AP Chemistry Review Questions

In all electrochemical cells, the process that takes place at the anode is _________________ and the process that takes place at the cathode is _________________.
1. reduction, oxidation
2. oxidation, reduction
3. reduction, reduction
4. oxidation, oxidation
The standard hydrogen electrode is assigned a potential of:
1. zero volts
2. 1.00 volts
3. -1.00 volts
4. 0.76 volts
Calculate the value of E⁰_cell for a galvanic cell that contains the following half cells:
- Cl₂ + 2e^- → 2Cl^- (E⁰ = 1.36v)
- Cu⁺ + e^- → Cu (E⁰ = 0.52v)
1. E⁰_cell = 0.32 volts
2. E⁰_cell = 0.84 volts
3. E⁰_cell = -0.32 volts
4. E⁰_cell = -0.84 volts
5. E⁰_cell = 1.88 volts
For the galvanic cell described below, the correct line notation is:
- Cl₂ + 2e^- → 2Cl^- (E⁰ = 1.36v)
- Cu⁺ + e^- → Cu (E⁰ = 0.52v)
1. Cu(s)|Cu⁺(aq)||Cl₂(g)|2Cl^-(aq)
2. Pt(s)|Cu(s)|Cu⁺(aq)||Cl₂(g)|2Cl^-(aq)|Pt(s)
3. Cu(s)|Cu⁺(aq)||Cl₂(g)|2Cl^-(aq)|Pt(s)
4. Pt(s)|Cl₂(g)|2Cl^-(aq)||Cu(s)|Cu⁺(aq)|Pt(s)
5. Pt(s)|Cl₂(g)|2Cl^-(aq)||Cu(s)|Cu⁺(aq)
Calculate DG⁰ for the reaction:
- Cl₂ + 2e^- → 2Cl^- (E⁰ = 1.36v)
- Cu⁺ + e^- → Cu (E⁰ = 0.52v)
1. -8.1 x 10⁴ J
2. 8.1 x 10⁵ J
3. -3.1 x 10⁴ J
4. -6.2 x 10⁴ J
5. -1.6 x 10⁵ J
The equilibrium constant (K) for the reaction below is approximately:
- Cl₂ + 2e^- → 2Cl^- (E⁰ = 1.36v)
- Cu⁺ + e^- → Cu (E⁰ = 0.52v)
1. 10²⁸
2. 10¹⁷
3. 10²
4. 10^-34
5. 10¹¹
This picture of an electrochemical cell can best be described as:
1. a complete electrolytic cell
2. an electrolytic cell, but missing at least one essential component
3. a complete galvanic cell
4. a galvanic cell, but missing at least one essential component
Reduction potential is:
1. always positive
2. an intensive property
3. an extensive property
4. measured in amperes
A mole of electrons has a charge of 96,485 coulombs per mole of electrons. This quantity is known to chemists as:
1. 1 ampere
2. 1 volt
3. 1 joule
4. 1 faraday
5. 1 watt
What is the oxidation state of S in H₂SO₃?
1. +6
2. +4
3. +2
4. 0
5. -3
The equation that represents a reaction that is not a redox reaction is:

1. 2H₂ + O₂ → 2H₂O

2. Zn + CuSO₄ → ZnSO₄ + Cu

3. 2H₂O₂ → 2H₂O + O₂

4. H₂O + CO₂ → H₂CO₃
1. Reaction 1
2. Reaction 2
3. Reaction 3
4. Reaction 4
5. All of these are redox reactions
How many electrons are transferred in the following reaction?

2NaCl + 2H₂SO₄ + MnO₂ → Na₂SO₄ + MnSO₄ + 2H₂O + Cl₂
1. 1
2. 2
3. 4
4. 6
5. 8
In the reaction below, the substance that is reduced is:

2NaCl + 2H₂SO₄ + MnO₂ → Na₂SO₄ + MnSO₄ + 2H₂O + Cl₂
1. Na⁺
2. Cl^-
3. H⁺
4. Mn⁴⁺
5. O^2-
Which of the following would be most easily oxidized?
1. Na
2. Na⁺
3. F^-
4. Cl₂
5. O^2-
In the electrolytic decomposition of water:

2H₂O → 2H₂ + O₂
1. hydrogen is formed at the cathode and oxygen is formed at the anode
2. hydrogen is formed at the anode and oxygen is formed at the cathode
3. hydrogen is formed at both the anode and the cathode
4. oxygen is formed at both the anode and the cathode
What value of E do you expect for
Pb(s) → Pb²⁺ + 2e^-

in 0.015m Pb²⁺ solution? E⁰ = +0.13v
1. E = +0.13v
2. E = +0.18v
3. E = +0.83v
4. E = +0.27v
5. E = 0.00v
The current in a given wire is 1.80 amp. How many coulombs will pass a given point on the wire in 1.36 minutes?
1. 2.45 C
2. 1.32 C
3. 45.3 C
4. 147 C
5. 253 C
Two cells, one containing aqueous AgNO₃ and the other containing CuSO₄ are set up in series. In a given electrolysis that results in depositing 1.25 g of silver in the first cell, how much copper should deposit simultaneously in the second cell?
1. 1.25 g
2. 0.736 g
3. 0.368 g
4. 1.47 g
5. 2.65 g
With a current of 20.0 amps, how long would it take to generate 1.00 kilograms of aluminum by the reaction:

Al³⁺ + 3e^- → Al(s)
1. 5.36 x 10⁵ sec
2. 1.78 x 10⁵ sec
3. 2.19 x 10⁴ sec
4. 3.90 x 10³ sec
5. 1.68 x 10² sec
If a constant current of 8.00 amperes is passed through a cell containing Zn²⁺ for 2.00 hours, how many grams of zinc will plate out onto the cathode?
1. 39.0 g
2. 19.5 g
3. 0.985 g
4. 126 g
5. 1.43 x 10³ g

AP Chemistry Review Questions - Electrochemistry