A) \[\Delta H<0,\,\Delta S<0\]
B) \[\Delta H>0,\,\Delta S<0\]
C) \[\Delta H<0,\,\Delta S>0\]
D) \[\Delta H>0,\,\Delta S>0\]
Correct Answer: C
Solution :
For a reaction, to be spontaneous, \[\Delta G\] (free energy change) must be negative. \[\Delta G\] is given by Gibbs-Helmoltz equation, which is \[\Delta G=\Delta H-T\cdot \Delta S\] Hence, from this equation it follows that \[\Delta H\] will be negative at all temperature if, \[\Delta H=-\,ve\] and \[\Delta S=+ve\] i.e., \[\Delta H<0\] and \[\Delta S>0\]
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