The process of rusting of iron occurs as follows:
$Fe \rightarrow Fe^{2+} + 2e^{-}, E^{o} = 0.44 \ V$
$2H^{+} + 2e^{-} + \frac{1}{2} O_2 \rightarrow H_2O_{(l)}, E^{o} = 1.23 \ V$
Then for this reaction,$\Delta G^{o} = .... \ kJ/mol$

Consider the following two half-cell reactions:
$CO_2 + 6H^+ + 6e^- \rightarrow CH_3OH + H_2O$ $(E^{\ominus} = 0.02 \text{ V})$
$\frac{1}{2}O_2 + 2H^+ + 2e^- \rightarrow H_2O$ $(E^{\ominus} = 1.23 \text{ V})$
$A$ fuel cell was set up such that the cell operates under standard conditions. The fuel cell works with $80\%$ efficiency. If the work derived from the cell using $1 \text{ mol}$ of $CH_3OH$ is used to compress an ideal gas isothermally against a constant pressure of $1 \text{ kPa}$, then the change in the volume of the gas, $\Delta V =$ . . . . . . $\text{m}^3$. (nearest integer) Given: $F = 96500 \text{ C mol}^{-1}$

The equation that is incorrect is

The molar conductivity of $0.025 \ mol \ L^{-1}$ methanoic acid is $46.1 \ S \ cm^2 \ mol^{-1}$. Calculate its degree of dissociation and dissociation constant. Given $\lambda^o(H^{+}) = 349.6 \ S \ cm^2 \ mol^{-1}$ and $\lambda^o(HCOO^{-}) = 54.6 \ S \ cm^2 \ mol^{-1}$.

Given ${E^o}_{Ag^{+}/Ag} = 0.80 \ V$,${E^o}_{Mg^{2+}/Mg} = -2.37 \ V$,${E^o}_{Cu^{2+}/Cu} = 0.34 \ V$,${E^o}_{Hg^{2+}/Hg} = 0.79 \ V$.
Which of the following statements is correct?

Why is electrochemistry important for the invention of the latest technology?