The rusting of iron takes place as follows 2H++2e−+12O2→H2O(l);E∘=+1.23VFe2++2e−→Fe(s);E∘=−0.44V Calculate ΔG∘ for the net process
A
-322 kJ mol-1
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B
-161 kJ mol-1
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C
-152 kJ mol-1
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D
-76 kJ mol-1
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Solution
The correct option is A -322 kJ mol-1 Fe(s)⟶Fe2++2e−;ΔG∘12H++2e−+12O2⟶H2O(I);ΔG∘2Fe(s)+2H++12O2⟶Fe2++H2O;ΔG∘3 Applying, ΔG∘1+ΔG∘2=ΔG∘3 ΔG∘3=(−2F×0.44)+(−2F×1.23) ΔG∘3=−(2×96500×0.44+2×96500×1.23) ΔG∘3=−322310J ∴ΔG∘3=−322kJ