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Chemistry: Principles and Reactions

8th Edition
William L. Masterton + 1 other
ISBN: 9781305079373

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BuyFindarrow_forward

Chemistry: Principles and Reactions

8th Edition
William L. Masterton + 1 other
ISBN: 9781305079373
Textbook Problem

At a certain temperature, K = 0.29 for the decomposition of two moles of iodine trichloride, ICl3(s), to chlorine and iodine gases. The partial pressure of chlorine gas at equilibrium is three times that of iodine gas. What are the partial pressures of iodine and chlorine at equilibrium?

Interpretation Introduction

Interpretation:

The partial pressure of the iodine and chlorine gas at equilibrium needs to be determined.

Concept introduction:

For a general equilibrium reaction as follows:

A(g)+B(g)C(g)+D(g)

The expression for the equilibrium constant is represented as follows:

K=(PC)(PD)(PA)(PB)

Here, to calculate the equilibrium constant, the values of partial pressure of all the species in reactant and product side are required.

Explanation

The equilibrium constant for the reaction is 0.29. The equilibrium reaction for decomposition of 2 mol of the ICl3 can be shown as follows:

2ICl3(s)3Cl2(g)+I2(g)

The partial pressure of Cl2 is three times the partial pressure of I2.

Or,

PCl2=3PI2

The expression for the equilibrium constant will be:

K=(PCl2)3(PI2)

Or,

K=(3PI2)3(PI2)=3(PI2)4

Putting the values,

0

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