1. Which of the following terms can be used to describe an electrochemical cell
ID: 879913 • Letter: 1
Question
1. Which of the following terms can be used to describe an electrochemical cell in which a spontaneous chemical reaction generates an electric current?
(1) Electrolytic Cell (2) Galvanic Cell (3) Battery
A. (1) B. (2) C. (3) D. (2) and (3) E. (1), (2), and (3)
2. How many moles of electrons are transferred in the following oxidation-reduction reaction?
2MnO4–(aq) + 16H+(aq) + 10Cl–(aq) 2Mn2+ + 5Cl2(g) + 8H2O(l)
A. 1 B. 2 C. 4 D. 5 E. 10
3. A standard state galvanic cell is constructed using the Mg2+/Mg and Br2/Br– redox couples. What is the cell potential?
A. –3.46 V B. –1.28 V C. 1.28 V D. 1.73 V E. 3.46 V
4. A galvanic cell consists of Ag+/Ag and Cu2+/Cu half-cells. What species are produced at the electrodes under standard state conditions?
A. Ag(s) is formed at the cathode and Cu(s) is formed at the anode.
B. Ag(s) is formed at the cathode and Cu2+ is formed at the anode.
C. Cu(s) is formed at the cathode and Ag+ is formed at the anode.
D. Cu2+ is formed at the cathode and Ag+ is formed at the anode.
E. Cu2+ is formed at the cathode and Ag(s) is formed at the anode.
5. Consider the redox couples shown below. Of these, which species is the strongest oxidizing agent and which is the strongest reducing agent?
Ag+/Ag Cd2+/Cd
A. Oxidizing Agent: Ag Reducing Agent: Cd2+
B. Oxidizing Agent: Ag+ Reducing Agent: Cd
C. Oxidizing Agent: Ag+ Reducing Agent: Cd2+
D. Oxidizing Agent: Cd2+ Reducing Agent: Ag
E. Oxidizing Agent: Cd Reducing Agent: Ag+
Explanation / Answer
1. Answer: (2) Galvanic cell
2.
2MnO4–(aq) + 16H+(aq) + 10Cl–(aq) 2Mn2+ + 5Cl2(g) + 8H2O(l)
Here Mn is reduced from +7 to +2 (x2 = 10 electron)
Cl- is oxidised from -1 to 0 (X10 = 10 electron)
Answer: E.10
3.
Eo (Br2/Br–) = 1.1V (CATHODE)
Eo (Mg2+/Mg) = -2.36 V (ANODE)
Eo = Eo(cathode) - Eo(anode)
= 1.1 - (-2.36)
= 3.46 V
answer: E
4.
Eo(Ag+/Ag) = 0.8 V
Eo(Cu2+/Cu) = 0.34 V
Greater reduction potential will occur at cathode.
Ag+ ---> Ag (at cathode)
Cu -----> Cu2+ (at anode)
Answer: B
5.
Eo(Ag+/Ag) = 0.8 V
Eo (Cd2+/Cd) = -0.4 V
Greater reduction potential implies oxiding agent
reduction reaction: Ag+ ---> Ag
Oxidation reaction: Cd ----> Cd2+
Answer: B
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