7-A. Inquiry INVESTIGATION. 322 MHR Unit 3 Quantities in Chemical Reactions. Skill Check. Safety Precautions
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1 Inquiry INVESTIGATION 7-A Skill Check Initiating and Planning Performing and Recording Analyzing and Interpreting Communicating Safety Precautions Wear safety eyewear throughout this investigation. Wear a lab coat or apron throughout this investigation. Wear protective gloves when performing this investigation. Tie back loose hair and clothing. The reaction mixture may get hot. Do not hold the beaker as the reaction proceeds. Copper(II) chloride is toxic. Do not ingest. Do not inhale the vapours. If you get copper(ii) chloride on your skin, flush with plenty of water. Limiting and Excess Reactants In this investigation, you will observe a limiting reactant in a single displacement reaction. In the reaction, 0.50 g of solid aluminum, Al(s), will react with 0.50 g of copper (II) chloride, CuCl 2 (s), dissolved in water. After the reaction, you will determine which compound was the limiting reactant and which compound was the excess reactant. Pre-Lab Questions 1. What is the balanced chemical equation for the single displacement reaction described in the introduction of this investigation? 2. When a chemical reaction is in progress, what observations indicate that a chemical change is occurring? 3. What observations might indicate that a chemical reaction is complete. Question How can you use observations and calculations to determine the limiting reactant in the chemical reaction of aluminum foil and aqueous copper(ii) chloride? Materials 2.0 g of copper(ii) chloride, CuCl 2 (s) 0.50 g of aluminum foil, Al(s) distilled water graduated cylinder spatula electronic balance 100 ml beaker stirring rod When aluminum and copper(ii) chloride react, a single displacement reaction occurs. 322 MHR Unit 3 Quantities in Chemical Reactions
2 Procedure 1. Prepare a data table to record your observations and measurements. Give your table an appropriate title. 2. Observe the physical properites of the copper(ii) chloride and the aluminum foil. Write your observations in your data table. 3. Measure and record the mass of both reactants. Place the copper(ii) chloride in a beaker. Add 50 ml of distilled water to the beaker. Stir the contents of the beaker with a stirring rod, and record your observations. 4. Tear the aluminum foil into small pieces. Then add it to the copper(ii) chloride solution. Record the initial colour of the solution, and describe the appearance of the metal at the beginning of the reaction. 5. Record your observations as the reaction proceeds. Pay particular attention to any colour changes and any changes in the appearance of the metal. Stir occasionally with the stirring rod. 6. When the reaction is complete, ask your teacher for proper disposal instructions. Do not pour anything down the drain. Analyze and Interpret 1. a. What colour was the copper(ii) chloride solution before the aluminum foil was added? b. What colour was the solution after the reaction was complete? Did all the copper(ii) chloride react? Explain. c. Describe the appearance of the aluminum foil. Did all the aluminum foil react? How do you know? d. Based on the colour of the metal and the balanced chemical equation, what is the solid that formed during the chemical reaction? 2. a. Use the masses in your data table to determine the limiting reactant in this chemical reaction. Which reactant was in excess? b. Compare your observations and your calculations. Do your calculations support your observations? Explain. Conclude and Communicate 3. Summarize your findings. Are stoichiometric calculations an effective way to predict limiting and excess reactants? Explain your answer. 4. Write a conclusion to explain how your experimental observations did or did not support your theoretical calculations. Extend Further 5. INQUIRY Magnesium and hydrochloric acid react as follows: Mg(s) + 2HCl(aq) MgCl 2 (aq) + H 2 (g) a. Examine the equation. What would you expect to observe if magnesium was the limiting reactant? What would you expect to observe if the hydrochloric acid was the limiting reactant? b. Suppose that you have a piece of magnesium and a beaker that contains hydrochloric acid of unknown concentration. Design a procedure you could use to determine which reactant is the limiting reactant. State the safety precautions that you should take. If your teacher approves, carry out your procedure. 6. RESEARCH Use text or Internet sources to obtain the material data safety sheets (MSDSs) for copper(ii) chloride and aluminum chloride. Examine the information about first aid measures, accidental release measures, handling and storage, exposure controls, and personal protection. Write a brief summary of your findings. Chapter 7 Chemical Reactions and Stoichiometry MHR 323
