5. Given the reaction below, if 200.0 g of each reactant is used, determine the following: 3 NaBr(s) + H3PO4(1)→ 3HBr(g) + Na3PO4(s) a. Which reactant is limiting? b. What is the theoretical yield of each product? c. How much excess reactant will remain unreacted, assuming 100% yield?

5. Given the reaction below, if 200.0 g of each reactant is used, determine the following: 3 NaBr(s) + H3PO4(1)→ 3HBr(g) + Na3PO4(s) a. Which reactant is limiting? b. What is the theoretical yield of each product? c. How much excess reactant will remain unreacted, assuming 100% yield?

Introductory Chemistry: A Foundation

8th Edition

ISBN:9781285199030

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter9: Chemical Quantities

Section: Chapter Questions

Problem 45QAP: For each of the following unbalanced reactions, suppose exactly 5.00 g of each reactant is taken....

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Stoichiometry

Stoichiometry is a chemical division that evaluates the quantitative content of the chemical process with the help of the reacting molecules or products taking part in the reaction. The term “stoicheion” in “Stoichiometry”, is an old Greek term for "element" whereas “metron” means "measure".

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5. Given the reaction below, if 200.0 g of each reactant is used, determine the following:
3 NaBr(s) + H3PO4(1) ➜ 3HBr(g) + Na3PO4(s)
a. Which reactant is limiting?
b. What is the theoretical yield of each product?
c. How much excess reactant will remain unreacted, assuming 100% yield?
d. If the percent yield of the reaction is only 70.0%, what would be the actual yield of each product?

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d) If the percent yield of the reaction is only 70%, what would be the actual yield of each product?

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