A) \[+\,ve\text{ }\Delta H\]and \[+\,ve\text{ }\Delta S\]
B) \[-\,ve\text{ }\Delta H\] and \[-\,ve\text{ }\Delta S\]
C) \[+\,ve\text{ }\Delta H\]and \[-\,ve\text{ }\Delta S\]
D) \[-\,ve\text{ }\Delta H\] and\[+\,ve\text{ }\Delta S\]
Correct Answer: C
Solution :
For a process to be spontaneous, \[\Delta G\]will be negative. We know that, \[\Delta G=\Delta H-T\Delta S\] If \[\Delta H=+\,ve\]and \[\Delta S=-ve,\Delta G\]will be positive at all temperatures. Thus, the process is non-spontaneous.
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