpose of this section is to present some methods for calculating both how much of each reactant is used in a chemical reaction, and how much of each product

### Formulae, Equations & Formula Mass

St Peter the Apostle High School Chemistry Department Formulae, Equations & Formula Mass N4 & N5 Homework Questions Answer questions as directed by your teacher. National 4 level questions are first followed

### Friday 13 January 2012 Afternoon

Friday 13 January 2012 Afternoon AS GCE CHEMISTRY A F321 Atoms, Bonds and Groups *F314420112* Candidates answer on the Question Paper. OCR supplied materials: Data Sheet for Chemistry A (inserted) Other

### Chapter 15 - Nitrogen

Nitrogen an essential element The Haber process Obtaining nitrogen Obtaining hydrogen Making ammonia Chapter 15 - Nitrogen Ammonia gas Making ammonia in a laboratory Physical properties of ammonia Chemical

### Advanced Subsidiary Unit 1: The Core Principles of Chemistry

Write your name here Surname Other names Edexcel GCE Centre Number Chemistry Advanced Subsidiary Unit 1: The Core Principles of Chemistry Candidate Number Tuesday 15 May 2012 Afternoon Time: 1 hour 30

### Multiple Choice Questions NCERT

CHAPTER 3 Metals and Non-metals Multiple Choice Questions 1. Which of the following property is generally not shown by metals? (a) Electrical conduction (b) Sonorous in nature (c) Dullness (d) Ductility

### CHM-101-A Exam 2 Version 1 October 10, 2006

CHM-101-A Exam 2 Version 1 1. Which of the following statements is incorrect? A. SF 4 has ¼ as many sulfur atoms as fluorine atoms. B. Ca(NO 3 ) 2 has six times as many oxygen atoms as calcium ions. C.

### Chapter 9. Answers to Questions

Chapter 9 Answers to Questions 1. Word equation: Silicon Tetrachloride + Water Silicon Dioxide + Hydrogen Chloride Formulas: Next, the chemical formulas are needed. As these are all covalent compounds,

### Chemical Equations and Chemical Reactions. Chapter 8.1

Chemical Equations and Chemical Reactions Chapter 8.1 Objectives List observations that suggest that a chemical reaction has taken place List the requirements for a correctly written chemical equation.

### Chapter 3 Stoichiometry: Calculations with Chemical Formulas and Equations

CHE11 Chapter Chapter Stoichiometry: Calculations with Chemical Formulas and Equations 1. When the following equation is balanced, the coefficients are. NH (g) + O (g) NO (g) + H O (g) (a). 1, 1, 1, 1

### Formulae, stoichiometry and the mole concept

3 Formulae, stoichiometry and the mole concept Content 3.1 Symbols, Formulae and Chemical equations 3.2 Concept of Relative Mass 3.3 Mole Concept and Stoichiometry Learning Outcomes Candidates should be

### Chapter 8: Chemical Equations and Reactions

Chapter 8: Chemical Equations and Reactions I. Describing Chemical Reactions A. A chemical reaction is the process by which one or more substances are changed into one or more different substances. A chemical

### Number of moles of solute = Concentration (mol. L ) x Volume of solution (litres) or n = C x V

44 CALCULATIONS INVOLVING SOLUTIONS INTRODUCTION AND DEFINITIONS Many chemical reactions take place in aqueous (water) solution. Quantities of such solutions are measured as volumes, while the amounts

### Specimen Paper. Time allowed! 60 minutes

Centre Number Surname Candidate Number Specimen Paper For Examiner s Use Other Names Candidate Signature Examiner s Initials General Certificate of Secondary Education Foundation Tier Question 1 Mark Chemistry

### Chapter 7: Chemical Equations. Name: Date: Period:

Chapter 7: Chemical Equations Name: Date: Period: 7-1 What is a chemical reaction? Read pages 232-237 a) Explain what a chemical reaction is. b) Distinguish between evidence that suggests a chemical reaction

### Chapter 6 Oxidation-Reduction Reactions. Section 6.1 2. Which one of the statements below is true concerning an oxidation-reduction reaction?

