Question:
For a given reaction, Δ H = 35.5kJ mol⁻1 and Δ S = 83.6J K⁻1mol⁻1.
The reaction is spontaneous at (Assume that Δ H and Δ S do not vary with temperature)
For a given reaction, Δ H = 35.5kJ mol⁻1 and Δ S = 83.6J K⁻1mol⁻1.
The reaction is spontaneous at (Assume that Δ H and Δ S do not vary with temperature)
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If Δ H > 0 and Δ S > 0, reaction is spontaneous only at high temperatures.
Updated On: Mar 19, 2026
- T > 425K
- All temperatures
- T > 298K
- T < 425K
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The Correct Option is A
Solution and Explanation
Step 1: Gibbs free energy:
Δ G = Δ H - TΔ S
Step 2: Convert Δ S to kJ:
Δ S = 0.0836kJ K⁻1mol⁻1
Step 3: For spontaneity, Δ G < 0:
T > (Δ H)/(Δ S) = (35.5)/(0.0836) ≈ 425K
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