Given the following balanced chemical equation: 2 CO(g) + O2(g) 2CO2(g) 15.0 g of CO(g) and 15.0 g of O2(g) placed in this reaction a) Determine the limiting and excess reactant. Calculate the mass of product produced to support your answers. b) If 1.52 g of CO2(g) produced at the end of the reaction, what is the percent yield? Percent yield actual yield theoretical yield x 100 c) Calculate the mass of the excess reactant left over.
Given the following balanced chemical equation: 2 CO(g) + O2(g) 2CO2(g) 15.0 g of CO(g) and 15.0 g of O2(g) placed in this reaction a) Determine the limiting and excess reactant. Calculate the mass of product produced to support your answers. b) If 1.52 g of CO2(g) produced at the end of the reaction, what is the percent yield? Percent yield actual yield theoretical yield x 100 c) Calculate the mass of the excess reactant left over.
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter3: Chemical Reactions
Section: Chapter Questions
Problem 73QRT
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![Given the following balanced chemical equation:
2 CO(g) + O2(g) 2CO2(g)
15.0 g of CO(g) and 15.0 g of O2(g) placed in this reaction
a) Determine the limiting and excess reactant. Calculate the mass of product produced to support
your answers.
b) If 1.52 g of CO2(g) produced at the end of the reaction, what is the percent yield?
actual yield
Percent yield
x 100
theoretical yield
c) Calculate the mass of the excess reactant left over.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F11c3e735-47a2-4be2-bcf0-76944b0744ea%2Fe54a254c-847b-4f07-9242-c9059b26ab7b%2Fcvzxubm_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Given the following balanced chemical equation:
2 CO(g) + O2(g) 2CO2(g)
15.0 g of CO(g) and 15.0 g of O2(g) placed in this reaction
a) Determine the limiting and excess reactant. Calculate the mass of product produced to support
your answers.
b) If 1.52 g of CO2(g) produced at the end of the reaction, what is the percent yield?
actual yield
Percent yield
x 100
theoretical yield
c) Calculate the mass of the excess reactant left over.
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