Chemistry - Electrochemistry Question with Solution | TestHub

The above fuel cell is used for electrolysis in Cu voltmeters of resistance $5.2\Omega$ using Pt electrodes. Initially Cu voltmeter contains 1 L solutions of $0.05\mathrm{M}{\mathrm{CuSO}}_4$. Find conc. of $\left[{\mathrm{H}}^{+}\right]$formed due to electrolysis for 96.5 minutes. (Assume no change in volume of solution)

Pt | H₂(g) | H⁺(aq) || H₂O(ℓ) | O₂(g) | Pt.

$$\frac{2.303}{F}=0.06$$

The above fuel cell is used to produce a constant current supply under constant temperature and 30 atm constant total pressure conditions in a cylinder. If 10 moles of H₂ and 5 moles of O₂ were taken initially, the rate of consumption of O₂ is 10 moles per minute.

The half-cell reactions are:

1/2O₂(g) + 2H⁺(aq) + 2e⁻ → H₂O(ℓ); $E^{\circ }=1.246\mathrm{V}$

2H⁺(aq) + 2e⁻ → H₂(g); $E^{\circ }=0\mathrm{V}$.