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.
You need to login to perform this action.
You will be redirected in
3 sec
