What is the change in free energy for the following reaction when we have 2.00 m

Question

What is the change in free energy for the following reaction when we have 2.00 mol Fe2O3, 1.5 mol FeO, 0.35 mol Fe, and the partial pressure of O2 is 200.0 atm in a sealed 1.00 L reaction vessel at 298 K?

FeO(s) + Fe(s) + O2(g) ?Fe2O3(s)

A) -482 B) -500 C) -474 D) -493 E) -487

What is the change in free energy for the following reaction when we have 2.00 mol Fe2O3, 1.5 mol FeO, 0.35 mol Fe, and the partial pressure of O2 is 200.0 atm in a sealed 1.00 L reaction vessel at 298 K?

FeO(s) + Fe(s) + O2(g) ?Fe2O3(s)

A) -482 B) -500 C) -474 D) -493 E) -487

Explanation / Answer

K=1/[O2]

=1/200

=0.0025

so, dG=-RTln(k)

=-8.31*(298)*ln(0.005)

=13120.6 kJ/mol

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