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Question

ΔH and ΔS for the system
H2O(l)H2O(g)
at 1 atmospheric pressure are 40.63 kJmol1 and 108.8 JK1mol1 respectively. Calculate the temperature at which the rates of forward and backward reactions will be the same. Predict the sign of free energy for this transformation above this temperature.

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Solution

Given, ΔH=40.63kJmol1
ΔS=108.8JK1mol1=0.1088kJK1mol1
ΔG=0 (when the system is in equilibrium)
Applying ΔG=ΔHTΔS
The sign of ΔG above 373K, say 374K may be calculated as follows
Again applying ΔG=ΔHTΔS
40.63374×0.1088
=0.06kJ
ΔG will be negative; hence the reaction will be spontaneous.

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