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For a certain reaction, ΔH0 = -224 kJ and ΔS0 = -153 JK-1. At what temperature will it change from spontaneous to non-spontaneous?

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Given : 

ΔH0 = – 224 kJ = – 224000 J

ΔS0 = – 153 JK-1

Temperature (T) at which, reaction changes from spontaneous to non-spontaneous = ? 

Find the temperature at equilibrium, where ΔG0 = 0

ΔG0 = ΔH0 - TΔS0

0 = ΔH0 – TΔS0

∴ TΔS0 = ΔH0

∴ T = \(\frac{ ΔH^0}{ ΔS^0}\)

\(\frac{224000}{153}\)

= 1464 K.

Hence reaction will be spontaneous below 1464 K. It will be at equilibrium at 1464 K and non-spontaneous above 1464 K.

∴ Change over temperature from spontaneous to non-spontaneous = 1464 K.

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