Assertion: $\left(\mathrm{A}\right):{\mathrm{E}}_{\text{cefl }}$ increase with increase in concentration of ${\mathrm{Ag}}^{+}$ ions

Reason $\left(\mathrm{R}\right)$: Ecen has positive value.

Cell equation: $\mathrm{A}+2{\mathrm{B}}^{+}⟶{\mathrm{A}}^{2+}+2\mathrm{B}$

${\mathrm{A}}^{2+}+2\mathrm{e}⟶\mathrm{A} \mathrm{E}°=+0.34\mathrm{V}$ and ${\log }_{10}\mathrm{K}=15.6$ at $300\mathrm{K}$ for cell reactions

Find $\mathrm{E}°$ for ${\mathrm{B}}^{+}+\mathrm{e}\to \mathrm{B}$

Given ${\left[\frac{2.303\mathrm{RT}}{\mathrm{nF}}=0.059\right]}_{\text{at300k }}$

In the following cell reaction:

$\mathrm{Mg}\left(\mathrm{s}\right)+2{\mathrm{Ag}}^{+}(0.001\mathrm{M})⟶{\mathrm{Mg}}^{2+}(0.20\mathrm{M})+2\mathrm{Ag}\left(\mathrm{S}\right)$

Calculate ${\mathrm{E}}_{\mathrm{cell}}$ for the reaction $\left[\mathrm{E}°=3.17\vee ,\frac{2.30\mathrm{RT}}{\mathrm{F}}=0.054\right]$

The equilibrium constant of the reaction:

$\mathrm{Cu} \left(\mathrm{s}\right)+2{\mathrm{Ag}}^{+}\left(\mathrm{aq}\right)\to {\mathrm{Cu}}^{2+}\left(\mathrm{aq}\right)+2\mathrm{Ag} \left(\mathrm{s}\right)$,

$\mathrm{E}°=0.46\mathrm{V}$ at $298 \mathrm{K}$ is: