The half cell reaction for rusting of iron are: `2H^(+)+2e^(-)+(1)/(2)O_(2)rarrH_(2)O(l), E^(@)=+1.23V` `Fe^(2+)+2e^(-)rarrFe(s), E^(@)=-0.44V` `DeltaG^(@)` (in KJ) for the reaction isA. `-76`B. `-322`C. `-122`D. `-176`

The half cell reaction for rusting of iron are: `2H^(+)+2e^(-)+(1)/(2)

1.	The half cell reaction for rusting of iron are: `2H^(+)+2e^(-)+(1)/(2)O_(2)rarrH_(2)O(l), E^(@)=+1.23V` `Fe^(2+)+2e^(-)rarrFe(s), E^(@)=-0.44V` `DeltaG^(@)` (in KJ) for the reaction isA. `-76`B. `-322`C. `-122`D. `-176`
Answer» Correct Answer - B For e.m.f. to be _ve, oxidation should occur at iron electrode, `E_("cell")=1.23+1.67V` `DeltaG=-nFE_("cell")^(@)=2xx 96500xx1.67`. =-322kJ.

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The half cell reaction for rusting of iron are: `2H^(+)+2e^(-)+(1)/(2)O_(2)rarrH_(2)O(l), E^(@)=+1.23V` `Fe^(2+)+2e^(-)rarrFe(s), E^(@)=-0.44V` `DeltaG^(@)` (in KJ) for the reaction isA. `-76`B. `-322`C. `-122`D. `-176`

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