Question

For the reaction CH4(g) + 2O2(g)CO2(g) + 2H2O(g) H° = -802 kJ and S° = -5.20 J/K At standard conditions, this reaction would be product favored at all temperatures. at relatively high temperatures. at relatively low temperatures. at no temperature.

Answer 1

Answer: at relatively low temperatures.

Explanation:

According to Gibbs equation;

$\Delta G=\Delta H-T\Delta S$

$\Delta G$ = Gibb's free energy change

$\Delta H$ = enthalpy change

T = temperature

$\Delta S$ = entropy change

A reaction is spontaneous when $\Delta G$ = Gibb's free energy change is negative.

Thus $\Delta G=(-\Delta H)-T(-\Delta S)$

$\Delta G=-(\Delta H)+T(\Delta S)$

Thus the reaction is spontaneous or $\Delta G$ is negative only when $T(\Delta S)$

Thus the reaction is spontaneous at relatively low temperatures