A voltaic cell is constructed from an Ni²⁺(aq) / Ni(s) half-cell and an Ag⁺(aq) / Ag(s) half-cell. The initial concentration of Ni²⁺(aq) in the Ni²⁺ - Ni half-cell is [Ni²⁺] = 0.0100 M. The initial cell voltage is +1.12 V. (a) By using data in Appendix E, calculate the standard emf of this voltaic cell.

Verified step by step guidance

1. Identify the half-reactions for the voltaic cell: Ni^{2+} + 2e^- \rightarrow Ni(s) and Ag^+ + e^- \rightarrow Ag(s).
2. Look up the standard reduction potentials (E^\circ) for each half-reaction from Appendix E: E^\circ_{Ni^{2+}/Ni} and E^\circ_{Ag^+/Ag}.
3. Calculate the standard cell potential (E^\circ_{cell}) using the formula: E^\circ_{cell} = E^\circ_{cathode} - E^\circ_{anode}.
4. Determine which half-reaction is the cathode and which is the anode based on their standard reduction potentials (the more positive potential is the cathode).
5. Substitute the standard reduction potentials into the formula to find the standard emf of the cell.