   # The equilibrium constant for a certain reaction increases by a factor of 6.67 when the temperature is increased from 300.0 K to 350.0 K. Calculate the standard change in enthalpy (∆ H °) for this reaction (assuming ∆ H ° is temperature-independent). ### 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 16, Problem 102CWP
Textbook Problem
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## The equilibrium constant for a certain reaction increases by a factor of 6.67 when the temperature is increased from 300.0 K to 350.0 K. Calculate the standard change in enthalpy (∆H°) for this reaction (assuming ∆H° is temperature-independent).

Interpretation Introduction

Interpretation: The standard enthalpy change of the reaction with the given values of increase in temperature and increase in equilibrium constant is to be calculated.

Concept Introduction: The relation between standard enthalpy change, temperature and equilibrium constant is determined by the formula,

ln(K2K1)=ΔHR(1T21T1)

To determine: The standard enthalpy change of the given reaction.

### Explanation of Solution

Given

The equilibrium constant of the reaction increases by 6.67 .

The initial temperature of the reaction is 300.0K .

The final temperature of the reaction is 350.0K .

The standard enthalpy change of the given reaction is calculated by using the formula,

ln(K2K1)=ΔHR(1T21T1)

Where,

• K1 is the initial equilibrium constant of the reaction.
• K2 is the final equilibrium constant of the reaction.
• ΔH is the standard enthalpy change of the reaction.
• R is the gas constant

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