Efficiency of a cell with cell reaction under | vedclass

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(A) The efficiency of a cell is given by $\eta = \frac{\Delta G^o}{\Delta H^o}$.Given $\eta = 0.70$,$\Delta H^o = -300 	imes 10^3 \ J$,and $n = 1$ (f

Vedclass · Accepted Answer

$2.176$

Vedclass · Answer

(A) The efficiency of a cell is given by $\eta = \frac{\Delta G^o}{\Delta H^o}$.Given $\eta = 0.70$,$\Delta H^o = -300 	imes 10^3 \ J$,and $n = 1$ (from the reaction $A + B^+ 	o A^+ + B$),$\Delta G^o = -nFE^o = -1 	imes 96500 	imes E^o$.Substituting these into the efficiency formula:$0.70 = \frac{-nFE^o}{\Delta H^o} = \frac{-1 	imes 96500 	imes E^o}{-300000}$.$0.70 = \frac{96500 	imes E^o}{300000}$.$E^o = \frac{0.70 	imes 300000}{96500} = \frac{210000}{96500} \approx 2.176 \ V$.

List-$I$ (Applications)	List-$II$ (Batteries/Cell)
$A$. Transistors	$I$. Anode $- Zn/Hg$; Cathode $- HgO + C$
$B$. Hearing aids	$II$. Hydrogen fuel cell
$C$. Inverters	$III$. Anode $- Zn$; Cathode $- Carbon$
$D$. Apollo space ship	$IV$. Anode $- Pb$; Cathode $- PbO_2$

Efficiency of a cell with cell reaction under standard conditions,$A_{(s)} + B^{+} \to A^{+} + B_{(s)}$; $\Delta H^o = -300 \ kJ$ is $70\%$. The standard electrode potential of the cell is :- .................... $V$

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