   # At 327 ο c, the equilibrium concentrations are [CH 3 OH] = 0.15 M, [CO] = 0.24 M, and [H 2 ] = 1.1 M for the reaction CH 3 OH ( g ) ⇌ CO ( g ) + 2 H 2 ( g ) Calculate K p at this temperature ### 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 12, Problem 31E
Textbook Problem
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## At 327οc, the equilibrium concentrations are [CH3OH] = 0.15 M, [CO] = 0.24 M, and [H2] = 1.1 M for the reaction CH 3 OH ( g ) ⇌ CO ( g ) + 2 H 2 ( g ) Calculate Kp at this temperature

Interpretation Introduction

Interpretation: The equilibrium concentration values for the species involved in the stated reaction are given. The value of the equilibrium constant (Kp) for the reaction is to be calculated.

Concept introduction: The state when the reactants involved in a chemical reaction and the products formed in the reaction exist in concentrations having no further tendency to change is known as an equilibrium state of the reaction. When the equilibrium constant is expressed in terms of pressure, it is represented Kp .

To determine: The equilibrium constant (K) for the given reaction.

### Explanation of Solution

Given

The stated reaction is,

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

The concentration of [CH3OH(g)] is 0.15M .

The concentration of [CO(g)] is 0.24M .

The concentration of [H2(g)] is 1.1M .

At equilibrium, the equilibrium ratio is expressed by the formula,

K=ConcentrationofproductsConcentrationofreactants

Where,

• K is the equilibrium constant.

The equilibrium ratio for the given reaction is,

K=[CO][H2]2[CH3OH]

Substitute the given concentration values in the above expression.

K=[CO][H2]2[CH3OH]=[0.24][1.1]2[0.15]=1.936_

To determine: The equilibrium constant (Kp) for the given reaction.

The relation between ‘ K ’ and ‘ Kp ’ is,

Kp=K(RT)Δn (1)

Where,

• R is the gas constant

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