For a given reaction, H = 35.5 kJ mol^-1 and S = 83.6 JK^-1mol^-1 . The reaction is spontaneous at (Assume that H and S do not vary with temperature): - Chemistry MCQ NEET 2017 2026 | ExamTest.live

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For a given reaction, Δ H = 35.5 kJ mol^{- 1} and Δ S = 83.6 JK^{- 1} mol^{- 1} . The reaction is spontaneous at (Assume that Δ H and Δ S do not vary with temperature):

Solution & Step-by-step Explanation

For a reaction to be spontaneous, Δ G < 0 . Δ H - T Δ S < 0 ⟹ Δ H < T Δ S ⟹ T > \frac{Δ H}{Δ S} . T > \frac{35500 J/mol}{83.6 J/K \cdot mol} T > 424.64 K \approx 425 K .

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For a given reaction, Δ H = 35.5 kJ mol^{- 1} and Δ S = 83.6 JK^{- 1} mol^{- 1} . The reaction is spontaneous at (Assume that Δ H and Δ S do not vary with temperature):

T < 425 K

T > 425 K

All temperatures

T > 298 K

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