AP EAMCET · Chemistry · Thermodynamics (C)

What is the nature of reaction at $298 K$ , if the entropy change and enthalpy change for a chemical reaction are $7.4 cal$ $K^{- 1}$ and $- 2.5 \times 10^{3} cal$ , respectively.

A Reversible
B Spontaneous
C Non-Spontaneous
D Irreversible

Verified Solution

Answer & Solution

Correct Answer

(B) Spontaneous

Step-by-step Solution

Detailed explanation

As Gibbs free energy tells us about the spontenity of the reaction which is calculated as: ∆G=∆H-T∆S∆G=(-2.5×103) - 298×7.4∆G=-4705.2 cal As, Gibbs free energy is negative. So, reaction is spontaneous.

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.

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What is the nature of reaction at 298 K, if the entropy change and enthalpy change for a chemical reaction are 7.4 cal K-1 and-2.5×103 cal, respectively.

Step-by-step Solution

What is the nature of reaction at $298 K$ , if the entropy change and enthalpy change for a chemical reaction are $7.4 cal$ $K^{- 1}$ and $- 2.5 \times 10^{3} cal$ , respectively.