Calculate E°_cell for each balanced redox reaction and determine if the reaction is spontaneous as written. c. PbO₂(s) + 4 H⁺(aq) + Sn(s) → Pb²⁺(aq) + 2 H₂O(l) + Sn²⁺(aq)

Which metal cation is the best oxidizing agent? a. Zn2+ b. Sn2+ c. Cd2+ d. Ni2+

Use tabulated electrode potentials to calculate 𝛥𝐺rxn° for each reaction at 25 °C. c. O2( g) + 2 H2O(l) + 2 Cu(s)¡4 OH-(aq) + 2 Cu2+(aq)

Use tabulated electrode potentials to calculate 𝛥𝐺rxn° for each reaction at 25 °C. a. MnO2(s) + 4 H+(aq) + Cu(s)¡Mn2+(aq) + 2 H2O(l) + Cu2+(aq)

Use tabulated electrode potentials to calculate 𝛥𝐺rxn° for each reaction at 25 °C. c. Br2(l) + 2Cl–(aq) → 2 Br–(aq) + Cl2(g)

Calculate the equilibrium constant for each of the reactions in Problem 70.

Calculate the equilibrium constant for the reaction between Fe²⁺(aq) and Zn(s) (at 25 °C).

A voltaic cell employs the following redox reaction: Sn²⁺(aq) + Mn(s) → Sn(s) + Mn²⁺(aq) Calculate the cell potential at 25 °C under each set of conditions. c. [Sn²⁺] = 2.00 M; [Mn²⁺] = 0.0100 M

An electrochemical cell is based on these two half-reactions:

Ox: Pb(s) → Pb²⁺(aq, 0.10 M) + 2 e^–

Red: MnO₄^–(aq, 1.50 M) + 4 H⁺(aq, 2.0 M) + 3 e^– → MnO₂(s) + 2 H₂O(l)

Calculate the cell potential at 25 °C.

An electrochemical cell is based on these two half-reactions:

Ox: Sn(s) → Sn²⁺(aq, 2.00 M) + 2 e^–

Red: ClO₂(g, 0.100 atm) + e^– → ClO₂^–(aq, 2.00 M)

Calculate the cell potential at 25 °C.

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. a. What is the initial cell potential?

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. b. What is the cell potential when the concentration of Ni²⁺ has fallen to 0.500 M?

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