Balance the following redox reaction if it occurs in acidic solution.  What are the coefficients in front of Zn and H+ in the balanced reaction?

            Zn²⁺(aq) + NH₄+(aq) → Zn(s) + NO₃⁻(aq)  

Determine the cell notation for the redox reaction given below.

            Sn(s) + 2 Ag⁺(aq) → Sn²⁺(aq) + 2 Ag(s)  

What is the oxidizing agent in the redox reaction represented by the following cell notation?

                        Ni(s) ∣ Ni²⁺(aq) || Ag+(aq) ∣ Ag(s)

What statement is NOT true about standard electrode potentials?

Which of the following is the strongest reducing agent?

Use the standard half-cell potentials listed below to calculate the standard cell potential for the following reaction occurring in an electrochemical cell at 25 °C. (The equation is balanced.)

            2 K(s) + I₂(s) → 2 K⁺(aq) + 2 I⁻(aq)

K+(aq) + e⁻ → K (s)               E° = -2.93 V

I₂(s) + 2 e⁻  → 2 I⁻(aq)           E° = +0.54 V

Which of the following metals will dissolve in nitric acid but not hydrochloric?

Use the tabulated half-cell potentials to calculate ΔG° (in kJ) for the following redox reaction.

            2 Al(s) + 3 Mg²⁺(aq) → 2 Al³⁺(aq) + 3 Mg(s)