A voltaic cell consists of a Zn/Zn²⁺ half-cell and a Ni/Ni²⁺ half-cell at 25 °C. The initial concentrations of Ni²⁺ and Zn²⁺ are 1.50 M and 0.100 M, respectively. c. What are the concentrations of Ni²⁺ and Zn²⁺ when the cell potential falls to 0.45 V?

A voltaic cell consists of a Pb/Pb²⁺ half-cell and a Cu/Cu²⁺ half-cell at 25°C. The initial concentrations of Pb²⁺ and Cu²⁺ are 0.0500 M and 1.50 M, respectively. a. What is the initial cell potential?

A voltaic cell consists of a Pb/Pb²⁺ half-cell and a Cu/Cu²⁺ half-cell at 25°C. The initial concentrations of Pb²⁺ and Cu²⁺ are 0.0500 M and 1.50 M, respectively. b. What is the cell potential when the concentration of Cu²⁺ has fallen to 0.200 M?

A voltaic cell consists of a Pb/Pb²⁺ half-cell and a Cu/Cu²⁺ half-cell at 25°C. The initial concentrations of Pb²⁺ and Cu²⁺ are 0.0500 M and 1.50 M, respectively. c. What are the concentrations of Pb²⁺ and Cu²⁺ when the cell potential falls to 0.35 V?

Make a sketch of a concentration cell employing two Zn/Zn²⁺ half-cells. The concentration of Zn²⁺ in one of the half-cells is 2.0 M and the concentration in the other half-cell is 1.0×10^–3 M. Label the anode and the cathode and indicate the half-reaction occuring at each electrode. Also indicate the direction of electron flow.

Consider the concentration cell: b. Indicate the direction of electron flow.

Consider the concentration cell:

c. Indicate what happens to the concentration of Pb²⁺ in each half-cell.

A concentration cell consists of two Sn/Sn²⁺ half-cells. The cell has a potential of 0.10 V at 25°C. What is the ratio of the Sn²⁺ concentrations in the two half-cells?

A Cu/Cu²⁺ concentration cell has a voltage of 0.22 V at 25 °C. The concentration of Cu²⁺ in one of the half-cells is 1.5×10^–3 M. What is the concentration of Cu²⁺ in the other half-cell? (Assume the concentration in the unknown cell is the lower of the two concentrations.)

Determine the optimum mass ratio of Zn to MnO₂ in an alkaline battery.

What mass of lead sulfate is formed in a lead–acid storage battery when 1.00 g of Pb undergoes oxidation?

Refer to the tabulated values of ∆G°_f in Appendix IIB to calculate E°_cell for the fuel-cell breathalyzer, which employs the following reaction. ((∆G° for HC₂H₃O₂(g) = -374.2 kJ/mol.)

CH₃CH₂OH(g) + O₂(g) → HC₂H₃O₂(g) + H₂O(g)

Determine whether or not each metal, if coated onto iron, would prevent the corrosion of iron. a. Zn

Determine whether or not each metal, if coated onto iron, would prevent the corrosion of iron. b. Sn

Determine whether or not each metal, if coated onto iron, would prevent the corrosion of iron. c. Mn

Determine whether or not each metal, if coated onto iron, would prevent the corrosion of iron. a. Mg

Determine whether or not each metal, if coated onto iron, would prevent the corrosion of iron. b. Cr

Determine whether or not each metal, if coated onto iron, would prevent the corrosion of iron. c. Cu

Consider the electrolytic cell: b. Indicate the direction of electron flow.

Draw an electrolytic cell in which Mn²⁺ is reduced to Mn and Sn is oxidized to Sn²⁺. Label the anode and cathode, indicate the direction of electron flow, and write an equation for the half-reaction occurring at each electrode. What minimum voltage is necessary to drive the reaction?

Write equations for the half-reactions that occur in the electrolysis of molten potassium bromide.

What products are obtained in the electrolysis of molten NaI?

What products are obtained in the electrolysis of a molten mixture of KI and KBr?

Write equations for the half-reactions that occur at the anode and cathode for the electrolysis of each aqueous solution. a. Ni(NO₃)₂(aq)

Make a sketch of an electrolysis cell that electroplates copper onto other metal surfaces. Label the anode and the cathode and indicate the reactions that occur at each.

Silver can be electroplated at the cathode of an electrolysis cell by the half-reaction: Ag⁺(aq) + e^– → Ag(s) What mass of silver would plate onto the cathode if a current of 6.8 A flowed through the cell for 72 min?