For reversible operation of the lead storage cell (given in following figure) at 298 K and all species in the cell in their standard state,

Select the correct statement(s) based on following data.
Half cell reaction E°(volt)
$\begin{array}{l} {PbO}_{2} (s) + {SO}_{4}^{- 2} (aq) + 4 H^{+} (aq) 2 e^{-} \to {PbSO}_{4} (s) + 2 H_{2} O (ℓ) + 1.7 V \\ {PbO}_{2} (s) + 4 H^{+} + 2 e^{-} \to {Pb}^{+ 2} (aq) + 2 H_{2} O (ℓ) + 1.46 V \\ {Pb}^{+ 2} (aq) + 2 e^{-} \to Pb (s) - 0.13 V \\ {PbSO}_{4} (s) + 2 e^{-} \to Pb (s) + {SO}_{4}^{- 2} (aq) \\ {ΔH}^{\circ} of the overall cell reaction = - 306 kJ / mol \end{array}$

Question

For reversible operation of the lead storage cell (given in following figure) at 298 K and all species in the cell in their standard state,

Select the correct statement(s) based on following data.
Half cell reaction E°(volt)
$\begin{array}{l} {PbO}_{2} (s) + {SO}_{4}^{- 2} (aq) + 4 H^{+} (aq) 2 e^{-} \to {PbSO}_{4} (s) + 2 H_{2} O (ℓ) + 1.7 V \\ {PbO}_{2} (s) + 4 H^{+} + 2 e^{-} \to {Pb}^{+ 2} (aq) + 2 H_{2} O (ℓ) + 1.46 V \\ {Pb}^{+ 2} (aq) + 2 e^{-} \to Pb (s) - 0.13 V \\ {PbSO}_{4} (s) + 2 e^{-} \to Pb (s) + {SO}_{4}^{- 2} (aq) \\ {ΔH}^{\circ} of the overall cell reaction = - 306 kJ / mol \end{array}$

Infinity Learn · Accepted Answer

Anode : $$Pbs+SO42$$−aq→  $$PbSO4s+2e$$−E° $$=$$ $$0.3VCathode$$: $$PbO2+SO42$$−$$aq+4H++2e$$−→  $$PbSO4+2H2Ol$$ E° $$=$$ $$1.7$$ $$VEcello=2V$$ΔGcetl ∘$$=$$−$$(2)(96500)(2)1000=$$−$$386$$ΔG∘$$=$$ΔH∘−TΔS∘TΔS∘$$=$$ΔH∘−ΔG∘TΔS∘$$=$$−$$306+386=80$$ΔS∘$$=+$$

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