Consider the galvanic cell based on the following half$-$reactions:

$M{n}^{2+}+2e^{-}Mn,=-1\mathrm{.}18V$

$C{d}^{2+}+2e^{-}Cd,=-0\mathrm{.}40V$

a$.$ Determine the overall cell reaction and calculate

${}_{\text{c}\text{e}\text{l}\text{l}}.$

$($Use the lowest possible coefficients. Be sure to specify states such as $($aq$)$ or $($s$).$ If a

box is not needed, leave it blank.$)$

$eps{i}_{\text{c}\text{e}\text{l}\text{l}}^{\text{@}}++$

b$.$ Calculate

$\frac{?}{{?}_{\frac{?}{?}}G}$ and

$K$ for the cell reaction at $25C.$

$\frac{?}{{?}_{\frac{?}{?}}G}=$

kJ

$K=$

c$.$ Calculate

${}_{\text{c}\text{e}\text{l}\text{l}}$ at $25C$ when

$[M{n}^{2+}]=0\mathrm{.}10M$ and

$[C{d}^{2+}]=6\mathrm{.}0{10}^{-5}M.$

${}_{\text{c}\text{e}\text{l}\text{l}}=$