**Problem Statement:**Determine ΔG° for a reaction when ΔG = -168.4 kJ/mol and Q = 0.035 at 223 K. (R = 8.314 J/mol · K)**Solution Explanation:**To find ΔG°, we use the formula:\[ΔG = ΔG° + RT \ln Q\]Where:- ΔG is the Gibbs free energy change for the reaction.- ΔG° is the standard Gibbs free energy change.- R is the universal gas constant (8.314 J/mol·K).- T is the temperature in Kelvin.- Q is the reaction quotient.**Steps to Solve:**1. Convert units if necessary: - Since ΔG is given in kJ/mol, convert it to J/mol: \(-168.4 \, \text{kJ/mol} = -168400 \, \text{J/mol}\).2. Plug in the known values and solve for ΔG°:\[-168400 = ΔG° + (8.314)(223) \ln 0.035\]3. Calculate \(\ln 0.035\) and the entire RT ln Q term.4. Rearrange the equation to solve for ΔG°.This process will yield the standard Gibbs free energy change, ΔG°, for this particular reaction at the specified conditions.

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Determine AG° for a reaction when AG = -168.4 kJ/mol and Q = 0.035 at 223 K. (R = 8.314 J/mol · K)

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

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Question

**Problem Statement:**

Determine ΔG° for a reaction when ΔG = -168.4 kJ/mol and Q = 0.035 at 223 K.
(R = 8.314 J/mol · K)

**Solution Explanation:**

To find ΔG°, we use the formula:

\[
ΔG = ΔG° + RT \ln Q
\]

Where:
- ΔG is the Gibbs free energy change for the reaction.
- ΔG° is the standard Gibbs free energy change.
- R is the universal gas constant (8.314 J/mol·K).
- T is the temperature in Kelvin.
- Q is the reaction quotient.

**Steps to Solve:**

1. Convert units if necessary:
- Since ΔG is given in kJ/mol, convert it to J/mol:
\(-168.4 \, \text{kJ/mol} = -168400 \, \text{J/mol}\).

2. Plug in the known values and solve for ΔG°:

\[
-168400 = ΔG° + (8.314)(223) \ln 0.035
\]

3. Calculate \(\ln 0.035\) and the entire RT ln Q term.

4. Rearrange the equation to solve for ΔG°.

This process will yield the standard Gibbs free energy change, ΔG°, for this particular reaction at the specified conditions.

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