Calculate the entropy change in surroundings when 1.00 mol of H2
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The equilibrum constant for a reaction is 10. What will be the value of ∆G0 ? R = 8.314 JK–1 mol–1, T = 300 K. 

We know, 
        

Substituting the values, we get,

         

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Calculate the entropy change in surroundings when 1.00 mol of H2O(l) is formed under standard conditions. ∆fH0 = –286 kJ mol–1.


The thermochemical equation is,


From the above equation, it is clear that when 1 mol of H2O(l) is formed, 286 kJ of heat is released. The same amount of heat is absorbed by the surroundings.

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