At 300 K, the enthalpy change and entropy change of a reaction are -10 kcal and `-30 " cal". K^(-1)` respectively. Does the reaction occur spontaneously at 400 K ? If not, then calculate the maximum temperature at which the reaction will occur spontaneously ?

Explanation

At `400 K, Delta G= Delta H - T Delta S= {-10xx10^(3)-400xx(-30)}= 2000` cal
Since `Delta G gt 0`, the reaction cannot occur spontaneously. If the reaction is spontaneous at temperature TK, then at this temeperature `Delta G lt 0`.
or, `|DeltaH| lt T |Delta S| " or ", T gt |(Delta H)/(Delta S)|`
or, `T gt (10xx10^(3))/(30)= 333.33 K`