NCERT Class XI Chemistry Thermodynamics Solutions
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Question : 17
Total: 22
For the reaction at 298 K, 2A + B → C, ΔH = 400 k J m o l – 1 and ΔS = 0.2 k J K – 1 m o l – 1 . At what temperature will the reaction become spontaneous considering ΔH and ΔS to be constant over the temperature range.
Solution:
According to Gibbs Helmholtz equation, ΔG = ΔH – TΔS.
At equilibrium, ΔG = 0
∴ T =
=
=
= 2000 K
Thus, the reaction will be spontaneous at temperature above 2000 K.
[Since Above 2000 K, ΔG = –ve]
At equilibrium, ΔG = 0
∴ T =
Thus, the reaction will be spontaneous at temperature above 2000 K.
[Since Above 2000 K, ΔG = –ve]
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