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(A) The cell reaction is: $Pb_{(s)} + 2Ag^{+}_{(10 \ M)} \rightarrow Pb^{2+}_{(1 \ M)} + 2Ag_{(s)}$Using the Nernst equation at $25^{\circ} C$ $(298 \

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$E_{cell} = (E^{\circ}_{cell} + 0.0592) \ V$

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(A) The cell reaction is: $Pb_{(s)} + 2Ag^{+}_{(10 \ M)} ightarrow Pb^{2+}_{(1 \ M)} + 2Ag_{(s)}$Using the Nernst equation at $25^{\circ} C$ $(298 \ K)$:$E_{cell} = E^{\circ}_{cell} - \frac{0.0592}{n} \log_{10} Q$Here,$n = 2$ (number of electrons transferred).$Q = \frac{[Pb^{2+}]}{[Ag^{+}]^{2}} = \frac{1}{(10)^{2}} = 10^{-2}$Substituting the values:$E_{cell} = E^{\circ}_{cell} - \frac{0.0592}{2} \log_{10} (10^{-2})$$E_{cell} = E^{\circ}_{cell} - \frac{0.0592}{2} 	imes (-2)$$E_{cell} = E^{\circ}_{cell} + 0.0592 \ V$

Which of the following expressions is used to calculate $E_{cell}$ for the following cell at $25^{\circ} C$?
$Pb_{(s)} | Pb^{2+}_{(1 \ M)} || Ag^{+}_{(10 \ M)} | Ag_{(s)}$

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Which of the following expressions is used to calculate $E_{cell}$ for the following cell at $25^{\circ} C$?$Pb_{(s)} | Pb^{2+}_{(1 \ M)} || Ag^{+}_{(10 \ M)} | Ag_{(s)}$