A) The entropy change is negative
B) Equilibrium constant is greater than one
C) The reaction should be instantaneous
D) The reaction is thermodynamically not feasible
Correct Answer: B
Solution :
In the reversible reaction, \[A(s)+B(g)C(g)+D(g);\] \[\Delta {{G}^{o}}=-350\,kJ\] Since, the randomness increases (because solid is changing into gas), entropy will increase and thus, \[\Delta S\] is positive. Reversible reaction never undergo to completion (ie, never be instantaneous). \[\because \] For the given reaction, \[\Delta {{G}^{o}}=-350\,kJ\] and we know that \[\Delta {{G}^{o}}=-RT\,\log \,K\] \[-350=-RT\,\log \,K\] ie, K (equilibrium constant) is greater than one. Moreover, the reaction is thermodynamically feasible.
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