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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.

Respuesta :

Answer: at relatively low temperatures.

Explanation:

According to Gibbs equation;

[tex]\Delta G=\Delta H-T\Delta S[/tex]

[tex]\Delta G[/tex] = Gibb's free energy change

[tex]\Delta H[/tex] = enthalpy change

T = temperature

[tex]\Delta S[/tex] = entropy change

A reaction is spontaneous when [tex]\Delta G[/tex] = Gibb's free energy change is negative.

Thus [tex]\Delta G=(-\Delta H)-T(-\Delta S)[/tex]

[tex]\Delta G=-(\Delta H)+T(\Delta S)[/tex]

Thus the reaction is spontaneous or [tex]\Delta G[/tex] is negative only when [tex]T(\Delta S)<\Delta H[/tex]

Thus the reaction is spontaneous at relatively low temperatures

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