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(C) The Nernst equation for the given cell reaction is: $E_{cell} = E_{cell}^0 - \frac{0.059}{2} \log \frac{[Sn^{2+}]}{[Ag^{+}]^2}$.According to the e

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Increase in the concentration of $Ag^{+}$ ions

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(C) The Nernst equation for the given cell reaction is: $E_{cell} = E_{cell}^0 - \frac{0.059}{2} \log \frac{[Sn^{2+}]}{[Ag^{+}]^2}$.According to the equation,$E_{cell}$ depends on the ratio of the concentrations of the products to the reactants.To increase the voltage $(E_{cell})$,we need to decrease the value of the logarithmic term $\frac{[Sn^{2+}]}{[Ag^{+}]^2}$.This can be achieved by increasing the concentration of the reactant $Ag^{+}$ ions or by decreasing the concentration of the product $Sn^{2+}$ ions.Therefore,an increase in the concentration of $Ag^{+}$ ions will increase the voltage of the cell.

Which one of the following will increase the voltage of the cell? $(T = 298 \ K)$ :- $Sn_{(s)} + 2Ag_{(aq)}^{+} \rightarrow Sn_{(aq)}^{2+} + 2Ag_{(s)}$

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