### Calculation of ΔG° for the Dissociation of Lead(II) Iodide in Water**Problem Statement:**Calculate ΔG° at 298K for the dissociation of lead(II) iodide in water given that the equilibrium constant is 1.4 x 10⁻⁸.**Options:**A. 45 kJ B. 18 kJ C. 1125 kJ D. 2478 kJ E. 137 kJ To solve this problem, you need to use the relationship between the Gibbs free energy change (\(\Delta G°\)) and the equilibrium constant (K) as given by the equation:\[\Delta G° = -RT \ln K\]Where:- \(R\) is the gas constant, which is approximately 8.314 J/(mol·K).- \(T\) is the temperature in Kelvin.- \(K\) is the equilibrium constant.Given:- \(T = 298\) K- \(K = 1.4 \times 10^{-8}\)Calculate \(\Delta G°\) as follows:1. Convert K into natural logarithm form.2. Multiply by the gas constant and temperature.3. Adjust units to kJ.This understanding will help you arrive at the correct option from the provided multiple choices.*Note: The above details are for educational purposes to help understand the thermodynamic calculation involved in chemical equilibrium.*

Answered: Calculate AG, at 298K, for the…

Calculate AG, at 298K, for the dissociation of lead(II) iodide in water given that the equilibrium constant is 1.4 x 108.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Question

### Calculation of ΔG° for the Dissociation of Lead(II) Iodide in Water

**Problem Statement:**

Calculate ΔG° at 298K for the dissociation of lead(II) iodide in water given that the equilibrium constant is 1.4 x 10⁻⁸.

**Options:**

A. 45 kJ
B. 18 kJ
C. 1125 kJ
D. 2478 kJ
E. 137 kJ

To solve this problem, you need to use the relationship between the Gibbs free energy change (\(\Delta G°\)) and the equilibrium constant (K) as given by the equation:

\[
\Delta G° = -RT \ln K
\]

Where:
- \(R\) is the gas constant, which is approximately 8.314 J/(mol·K).
- \(T\) is the temperature in Kelvin.
- \(K\) is the equilibrium constant.

Given:
- \(T = 298\) K
- \(K = 1.4 \times 10^{-8}\)

Calculate \(\Delta G°\) as follows:

1. Convert K into natural logarithm form.
2. Multiply by the gas constant and temperature.
3. Adjust units to kJ.

This understanding will help you arrive at the correct option from the provided multiple choices.

*Note: The above details are for educational purposes to help understand the thermodynamic calculation involved in chemical equilibrium.*

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The standard Gibbs free energy and equilibrium constant are related by the following formula.

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