Chapter 6 Oxidation-Reduction Reactions 1. Oxidation is defined as a. gain of a proton b. loss of a proton c. gain of an electron! d. loss of an electron e. capture of an electron by a neutron 2. Which

### W1 WORKSHOP ON STOICHIOMETRY

INTRODUCTION W1 WORKSHOP ON STOICHIOMETRY These notes and exercises are designed to introduce you to the basic concepts required to understand a chemical formula or equation. Relative atomic masses of

### Chapter 12 Stoichiometry

Chapter 12 Stoichiometry I. How much can a reaction produce? (12.1) A. Proportional Relationships 1. like recipes 2. how much can I get? 3. how much do I need? Stoichiometry: mass and quantity relationships

### CHEMISTRY. SCIENCE Paper 2. SECTION I (40 Marks)

CEMISTRY SCIENCE Paper 2 (Two hours) Answers to this Paper must be written on the paper provided separately. You will not be allowed to write during the first 15 minutes. This time is to be spent in reading

Candidate Style Answer Chemistry A Unit F321 Atoms, Bonds and Groups High banded response This Support Material booklet is designed to accompany the OCR GCE Chemistry A Specimen Paper F321 for teaching

### Question Bank Nitric Acid and Nitrates

Question Bank Nitric Acid and Nitrates 1. In laboratory preparation of nitric acid from potassium nitrate or sodium nitrate state with reasons : (a) the acid used (b) the type of apparatus used (c) temperature

### THIS IS A NEW SPECIFICATION

THIS IS A NEW SPECIFICATION ADVANCED SUBSIDIARY GCE CHEMISTRY A Atoms, Bonds and Groups F321 *CUP/T73723* Candidates answer on the question paper OCR Supplied Materials: Data Sheet for Chemistry A (Inserted)

### hij GCSE Additional Science Chemistry 2 Higher Tier Chemistry 2H SPECIMEN MARK SCHEME Version 1.0

hij GCSE Additional Science Chemistry 2 Higher Tier Chemistry 2H SPECIMEN MARK SCHEME Version.0 Copyright 20 AQA and its licensors. All rights reserved. The Assessment and Qualifications Alliance (AQA)

### Writing and Balancing Chemical Equations

Name Writing and Balancing Chemical Equations Period When a substance undergoes a chemical reaction, chemical bonds are broken and new bonds are formed. This results in one or more new substances, often

### Unit 9 Stoichiometry Notes (The Mole Continues)

Unit 9 Stoichiometry Notes (The Mole Continues) is a big word for a process that chemist s use to calculate amounts in reactions. It makes use of the coefficient ratio set up by balanced reaction equations

### Chemistry Post-Enrolment Worksheet

Name: Chemistry Post-Enrolment Worksheet The purpose of this worksheet is to get you to recap some of the fundamental concepts that you studied at GCSE and introduce some of the concepts that will be part

### IB Chemistry 1 Mole. One atom of C-12 has a mass of 12 amu. One mole of C-12 has a mass of 12 g. Grams we can use more easily.

The Mole Atomic mass units and atoms are not convenient units to work with. The concept of the mole was invented. This was the number of atoms of carbon-12 that were needed to make 12 g of carbon. 1 mole

### Chapter 3 Mass Relationships in Chemical Reactions

Chapter 3 Mass Relationships in Chemical Reactions Student: 1. An atom of bromine has a mass about four times greater than that of an atom of neon. Which choice makes the correct comparison of the relative

### GCSE Chemistry. Making Salts Instructions and answers for teachers

GCSE Chemistry Making Salts Instructions and answers for teachers The Activity: Learning Outcomes: To be able to recall the names and chemical formulae for commonly used acids To understand how salts can

### Period 3 elements

3.1.4.2 Period 3 elements 173 minutes 169 marks Page 1 of 17 Q1. (a) Explain why certain elements in the Periodic Table are classified as p-block elements. Illustrate your answer with an example of a p-block

### Unit 10A Stoichiometry Notes

Unit 10A Stoichiometry Notes Stoichiometry is a big word for a process that chemist s use to calculate amounts in reactions. It makes use of the coefficient ratio set up by balanced reaction equations

### CHEMICAL EQUATIONS and REACTION TYPES

31 CHEMICAL EQUATIONS and REACTION TYPES The purpose of this laboratory exercise is to develop skills in writing and balancing chemical equations. The relevance of this exercise is illustrated by a series

