A student determines the value of the equilibrium constant to be 62×10-18for the following reaction.Fe3O4(s) + 4H2(g)3Fe(s) + 4H2O(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 1.89 moles of Fe3O4(s) at standard conditions at 298K.     G°rxn =  ______ kJ

Question
Asked Jul 31, 2019
  1. A student determines the value of the equilibrium constant to be 62×10-18for the following reaction.

    Fe3O4(s) + 4H2(g)3Fe(s) + 4H2O(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 1.89 moles of Fe3O4(s) at standard conditions at 298K.
         G°rxn =  ______ kJ
check_circleExpert Solution
Step 1

From the relationship between equilibrium constant (K) and ΔG0, it is clear that when the value of K becomes less than one, then G° for the reaction is expected to be less than zero.

=- RT ln K
AG0
AG°
RT
K e
Since, K value is less than one(K < 1) AG
becomes positive
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=- RT ln K AG0 AG° RT K e Since, K value is less than one(K < 1) AG becomes positive

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Step 2

The value of ∆G per mole for the reaction can be determined using the given formula as follows,

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Step 3

The value of ∆G per mole for the reaction is 92.46 kJ/mol. There are 1.89 moles of Fe3O4 presen...

AG for the reaction = (92.46 kJ /mol) (1.89 moles)
= 174.75 kJ
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AG for the reaction = (92.46 kJ /mol) (1.89 moles) = 174.75 kJ

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