(Solved): Consider the battery. Cd(s)CdCl2(aq)Cl(aq)Cl2(l)C(s) Write the ...

Consider the battery. $\mathrm{Cd}(\mathrm{s})?{\mathrm{CdCl}}_2(\mathrm{aq})??{\mathrm{Cl}}^{?}(\mathrm{aq})?{\mathrm{Cl}}_2(\mathrm{l})?\mathrm{C}(\mathrm{s})$ Write the reduction half-reaction occuring at the $\mathrm{C}(\mathrm{s})$ electrode. Include physical states. C(s) electrode $E^{?}=1.4\mathrm{V}$ From which electrode will electrons flow from the battery into a circuit? $\begin{array}{l}\mathrm{C}(\mathrm{s})\text{ electrode }\\ \mathrm{Cd}(\mathrm{s})\text{ electrode }\end{array}$ Calculate the mass of ${\mathrm{Cl}}_2$ consumed if the battery delivers a constant current of $559\mathrm{A}$ for $46.0\min$. mass: $\mathrm{kg}$