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Question

The rusting of iron takes place as follows 2H++2e+12O2H2O(l); E=+1.23 V Fe2++2eFe(s); E=0.44 V 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; ΔG12H++2e+12O2H2O(I);ΔG2Fe(s)+2H++12O2Fe2++H2O;ΔG3
Applying, ΔG1+ΔG2=ΔG3
ΔG3=(2F×0.44)+(2F×1.23)
ΔG3=(2×96500×0.44+2×96500×1.23)
ΔG3=322310 J
ΔG3=322 kJ

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