3 Inquiry INVESTIGATION Skill Check Initiating and Planning Performing and Recording Analyzing and Interpreting Communicating Safety Precautions Wear safety eyewear throughout this investigation. Wear a lab coat or apron throughout this investigation. Tie back loose hair and clothing Copper(II) chloride dihydrate is toxic. Do not ingest. Do not inhale the vapours. Do not inhale hydrochloric acid vapours. If you get copper(ii) chloride dihydrate or hydrochloric acid solution on your skin, flush with plenty of water. Materials 5.00 g of copper(ii) chloride dihydrate, CuCl 2 2H 2 O(s) distilled water 1.00 g piece of steel wool, Fe(s) 10 ml of 1 mol/l hydrochloric acid, HCl(aq) two 250 ml beakers waterproof grease marker electronic balance stirring rod wash bottle with distilled water drying oven or heat lamp 7-B Finding the Percentage Yield of a Single Displacement Reaction The percentage yield of any reaction can be affected by several different factors. One of these factors is the impurity of the reactants. In this investigation, you will conduct a single displacement reaction in which the iron, Fe(s), in steel wool reacts with aqueous copper(ii) chloride, CuCl 2 (aq), to produce aqueous iron(ii) chloride, FeCl 2 (aq), and a precipitate. You will then determine the percentage yield of the precipitate in the reaction and determine the effect of an impure reactant on this yield. Pre-Lab Questions 1. What is the balanced chemical equation for the reaction in this investigation? 2. Which reactant is considered impure in this investigation? 3. How might an impure reactant affect the percentage yield of a reaction? Explain. 4. Why is it important to flush your skin with plenty of water if it comes in contact with copper(ii) chloride dihydrate or hydrochloric acid? Question What is the percentage yield of the precipitate in the reaction of iron and copper(ii) chloride when steel wool and aqueous copper(ii) chloride are used as reactants? Procedure 1. Obtain a clean, dry 250 ml beaker. Mark the beaker with a grease marker so that you can identify it later. 2. Copy the following data table into your notebook. Data Table Material Empty labelled beaker Copper(II) chloride dihydrate Iron (steel wool) Beaker containing clean, dry copper Mass (grams) 324 MHR Unit 3 Quantities in Chemical Reactions
4 3. Measure the mass of the beaker, and record the mass in your data table. 4. Measure 5.00 g of copper(ii) chloride dihydrate, and place it in the beaker. Add 50 ml of distilled water. Stir to dissolve the solid blue material. (Note: When a copper(ii) chloride dihydrate is dissolved in water, it is aqueous copper(ii) chloride.) 5. Measure 1.00 g of iron (steel wool) and record the mass in your data table. 6. Unravel the iron (steel wool) over a piece of paper to catch all the pieces. Then add the steel wool to the solution in the beaker. Allow the reaction mixture to sit until all the iron has reacted. It should take 2 to 3 min for the reaction to go to completion. 7. When the reaction is complete and no iron is visible, carefully pour the solution into a 250 ml beaker by decanting the liquid. To decant the liquid, slowly pour the liquid down the length of a stirring rod, as shown in the diagram below. Decanting the liquid in this way prevents the liquid from flowing down the side of the reaction beaker instead of flowing into the second beaker. Decant the liquid carefully to prevent any precipitate from escaping from the reaction beaker. stirring rod beaker 8. Rinse the precipitate several times with distilled water, using a wash bottle. Decant the water each time. 9. Clean the precipitate with hydrochloric acid by adding approximately 10 ml of 1 mol/l hydrochloric acid. Decant the hydrochloric acid, and perform a final distilled water rinse of the precipitate. Try to decant as much liquid as possible from the beaker without losing any precipitate. 10. Place your labelled reaction beaker, containing the cleaned precipitate, in a drying oven overnight. 11. On the following day, determine the mass of the beaker with the dry precipitate. 12. Dispose of the precipitate as instructed by your teacher. Analyze and Interpret 1. a. Identify the precipitate that was formed in the reaction. b. Which reactant was the limiting reactant, and which was the excess reactant? c. Calculate the theoretical yield of the precipitate, in grams, using the mass of the steel wool that you measured in Procedure step 5. d. Compare the mass of the precipitate you collected (the actual yield) with the expected theoretical yield. Describe your observations. 2. Calculate the percentage yield of this reaction. Conclude and Communicate 3. Suggest reasons why the percentage yield of this reaction was not 100%. 4. Explain how the impurity of the iron affected the actual yield. 5. Review the laboratory techniques that you used in this investigation. Did these laboratory techniques affect your actual percentage yield? Explain. Extend Further 6. INQUIRY Design an investigation that uses the same balanced chemical equation as this investigation but improves your percentage yield. State the safety precautions that you should take. With your teacher s approval, conduct your investigation. Calculate the actual percentage yield, and compare it with the percentage yield you obtained in this investigation. 7. RESEARCH Conduct research to find the percent by mass of iron in steel wool. Do you think your percentage yield would have been different if you had used pure iron in this investigation? Explain your reasoning. Chapter 7 Chemical Reactions and Stoichiometry MHR 325
