A) \[T\Delta S<\Delta H\] and both\[\Delta H\]and\[\Delta S\]are +ve
B) \[T\Delta S>\Delta H\] and both \[\Delta H\] and \[\Delta S\] are +ve
C) \[T\Delta S=\Delta H\] and both \[\Delta H\] and \[\Delta S\] are +ve
D) \[T\Delta S>\Delta H\]and \[\Delta H\] is + ve and \[\Delta S\] is -ve
Correct Answer: B
Solution :
The spontaneity of reaction is based upon the negative value of \[\Delta G,\]\[\Delta G\] is based upon \[T,\]\[\Delta S\]and \[\Delta H\]according to following equation (Gibbs-Helmholtz equation) \[\Delta G=\Delta H-T\Delta S\] If the magnitude of \[\Delta H-T\Delta S\] is negative, then the reaction is spontaneous. when \[T\Delta S>\Delta H\] and \[\Delta H\] and \[\Delta S\] are +ve, then \[\Delta G\] is negative.
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