Calculations with a Chemical Reaction
Purpose:
-Observe the reaction between solutions of CaCl2 and Na2CO3, forming insoluble CaCO3
-Determine the theoretical amount of CaCO3 produced from the starting reactants
-Calculate the percent yield of CaCO3
Materials:
Balance 0.60 M Na2CO3 solution
100 ml glass graduated cylinder 0.40 M CaCl2 solution
100 ml plastic graduated cylinder deionized water
funnel
filter paper
2 beakers(250 ml)
stirring rod with rubber scraper
Ring stand with ring support
Safety:
-Follow general safety procedures and be sure to wear goggles
Pre-Lab:
A student performed a lab which involved the production of 1.52 g of copper and an aqueous iron(II)sulfate by heating aqueous solution containing 8.00 g of copper(II) sulfate with 1.40 g of solid iron.
1. Write a balanced chemical equation for this reaction. What type of reaction is this?
2. Calculate the number of moles of copper(II) sulfate and iron that reacted in this lab.
3. Calculate the number of moles of copper that were produced when the iron reacted with the copper(II) sulfate solution.
4. Determine the limiting and excess reagents in this reaction.
5. Calculate the amount of copper that should theoretically form from this reaction.
6. Calculate the percent yield of copper in this reaction.
Procedure:
Part One
1. Pour approximately 35 ml of Na2CO3 solution into the
plastic 100 ml graduated cylinder. Record the volume to
the nearest 0.1 ml. Record the volume in the data table.
Pour the Na2CO3 solution into the 250 ml beaker.
2. Pour approximately 25 ml of CaCl2 solution into the
glass 100 ml graduated cylinder. Record the volume to
the nearest 0.1 ml. Record the volume in the data table.
Pour the CaCl2 solution into the 250 ml beaker with the
Na2CO3 solution. Stir the contents of the beaker
for about one minute, then allow the solid to settle.
3. While waiting for the solid to settle, find the mass of a
piece of filter paper and record the amount in the data table.
4. Set up a funnel and the filter paper of known mass as Figure 1
shown in Figure 1. Place the second beaker under the funnel.
5. Wet the filter paper with a small amount of distilled water. Pour the contents of the beaker from step 2 slowly into the funnel. Be careful as you pour, so that none of the solid flows out of the filter paper or funnel. Use the rubber scraper to remove as much of the solid from the beaker as possible. Rinse the inside of the beaker with some distilled water to remove as much solid as possible. Rinse again to ensure the entire solid has been removed.
6. Once the entire solid is on the filter paper and all the liquid has drained into the beaker, carefully remove the filter paper from the funnel and unfold it onto a paper towel. Put your name on the paper towel and place in the designated area for drying.
7. Clean your lab area and wash your hands before returning to your desk.
Part Two
1. Find the mass of the precipitate and filter paper and record the amount in the data table.
Data and Analysis:
Create a data table to record the following information: Volume of Na2CO3 solution, Volume of CaCl2 solution, Mass of dry filter paper and Mass of filter paper + dry solid
Conclusion Questions
FOR ALL CALCULATIONS-SHOW YOUR WORK!!!
1. Calculate the moles of sodium carbonate used.
2. Calculate the moles of calcium chloride used.
3. Calculate the mass of calcium carbonate produced.
4. Calculate the moles of calcium carbonate produced.
5. Write a balanced chemical equation for the reaction observed in this experiment.
6. Determine which of the reactants was the limiting reagent? Which was the excess reagent?
7. Calculate the amount of calcium carbonate that should theoretically form from the amount of the limiting reagent.
8. Calculate the percent yield for your reaction.
Conclusion Questions
FOR ALL CALCULATIONS-SHOW YOUR WORK!!!
1. Calculate the moles of sodium carbonate used.
2. Calculate the moles of calcium chloride used.
3. Calculate the mass of calcium carbonate produced.
4. Calculate the moles of calcium carbonate produced.
5. Write a balanced chemical equation for the reaction observed in this experiment.
6. Determine which of the reactants was the limiting reagent? Which was the excess reagent?
7. Calculate the amount of calcium carbonate that should theoretically form from the amount of the limiting reagent.
8. Calculate the percent yield for your reaction.
Conclusion Questions
FOR ALL CALCULATIONS-SHOW YOUR WORK!!!
1. Calculate the moles of sodium carbonate used.
2. Calculate the moles of calcium chloride used.
3. Calculate the mass of calcium carbonate produced.
4. Calculate the moles of calcium carbonate produced.
5. Write a balanced chemical equation for the reaction observed in this experiment.
6. Determine which of the reactants was the limiting reagent? Which was the excess reagent?
7. Calculate the amount of calcium carbonate that should theoretically form from the amount of the limiting reagent.
8. Calculate the percent yield for your reaction.
Calculations with a Chemical Reaction
Intro: Date, Table of Contents, Purpose, Materials, Safety
Pre-Lab:
A student performed a lab which involved the production of 1.52 g of copper and an aqueous iron(II)sulfate by heating aqueous solution containing 8.00 g of copper(II) sulfate with 1.40 g of solid iron.
1. Write a balanced chemical equation for this reaction. What type of reaction is this?
2. Calculate the number of moles of copper(II) sulfate and iron that reacted in this lab.
3. Calculate the number of moles of copper that were produced when the iron reacted with the copper(II) sulfate solution.
4. Determine the limiting and excess reagents in this reaction.
5. Calculate the amount of copper that should theoretically form from this reaction.
6. Calculate the percent yield of copper in this reaction.
Procedure:
Data and Analysis:
Conclusion:
1. Calculate the moles of sodium carbonate used.
2. Calculate the moles of calcium chloride used.
3. Calculate the mass of calcium carbonate produced.
4. Calculate the moles of calcium carbonate produced.
5. Write a balanced chemical equation for the reaction observed in this experiment.
6. Determine which of the reactants was the limiting reagent? Which was the excess reagent?
7. Calculate the amount of calcium carbonate that should theoretically form from the amount of the limiting reagent.
8. Calculate the percent yield for your reaction.