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.

Step-by-step 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)<\Delta H`

Thus the reaction is spontaneous at relatively low temperatures