1) A student determines the value of the equilibrium constant to be 1.10×10 6 fo

Question

1) A student determines the value of the equilibrium constant to be 1.10×106 for the following reaction.

3Fe2O3(s) + H2(g) -----> 2Fe3O4(s) + H2O(g)

Based on this value of Keq:

G° for this reaction is expected to be (greater, less) than zero?

Calculate the free energy change for the reaction of 2.02 moles of Fe2O3(s) at standard conditions at 298K.

2) A student determines the value of the equilibrium constant to be 1.10×106 for the following reaction.

3Fe2O3(s) + H2(g) -----> 2Fe3O4(s) + H2O(g)

Based on this value of Keq:

G° for this reaction is expected to be (greater, less) than zero?

Calculate the free energy change for the reaction of 2.02 moles of Fe2O3(s) at standard conditions at 298K.

Explanation / Answer

delta G = -RTln(Keq) = -8.314*T*ln(1.1*106) = -115..65*T

Hence at any T the delta G value is expected to be less than zero making reaction sponteneous at any T.

At T = 298 K delta G = -34465 J/mol

so for 2.02 moles delta G = -34465*2.02 = -69619 J = -69.619 kJ

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