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, 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+?

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?

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.

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?

What is the change in the cell voltage when the ion concentrations in the cathode half-cell are increased by a factor of 10, according to the Nernst Equation?

What is the emf of this cell when [Fe²⁺] = 1.5 M, [Fe³⁺] = 1.4 × 10⁻² M, P(O₂) = 0.56 atm, and the pH of the solution in the cathode compartment is 3.5, given that the standard cell potential (E°) is 1.23 V?

Calculate the cell potential at 25°C for a galvanic cell with the following reaction: Zn(s) + Cu²⁺(aq) → Zn²⁺(aq) + Cu(s), given that the concentrations are [Zn²⁺] = 0.010 M and [Cu²⁺] = 1.0 M. The standard cell potential (E°) is 1.10 V.