A voltaic cell is constructed with two Zn2+-Zn electrodes, where the half-reaction is Zn2+ + 2e- → Zn(s) with E° = -0.763 V. The concentrations of zinc ion in the two compartments are 5.50 M and 1.11 × 10^-2 M, respectively. What is the cell emf in volts?

Using the Nernst equation, calculate the concentration of Cu^2+ ions given the cell potential is 0.5540 V and the standard cell potential is 0.4260 V. The equation is: 0.5540 V = 0.4260 V - (0.0592/2) log ([Cu^2+]/[1]^2). What is the concentration of Cu^2+?

At 25°C, E° = +1.88 V for a cell based on the reaction 3 AgCl(s) + Al(s) → 3 Ag(s) + Al³⁺(aq) + 3 Cl⁻(aq). Find the cell potential E if [Al³⁺] = 0.20 M and [Cl⁻] = 0.010 M using the Nernst equation.

Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25 °C: Cu(s) | Cu2+(aq, 3.2×10^(-3) mol L^-1) || Cu2+(aq, 4.48 mol L^-1) | Cu(s). Given E°(Cu2+/Cu) = +0.34 V, express your answer to two significant figures.

Calculate the ΔE°cell for the following concentration cell: Cu(s) | Cu2+(aq, 0.049M) || Cu2+(aq, 0.231M) | Cu(s). Cu2+(aq) + 2e- → Cu(s), E° = 0.340V.

Using the Nernst equation, what is the concentration of Ag+ in the cathode half-cell if the cell potential is measured to be 0.70 V?