Chemistry-Gibbs Free Energy
NEET Chemistry Gibbs Free Energy MCQ Question
Type: MCQ-numerical-Easy-Class 11
Given that the standard Gibbs energy change, ∆rG° at a certain temperature is -13.6 kJ mol–1, which of the following best expresses the relationship between the equilibrium constant (K) and Gibbs energy?
A
log K = -∆rG° / 2.303RT
B
log K = ∆rG° / 2.303RT
C
log K = -2.303RT / ∆rG°
D
log K = 2.303RT / ∆rG°
Correct Answer
Option A
Detailed Explanation
The relationship is derived from the equation ∆rG° = -RT ln K, which can be expressed as log K = -∆rG° / 2.303RT by converting to base 10 logarithms.
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