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(C) In the corrosion of iron,the anodic reaction is $Fe \rightarrow Fe^{+2} + 2e^-$ and the cathodic reaction is $O_2 + 4H^+ + 4e^- \rightarrow 2H_2O$

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$1.67$

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(C) In the corrosion of iron,the anodic reaction is $Fe \rightarrow Fe^{+2} + 2e^-$ and the cathodic reaction is $O_2 + 4H^+ + 4e^- \rightarrow 2H_2O$.The standard cell potential is calculated as:$E^{\circ}_{cell} = E^{\circ}_{cathode} - E^{\circ}_{anode}$Given $E^{\circ}_{cathode} = 1.23 \, V$ and $E^{\circ}_{anode} = -0.44 \, V$.$E^{\circ}_{cell} = 1.23 \, V - (-0.44 \, V)$$E^{\circ}_{cell} = 1.23 + 0.44 = 1.67 \, V$

The standard electrode potentials are given as:
$E^o_{Fe^{+2}/Fe} = -0.44 \, V$ and $E^o_{H^{+}/O_2/H_2O} = 1.23 \, V$
Calculate the $E^o_{cell}$ for the corrosion process: ............. $V$

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The standard electrode potentials are given as:$E^o_{Fe^{+2}/Fe} = -0.44 \, V$ and $E^o_{H^{+}/O_2/H_2O} = 1.23 \, V$Calculate the $E^o_{cell}$ for the corrosion process: ............. $V$