What element is being oxidized in the following redox reaction?

            MnO₄⁻ (aq) + H₂C₂O₄(aq) →  Mn²⁺(aq) + CO₂(g)

Balance the following redox reaction if it occurs in acidic solution.  What are the coefficients in front of  H2C2O4 and H2O in the balanced reaction? (Ex. compound=number, compound=number)

            MnO₄⁻ (aq) + H₂C₂O₄(aq) →  Mn²⁺(aq) + CO₂(g)

Identify the location of oxidation in an electrochemical cell.

Define a salt bridge.

Determine the redox reaction represented by the following cell notation.

            Mg(s) ∣ Mg²⁺(aq) II Cu²⁺(aq) ∣ Cu(s)

Determine the cell notation for the redox reaction given below.

            3 Cl₂(g) + 2 Fe(s) → 6 Cl⁻(aq) + 2 Fe³⁺(aq)

Which of the following is the strongest reducing agent?

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

            3 Cl₂(g) + 2 Fe(s) → 6 Cl⁻(aq) + 2  Fe³⁺(aq)

Cl₂(g) + 2 e⁻ → 2 Cl⁻(aq)      E° = +1.36 V

Fe³⁺(aq) + 3 e⁻  →  Fe(s)       E° = -0.04 V

Determine which of the following pairs of reactants will result in a spontaneous reaction at 25°C.

Which of the following metals will dissolve in HCl?

How many electrons are transferred in the following reaction? (The reaction is unbalanced.)

            I₂(s) + Fe(s)  →  Fe³⁺(aq) + I⁻(aq)