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The equilibrium constant of a system, K, can be related to the standard free energy change,...

The equilibrium constant of a system, K, can be related to the standard free energy change, ΔG∘, using the following equation:

ΔG∘=−RTlnK

where T is a specified temperature in kelvins (usually 298 K) and R is equal to 8.314 J/(K⋅mol).

Under conditions other than standard state, the following equation applies:

ΔG=ΔG∘+RTlnQ

In this equation, Q is the reaction quotient and is defined the same manner as K except that the concentrations or pressures used are not necessarily the equilibrium values.

At 25 ∘C the reaction from Part A has a composition as shown in the table below.

Substance Pressure
(atm)
C2H2(g) 3.95
H2(g) 5.05
C2H6(g) 1.25×10−2

What is the free energy change, ΔG, in kilojoules for the reaction under these conditions?

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