# A student determines the value of the equilibrium constant to be 52.9 for the following reaction.C2H4(g) + H2O(g)----->CH3CH2OH(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 1.93 moles of C2H4(g) at standard conditions at 298K.     G°rxn = _____ kJ

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A student determines the value of the equilibrium constant to be 52.9 for the following reaction.

C2H4(g) + H2O(g)----->CH3CH2OH(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 1.93 moles of C2H4(g) at standard conditions at 298K.
G°rxn = _____ kJ

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Step 1

The general relation between G and K is that when Keq is greater than 1 then G0 value is less than zero that is G0 value will be negative and the reaction becomes spontaneous. The general equation is as follows,

Step 2

Therefore, for given value of equilibrium constant the G0 value is expected to be less than zero since 52.9 (equilibrium constant value) is greater than 1.

Step 3

The free energy change for the given reaction is calculated by using...

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