For a given reaction, H = 35.5 kJ mol^-1 and S = 83.6 JK^-1 mol^-1 . The reaction is spontaneous at: (Assume that H and S do not vary with temperature - Chemistry MCQ NEET (UG) 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, the Gibbs free energy change (Δ G) must be negative (Δ G < 0).Using the equation: Δ G = Δ H - T Δ S For spontaneity: Δ H - T Δ S < 0 Δ H < T Δ S T > \frac{Δ H}{Δ S} Given: Δ H = 35.5 kJ mol^{- 1} = 35500 J mol^{- 1} Δ S = 83.6 JK^{- 1} mol^{- 1} $ T > \frac{35500}{83.6} $ T > 424.64 K Rounding to the nearest integer, T > 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

All temperatures

T > 298 K

T < 425 K

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