   Chapter 4, Problem 19PS

Chapter
Section
Textbook Problem

In Example 4.2, you found that a particular mixture of CO and H2 could produce 407 g CH3OH.CO(g) + 2H2(g) → CH3OH (l)If only 332 g of CH3OH is actually produced, what is the percent yield of the compound?

Interpretation Introduction

Interpretation:

Mass percentage of methanol produced in the given reaction has to be determined.

Concept introduction:

• 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.
• Mass percentage of reacted mass in the original sample is the ratio of mass of substance reacted to mass of whole sample taken.
• For chemical reaction balanced chemical reaction equation written in accordance with the Law of conservation of mass.
• Law of conservation of mass states that for a reaction total mass of the reactant and product must be equal.
Explanation

Balanced chemical equation for the given reaction is,

CO(g)+2H2(g)CH3OH(l)

To find the mass of product formed in the reaction, the amount of each reactant involved in the given reaction should be determined.

Therefore,

AmountofCO=356gCO×1molCO28.01gCO=12.71molCOAmountofH2=65.0gH2×1molH22.016gH2=32.24molH2

The mass of product (methanol) expected based on each reactant is,

12.71molCO×1molCH3OHformed1molCOavailable×32

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