# An equilibrium mixture contains 0.60 g solid carbon and the gases carbon dioxide and carbon monoxide at partial pressures of 2.60 atm and 2.89 atm, respectively. Calculate the value of K p for the reaction C ( s ) + CO 2 ( g ) ⇌ 2 CO ( g )

### Chemistry: An Atoms First Approach

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

Chapter
Section

### Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243
Chapter 12, Problem 92CWP
Textbook Problem
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## An equilibrium mixture contains 0.60 g solid carbon and the gases carbon dioxide and carbon monoxide at partial pressures of 2.60 atm and 2.89 atm, respectively. Calculate the value of Kp for the reaction C ( s ) + CO 2 ( g ) ⇌ 2 CO ( g )

Interpretation Introduction

Interpretation: For the given reaction the equilibrium constant in terms of partial pressure is to be calculated.

Concept introduction: The equilibrium constant Kp describes the ratio of the reactant to the product on the equilibrium conditions in terms of partial pressure.

The equilibrium constant depends upon temperature.

Law of mass action is applicable on the equilibrium reactions.

To determine: The value of equilibrium constant for the given reaction.

### Explanation of Solution

Explanation

Given

The reaction is given as,

C(s)+CO2(g)2CO(g)

The equilibrium partial pressure of CO2(g) is 2.60atm .

The equilibrium partial pressure of CO(g) is 2.89atm .

The Carbon species is present in solid state; therefore, the equilibrium partial pressure for Carbon is taken as unity.

The equilibrium constant for the given reaction is calculated by the formula,

Kp=PCO2PCO2

Where,

• Kp is the equilibrium constant in terms of partial pressure

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