When solutions containing 1.0000 g of BaCl2 and 1.0000 g of Na2SO4 were mixed, solid BaSO4 formed. The BaSO4 precipitate was filtered out of the solution, allowed to dry, and then weighed. The mass of BaSO4 that was isolated from solution was 1.0400 g. Use this information to answer the following questions. Pay close attention to the proper use and reporting of significant figures and units. You must show all of your work (i.e., your calculations) for full credit.
(a) Write a balanced chemical equation that shows the reaction that occurs when an aqueous solution of BaCl2 reacts with an aqueous solution of Na2SO4 to form aqueous sodium chloride and solid BaSO4. In your equation, you should indicate the physical states of each reactant and product. Note: Precipitation reactions are discussed in Section 4.6 of your textbook.
(b) Calculate the moles of BaCl2 that are available for reaction.
(c) Calculate the grams of BaSO4 that should form if all of the available BaCl2 reacts.
(d) Calculate the moles of Na2SO4 that are available for reaction.
(e) Calculate the grams of BaSO4 that should form if all of the available Na2SO4 reacts.
(f) Which reactant (BaCl2 or Na2SO4) is the limiting reagent in this reaction? Why?
(g) What is the theoretical yield of BaSO4?
(h) What is the percent yield of BaSO4? (See Section 4.3 of your textbook for information regarding the calculation of a percent yield.)
(i) If this reaction went to completion, then how many grams of the excess reagent should remain after the reaction is complete?
When solutions containing 1.0000 g of BaCl2 and 1.0000 g of Na2SO4 were mixed, solid BaSO4 formed. The BaSO4 precipitate was filtered out of the solution, allowed to dry, and then weighed. The mass of BaSO4 that was isolated from solution was 1.0400 g. Use this information to answer the following questions. Pay close attention to the proper use and reporting of significant figures and units. You must show all of your work (i.e., your calculations) for full credit.
(a) Write a balanced chemical equation that shows the reaction that occurs when an aqueous solution of BaCl2 reacts with an aqueous solution of Na2SO4 to form aqueous sodium chloride and solid BaSO4. In your equation, you should indicate the physical states of each reactant and product. Note: Precipitation reactions are discussed in Section 4.6 of your textbook.
(b) Calculate the moles of BaCl2 that are available for reaction.
(c) Calculate the grams of BaSO4 that should form if all of the available BaCl2 reacts.
(d) Calculate the moles of Na2SO4 that are available for reaction.
(e) Calculate the grams of BaSO4 that should form if all of the available Na2SO4 reacts.
(f) Which reactant (BaCl2 or Na2SO4) is the limiting reagent in this reaction? Why?
(g) What is the theoretical yield of BaSO4?
(h) What is the percent yield of BaSO4? (See Section 4.3 of your textbook for information regarding the calculation of a percent yield.)
(i) If this reaction went to completion, then how many grams of the excess reagent should remain after the reaction is complete?
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