Galvanic Cells And Standard Potentials

To calculate the standard cell potential $E^\circ_{cell}$ for the reaction $Ni(s) + 2Ag^+(aq) \rightarrow Ni^{2+}(aq) + 2Ag(s)$, we first identify the half-reactions. The silver ions ($Ag^+$) are being reduced to silver metal, so the silver half-cell acts as the . The nickel solid ($Ni$) is being oxidized to nickel ions ($Ni^{2+}$), meaning the nickel half-cell acts as the . We use the standard formula $E^\circ_{cell} = E^\circ_{R} - E^\circ_{L}$ to find the overall cell potential. Substituting the given standard reduction potentials of $+0.80\text{V}$ for silver and $-0.25\text{V}$ for nickel, we set up the equation as $E^\circ_{cell} = 0.80\text{V} - (-0.25\text{V})$. Calculating this difference yields a final standard cell potential of .