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Question

For the reaction at 298 K,

2A + B → C

ΔH = 400 kJ mol–1 and ΔS = 0.2 kJ K–1 mol–1

At what temperature will the reaction become spontaneous considering ΔH and ΔS to be constant over the temperature range?

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Solution

From the expression,

ΔG = ΔHTΔS

Assuming the reaction at equilibrium, ΔT for the reaction would be:

G = 0 at equilibrium)

T = 2000 K

For the reaction to be spontaneous, ΔG must be negative. Hence, for the given reaction to be spontaneous, T should be greater than 2000 K.


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