Home
Class 12
CHEMISTRY
The half cell reactions for rusting of i...

The half cell reactions for rusting of iron are :
`2H^(+) + 2e^(-) + (1)/(2)O_(2) rightarrow H_(2)O (l)` ,` E^(@) = +1.23V`
`Fe^(2+) + 2e^(-) + (1)/(2)rightarrow H_(2)O_(2) ((l))` , `E^(@) = -0.44V`
` Delta^(@)` ((inKJ) for the reaction is : `Fe+2H^(+) + (1)/(2) O_(2)rightarrow Fe^(+2)+ H_(2) O ((l))`

A

`(-76)`

B

`(-322)`

C

`(-122)`

D

`(-176)`

Text Solution

AI Generated Solution

To find the standard Gibbs free energy change (ΔG°) for the reaction: \[ \text{Fe} + 2\text{H}^+ + \frac{1}{2}\text{O}_2 \rightarrow \text{Fe}^{2+} + \text{H}_2\text{O} \] we will use the standard reduction potentials provided for the half-cell reactions and the relationship between Gibbs free energy and cell potential. ### Step 1: Identify the half-reactions and their standard potentials ...
Promotional Banner

Similar Questions

Explore conceptually related problems

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 is

The rusting of iron takes place as follows : 2H^(o+)+2e^(-) +(1)/(2)O_(2)rarr H_(2)O(l)," "E^(c-)=+1.23V Fe^(2+)+2e^(-) rarr Fe(s)," "E^(c-)=-0.44V Calculae DeltaG^(c-) for the net process.

The half-cell reaction for the corrosion, {:(2H^(+)+,(1)/(2)O_(2)+2e^(-) rarr H_(2)O,,,E_(@) = 123 V),(,Fe^(2+)+2e^(-) rarrFe(s),,,E^(@) = -0.44 V):} Find the Delya G^(@) (in kJ) for the overall reaction :

The following reaction occurs during rusting of iron 2H^(+)+2e+(1)/(2)O_(2)rarrH_(2)O,E^(@)=+1.23V Fe^(2+)+2erarr Fe(s), E^(@)=0.44V Calculate magnitude of DeltaG^(@)(kJ) for the net process Fe(s)+2H^(+)+(1)/(2)O_(2)rarrFe^(2+)+H_(2)O