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(C) The cell reaction is: $Sn^{+2} (1 \ M) + 2Cl^{-} (2 \ M) \rightarrow Sn_{(s)} + Cl_2 (1 \ atm)$ Cathode (Reduction): $Cl_2 + 2e^- \rightarrow 2Cl^

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$+1.522 \ V$

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(C) The cell reaction is: $Sn^{+2} (1 \ M) + 2Cl^{-} (2 \ M) ightarrow Sn_{(s)} + Cl_2 (1 \ atm)$ Cathode (Reduction): $Cl_2 + 2e^- ightarrow 2Cl^-$,$E^o_{red} = 1.4 \ V$ Anode (Oxidation): $Sn ightarrow Sn^{+2} + 2e^-$,$E^o_{ox} = -E^o_{Sn^{+2}/Sn} = -(-0.14) = 0.14 \ V$ Standard cell potential: $E^o_{cell} = E^o_{cathode} - E^o_{anode} = -0.14 - 1.4 = -1.54 \ V$ Using the Nernst equation: $E_{cell} = E^o_{cell} - \frac{0.06}{n} \log Q$ Here,$n = 2$ and $Q = \frac{[Sn^{+2}]}{[Cl^-]^2} = \frac{1}{(2)^2} = \frac{1}{4} = 0.25$ $E_{cell} = -1.54 - \frac{0.06}{2} \log(0.25) = -1.54 - 0.03 	imes (-0.602) = -1.54 + 0.01806 = -1.52194 \ V$ The decomposition potential is the negative of the cell potential,which is approximately $+1.522 \ V$.

What minimum decomposition potential is necessary to produce $Cl_2$ gas in the following reaction?
Given: $(\frac{2.303RT}{F} = 0.06)$
$Sn^{+2} (1 \ M) + 2Cl^{-} (2 \ M) \rightleftharpoons Sn_{(s)} + Cl_2 (1 \ atm)$
Given: $E^{o}_{Sn^{+2}/Sn} = -0.14 \ V$,$E^{o}_{Cl_2/Cl^{-}} = 1.4 \ V$

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What minimum decomposition potential is necessary to produce $Cl_2$ gas in the following reaction? Given: $(\frac{2.303RT}{F} = 0.06)$ $Sn^{+2} (1 \ M) + 2Cl^{-} (2 \ M) \rightleftharpoons Sn_{(s)} + Cl_2 (1 \ atm)$ Given: $E^{o}_{Sn^{+2}/Sn} = -0.14 \ V$,$E^{o}_{Cl_2/Cl^{-}} = 1.4 \ V$