For a particular reaction, `Delta H ^(@) =- 38.3 kJ` and `Delta S ^(@) =- 113. JK ^(-1) mol ^(-1).` This reaction is:

Options

A. spontaneous at all temperatures
B. non-spontaneous at all temperatures
C. spontaneous at-temperatures below `66^(@)C`
D. spontaneous at temperatures above `66^(@)C`

Explanation

`Delta G = Delta H - T Delta G:` For supotaneous process, `Delta G lt 0.`
`therefore Delta H - T Delta S lt 0, ( Delta H )/( Delta S) lt T , ( - 38. 3 xx 1000)/(-113) lt T i.e., T gt 338.93 K, i.e., 66^(@)C`