KCET · Chemistry · Electrochemistry

The equilibrium constant of a reaction is \(0.008\) at \(298 \mathrm{~K}\). The standard free energy change of the reaction at the same temperature is

A \(-11.96 \mathrm{~kJ}\)
B \(-5.43 \mathrm{~kJ}\)
C \(-8.46 \mathrm{~kJ}\)
D + \(11.96 \mathrm{~kJ}\)

Verified Solution

Answer & Solution

Correct Answer

(D) + \(11.96 \mathrm{~kJ}\)

Step-by-step Solution

Detailed explanation

Standard free energy change,
\(\begin{aligned} \Delta \mathrm{G}^{\circ} &=-2.303 \mathrm{RT} \log \mathrm{K} \\ &=-2.303 \times 8.314 \times 298 \times \log 0.008 \\ &=-2.303 \times 8.314 \times 298 \times(3 \log 2-3 \log 10) \\ &=-2.303 \times 8.314 \times 298 \times(0.903-3.0) \\ &=-2.303 \times 8.314 \times 298 \times(-2.097) \\ &=+11965.16 \mathrm{~J}=+11.96 \mathrm{~kJ} \end{aligned}\)

Apply the relevant identity from the chapter and substitute the values established in the previous step, keeping the original constraint in view.

Use the simplified expression to isolate the unknown, then plug the result back into the question setup to confirm the working is internally consistent.

Cross-check against a boundary or limiting case. Both the dimensional balance and the qualitative behaviour at the extreme should agree with the candidate answer.

Combine the steps above to identify the correct option. The remaining choices each fail at least one of the consistency, dimensional, or boundary checks.

Same subject

Explore more questions on app

From KCET

Explore more questions on app