### Worked solutions to student book questions Chapter 4 Analysing acids and bases

Q. Antacid tablets should normally be chewed before they are swallowed. Why? A. Antacid tablets are normally chewed to provide a larger surface area for faster reaction with stomach acids. Q. A laboratory

### Balancing chemical equations

Balancing chemical equations The law of conservation of mass In order to balance a chemical equation, it is important to understand the law of conservation of mass. Definition 1: The law of conservation

### The component present in larger proportion is known as solvent.

40 Engineering Chemistry and Environmental Studies 2 SOLUTIONS 2. DEFINITION OF SOLUTION, SOLVENT AND SOLUTE When a small amount of sugar (solute) is mixed with water, sugar uniformally dissolves in water

### Chapter 5, Calculations and the Chemical Equation

1. How many iron atoms are present in one mole of iron? Ans. 6.02 1023 atoms 2. How many grams of sulfur are found in 0.150 mol of sulfur? [Use atomic weight: S, 32.06 amu] Ans. 4.81 g 3. How many moles

### Concept 1. The meaning and usefulness of the mole. The mole (or mol) represents a certain number of objects.

Chapter 3. Stoichiometry: Mole-Mass Relationships in Chemical Reactions Concept 1. The meaning and usefulness of the mole The mole (or mol) represents a certain number of objects. SI def.: the amount of

### Exampro GCSE Chemistry

Exampro GCSE Chemistry C2 Chapter 5 Higher Name: Class: Author: Date: Time: 73 Marks: 73 Comments: Page of 27 Q. (a) In this question you will be assessed on using good English, organising information

### HOMEWORK 4A. Definitions. Oxidation-Reduction Reactions. Questions

HOMEWORK 4A Oxidation-Reduction Reactions 1. Indicate whether a reaction will occur or not in each of following. Wtiring a balcnced equation is not necessary. (a) Magnesium metal is added to hydrochloric

### Balancing Chemical Equations

Balancing Chemical Equations Academic Success Center Science Tutoring Area Science Tutoring Area Law of Conservation of Mass Matter cannot be created nor destroyed Therefore the number of each type of

### Enthalpy of Reaction and Calorimetry worksheet

Enthalpy of Reaction and Calorimetry worksheet 1. Calcium carbonate decomposes at high temperature to form carbon dioxide and calcium oxide, calculate the enthalpy of reaction. CaCO 3 CO 2 + CaO 2. Carbon

### The Reaction of Calcium Chloride with Carbonate Salts

The Reaction of Calcium Chloride with Carbonate Salts PRE-LAB ASSIGNMENT: Reading: Chapter 3 & Chapter 4, sections 1-3 in Brown, LeMay, Bursten, & Murphy. 1. What product(s) might be expected to form when

### 10TH CHEMISTRY NOTES

1. Acids: Acids are sour in taste, turn blue litmus red and give H3O+ ion (hydronium ions in solution. e.g. HCl, H2SO4, HNO3 etc 2. Bases: Bases are bitter in taste, have soapy touch, turns red litmus

### DETERMINING THE ENTHALPY OF FORMATION OF CaCO 3

DETERMINING THE ENTHALPY OF FORMATION OF CaCO 3 Standard Enthalpy Change Standard Enthalpy Change for a reaction, symbolized as H 0 298, is defined as The enthalpy change when the molar quantities of reactants

### Moles and Empirical Formula

Privacy Statement Site Map Contact Us Home Papers Revision Community Blog Games Advertise GCSE: Biology Commerce Statistics A-Level: Physics Economics Home Revision GCSE Moles and Empirical Formula Moles

### EXPERIMENT 10: Electrical Conductivity Chem 111

EXPERIMENT 10: Electrical Conductivity Chem 111 INTRODUCTION A. Electrical Conductivity A substance can conduct an electrical current if it is made of positively and negatively charged particles that are

### Chem 1100 Chapter Three Study Guide Answers Outline I. Molar Mass and Moles A. Calculations of Molar Masses

Chem 1100 Chapter Three Study Guide Answers Outline I. Molar Mass and Moles A. Calculations of Molar Masses B. Calculations of moles C. Calculations of number of atoms from moles/molar masses 1. Avagadro