   # Methanol (CH 3 OH) can be produced by the following reaction: CO ( g ) + 2H 2 ( g ) → CH 3 OH ( g ) Hydrogen at STP flows into a reactor at a rate of 16.0 L/min. Carbon monoxide at STP flows into the reactor at a rate of 25.0 L/min. If 5.30 g methanol is produced per minute, what is the percent yield of the reaction? ### Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243

#### Solutions

Chapter
Section ### Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243
Chapter 8, Problem 95E
Textbook Problem
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## Methanol (CH3OH) can be produced by the following reaction: CO ( g )   +  2H 2 ( g )   →  CH 3 OH ( g ) Hydrogen at STP flows into a reactor at a rate of 16.0 L/min. Carbon monoxide at STP flows into the reactor at a rate of 25.0 L/min. If 5.30 g methanol is produced per minute, what is the percent yield of the reaction?

Interpretation Introduction

Interpretation: The percent yield of the given reaction is to be determined if the actual yield of methanol is 5.3g and volumes of H2 and CO are given as 16L and 25L respectively.

Concept introduction:

• Balance equation of a reaction is written according to law of conservation of mass.
• Number of moles of a substance, According to ideal gas equation,

Numberofmoles=Pressure×VolumeR×Temperature

• Mole ratios between the reactant and a product of a reaction are depends upon the coefficients of reactant and product in a balanced chemical equation.
• mass of a substance from its number of moles is,

Number of moles×Molecularmass in grams=producedmass

• Percent yield of reaction is the ratio of mass of actual yield to the mass of theoretical yield.
• Limiting reagent: limiting reagent is a reactant, which consumes completely in the chemical reaction. The quantity of the product depends on this limiting reagent, it can be determined with the help of balanced chemical equation for the reaction.

### Explanation of Solution

Explanation

• To find: the number of moles of H2 gas and CO reacted in the given reaction.

The number of moles of H2 gas is 16PRTmol .

The number of moles of CO gas is 25PRTmol .

The volume of H2 in the given reaction is given as 16L .

The volume of CO in the given reaction is given as 25L .

The equation for finding number of moles of a substance, According to ideal gas equation,

Numberofmoles=Pressure×VolumeR×Temperature

The pressure, temperature and R-value are constant for both H2 and CO in the given reaction.

Hence,

The pressure is taken as P .

The temperature is taken as T .

The value of R is taken as R .

Therefore,

The number of moles of H2 in the given reaction is,

nH2=16PRTmol

The number of moles of CO in the given reaction is,

nCO=25PRTmol

• To find: the limiting reagent in the given reaction of H2 and CO .

H2 is the limiting reagent in the given reaction.

The number of moles of H2 gas is calculated as 16PRTmol .

The number of moles of CO gas is calculated as 25PRTmol .

The balance equation of given reaction is CO+2H2CH3OH , here 1 mole of CO requires 2 moles of H2 .

Therefore,

The 25PRTmolofCO requires2×25PRTmolofH2 .

The given number of moles of H2 gas is 16PRTmol only.

Hence, H2 is the limiting reagent in the given reaction.

• To find: the mole ratio between CH3OH and H2 in the given reaction and the number of moles of CH3OH produced.

1/2 mole of CH3OH is produced for 1 mole of H2

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