5 Inquiry INVESTIGATION Skill Check Initiating and Planning Performing and Recording Analyzing and Interpreting Communicating Safety Precautions Wear safety eyewear throughout this investigation. Wear a lab coat or apron throughout this investigation. Tie back loose hair and clothing. If you get chemical compounds from this lab on your skin, flush with plenty of cold water. Caution: Calcium chloride is corrosive. Materials 2.00 g of sodium carbonate, Na 2 CO 3 (s) distilled water 1.00 g of calcium chloride, CaCl 2 (s) graduated cylinder two 250 ml beakers waterproof grease marker electronic balance, accurate to two decimal places stirring rod filter paper funnel retort stand with ring clamp Erlenmeyer flask wash bottle with distilled water drying oven or heat lamp 7-C Finding the Percentage Yield of a Double Displacement Reaction The percentage yield of a reaction is affected by different factors, including reaction procedures and laboratory techniques. In this investigation, you will conduct a double displacement reaction in which a solution of sodium carbonate, Na 2 CO 3 (aq), reacts with a solution of calcium chloride, CaCl 2 (aq), to produce aqueous sodium chloride, NaCl(aq), and a solid precipitate. You will then determine the percentage yield of calcium carbonate, CaCO 3 (s), in the reaction and determine the effects of reaction procedures and laboratory techniques on this yield. Pre-Lab Questions 1. Explain, in your own words, what a double displacement reaction is. 2. What is the balanced chemical equation for the reaction in this investigation? 3. List three ways in which the actual product yield can be reduced during the filtration of a precipitate. Question What is the percentage yield of calcium carbonate from the reactants sodium carbonate and calcium chloride? Procedure 1. Obtain two clean, dry 250 ml beakers. Label the beakers with a grease marker, using the names of the reactant solutions. 2. Copy the following data table into your notebook. Measure the masses of the empty labelled beakers, and record these masses in your data table. Data Table Material Sodium carbonate Empty labelled beaker Beaker and sodium carbonate Sodium carbonate Calcium chloride Empty labelled beaker Beaker and calcium chloride Calcium chloride Product Clean, dry, labelled filter paper Filter paper and dry calcium carbonate precipitate Mass (g) 326 MHR Unit 3 Quantities in Chemical Reactions
6 3. Measure 2.00 g of sodium carbonate, and place it in the corresponding labelled beaker. Measure and record the mass of the beaker with the sodium carbonate. Add 50 ml of distilled water to the beaker. Stir to dissolve the solid material. If the stirring rod is removed from the beaker, rinse it with distilled water, and allow the water to flow into the beaker so that you do not lose the reactant. 4. Measure 1.00 g of calcium chloride, and place it in the other labelled beaker. Measure and record the mass of the beaker with the calcium chloride. Add 50 ml of distilled water to the beaker. Stir to dissolve the solid material. If the stirring rod is removed from the beaker, rinse it as described in step When both solids have dissolved, gently pour the entire contents of the sodium carbonate beaker, a portion at a time, into the calcium chloride beaker while stirring constantly. 6. Observe and record all the changes that occur in the reaction beaker. 7. When the reaction is complete (about 2 min), label a piece of filter paper. Measure the mass of the filter paper, and record the mass in your data table. Set up the funnel, filter paper, and flask as shown in step 3 in the diagram. 8. Gently swirl the reaction beaker to suspend the precipitate. Carefully pour the entire contents, a portion at a time, onto the filter paper. 9. Rinse the reaction beaker several times with distilled water, using a wash bottle, and pour the rinse through the filter paper to capture all the precipitate. 10. Rinse the precipitate on the filter paper with more distilled water from the wash bottle to be sure that all the dissolved materials have been removed. 11. When the filtrate stops dripping from the funnel, carefully remove the filter paper from the funnel and place it in a drying oven overnight. 12. After the precipitate has dried, measure the mass of the filter paper and precipitate. Record the mass in your data table. 13. Dispose of the precipitate as instructed by your teacher. Analyze and Interpret 1. a. What is the solid precipitate that formed in this reaction? b. Which reactant was the limiting reactant, and which was the excess reactant? c. Calculate the theoretical yield of the precipitate, in grams, using the actual recorded masses. d. Compare the mass of the precipitate you collected (the actual yield) with the expected theoretical yield. Describe any differences. 2. Calculate the percentage yield of this reaction. Conclude and Communicate 3. How might reaction procedures and laboratory techniques have affected the percentage yield of this reaction? Explain your reasoning. Extend Further 4. INQUIRY Design new steps for this investigation to improve the laboratory techniques and possibly improve the percentage yield. State the safety precautions that you should take. With your teacher s permission, redo this investigation using your new steps. Calculate the actual percentage yield, and compare it with the original actual percentage yield. 5. RESEARCH Sodium carbonate is commonly called soda ash or washing soda. Research sodium carbonate as a green alternative for cleaning clothes. Write a short summary of your findings. 1 2 Fold a piece of fluted filter paper. a. b. c. d. Fold the filter paper in half. Make creases in the half to divide it into eight sections of equal size. Flip the piece over. Make a fan shape by folding each section in the direction opposite to the previous direction. Place your fluted filter paper in the plastic funnel. Use your washbottle to add a little distilled water to the centre of the filter paper so that it will stay in place. 3 Set up the filtration apparatus as shown. The diagram also shows how to pour the liquid down a stirring rod to ensure no product is lost. ring clamp retort stand filter paper Open up the two halves. You have now fluted your filter paper. funnel Erlenmeyer flask Chapter 7 Chemical Reactions and Stoichiometry MHR 327
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