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.

at relatively low temperatures.

Explanation:

According to Gibbs equation;

= Gibb's free energy change

= enthalpy change

T = temperature

= entropy change

A reaction is spontaneous when = Gibb's free energy change is negative.

Thus

Thus the reaction is spontaneous or is negative only when

Thus the reaction is spontaneous at relatively low temperatures

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