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A certain reaction is non-spontaneous at 298K. The entropy change during the reaction is 121 JK^–1. Is the reaction is endothermic or exothermic? The minimum value of ΔH for the reaction is

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A certain reaction is non-spontaneous at 298K. The entropy change during the reaction is 121 JK–1. Is the reaction is endothermic or exothermic? The minimum value of ΔH for the reaction is

(a) endothermic, ΔH = 36.06 kJ

(b) exothermic, ΔH = -36.06 kJ

(c) endothermic, ΔH = 60.12 kJ

(d) exothermic, ΔH = -60.12 kJ

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Correct answer: (a) endothermic, ΔH = 36.06 kJ

Explanation:

For non spontaneous reaction

ΔG = + ve

ΔG = ΔH – TΔS and

ΔS = 121 JK-1

For ΔG = +ve

ΔH has to be positive. Hence the reaction is endothermic.

The minimum value of ΔH can be obtained by putting ΔG = 0

ΔH = TΔS = 298 × 121 J

= 36.06 kJ

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