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ChemistryChemistry: Principles and Reactions8th Edition
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Consider the reaction 2 HI ( g ) ⇌ H 2 ( g ) + I 2 ( g ) At 500°C a flask initially has all three gases, each at a partial pressure of 0.200 atm. When equilibrium is established, the partial pressure of HI is determined to be 0.48 atm. What is Δ G ° for the reaction at 500°C?

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Chemistry: Principles and Reactions

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

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BuyFindarrow_forward

Chemistry: Principles and Reactions

8th Edition
William L. Masterton + 1 other
Publisher: Cengage Learning
ISBN: 9781305079373
Chapter 16, Problem 100QAP
Textbook Problem
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Consider the reaction

2 HI ( g ) ⇌ H 2 ( g ) + I 2 ( g ) At 500°C a flask initially has all three gases, each at a partial pressure of 0.200 atm. When equilibrium is established, the partial pressure of HI is determined to be 0.48 atm. What is ΔG° for the reaction at 500°C?

Interpretation Introduction

Interpretation:

The value of standard Gibbs free energy change for the reaction needs to be determined.

Concept introduction:

The value of ΔG∘ can be calculated from equilibrium constant as follows:

ΔG∘=−RTlnK

Here, R is Universal gas constant, T is temperature and K is equilibrium constant

Explanation of Solution

The given reaction is as follows:

2HI(g)⇌H2(g)+I2(g)

At 500∘C, all the three gases are present with partial pressure 0.2 atm. The partial pressure of HI at equilibrium is 0.48 atm.

At equilibrium, the partial pressure of HI increases, thus, all the reaction is moving in backward direction as follows:

H2(g)+I2(g)⇌2HI(g)

The change in partial pressure can be represented as follows:

H2(g)+I2(g)⇌2HI(g)0.2          0.2             0.20.2-x       0.2-x           0.2+2x

This is given that at equilibrium, partial pressure of HI is 0.48 atm.

Thus,

0.2+2x=0.48

Or,

x=0.14

Thus, partial pressure of H2 and I2 can be calculated as follows:

PH2=PI2=0

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