Electrochemistry MC Review

Which of the following occurs in the reaction above?

• AlF₆^3- is reduced at the cathode.

• Al is oxidized at the anode.

• Aluminum is converted from the - oxidation state to the 0 oxidation state.

• F^- acts as the reducing agent.

• F^- is reduced at the cathode.

As steady current of 10 amperes is passed through an aluminum-production cell for 15 minutes. Which of the following is the correct expressions for calculating the number of grams of aluminum produced? (1 faraday = 96,500 coulombs)

• 
• 
• 
• 
• 

According the to information above, what is the standard reduction potential for the half-reaction M³⁺ (aq) + 3 e^- → M(s)?

• -1.66 V

• -0.06 V

• 0.06 V

• 1.66 V

• 3.26 V

In which of the following reactions does the same reactant undergo both oxidation and reduction?

• H₂SeO₄(aq) + 2Cl^- (aq) + 2H⁺ (aq) → H₂SeO₃(aq) + Cl₂(g) + H₂O (l)

• S₈ (s) + 8O₂ (g) → 8SO₂ (g)

• 3Br₂ (aq) + 6OH^- (aq) → 5Br^-(aq) + BrO₃^- (aq) + 3H₂O (l)

• Ca²⁺(aq) + SO₄^2-(aq) → CaSO₄(s)

• PtCl₄ (s) + 2Cl^- (aq) → PtCl₆^2- (aq)

• I only

• II only

• III only

• I and II only

• II and III only

In the electroplating of nickel, 0.200 faraday of electrical charge is passed through a solution of NiSO₄. What mass of nickel is deposited?

• 2.94 g

• 5.87 g

• 11.7 g

• 58.7 g

• 294 g

Which of the following best accounts for the fact that a galvanic cell based on the reaction represented above will generate electricity?

• Cl₂ can easily lose two electrons.

• Cl₂ is a stronger oxidizing agent than I₂.

• I atoms have more electrons than do atoms of Cl.

• I^- is more stable species than I₂.

• I₂(s) is more soluble than Cl₂(g).

How many electrons are transferred in the reaction represented by the balanced equation above?

• 2

• 4

• 5

• 8

• 10

An electric current of 1.00 ampere is passed through an aqueous solution of Ni(NO₃)₂. How long will it take to plate out exactly 1.00 mol of nickel metal, assuming 100 percent current efficiency? (1 Faraday = 96,500 coulombs = 6.02 x 10²³ electrons)

• 386,000 sec

• 193,000 sec

• 96,500 sec

• 48,200 sec

• 24,100 sec

Oxygen is acting as an oxidizing agent in all of the following reactions EXCEPT

• 2C(s) + O₂(g) → 2CO(g)

• S(s) + O₂(g) → SO₂(g)

• 2F₂(g) + O₂(g) → 2OF₂(g)

• 2Na(s) + O₂(g) → Na₂O₂(s)

• 2Mg(s) + O₂(g) → 2MgO(s)