If $\Delta$ for a reaction is -2.03 kJ/mol, what is K for the reaction at 300 K?

Name: If $\Delta$ for a reaction is -2.03 kJ/mol, what is K for the reaction at 300 K?
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Question

Quizplus · Accepted Answer

We can use the formula:
ΔG = -RT ln K
where ΔG = -102.03 kJ/mol, R = 8.314 J/(mol*K), and T = 300 K.

Plugging in the values, we get:
-102.03 kJ/mol = -8.314 J/(mol*K) * 300 K * ln K
Simplifying, we get:
ln K = 12.348
K = e^(12.348) = 2.26

Therefore, the answer is D) 2.26.

If Δ\DeltaΔ For a Reaction Is -2 ×\times× 107 B)5 ×\times× 10-5 C)1