Multiple Choice ( Select 1 out of 4 options, for ne question below.
Which Process uses an electrolytic aqueous solution concentration as 10 to 25%.
Answers
Answer:
In an electrolytic cell the electrode at which the electrons enter the solution is called the ______ ; the chemical change that occurs at this electrode is called _______.
(a) anode, oxidation
(b) anode, reduction
(c) cathode, oxidation
(d) cathode, reduction
(e) cannot tell unless we know the species being oxidized and reduced.
2.
Which of the following statements is FALSE?
(a) Oxidation and reduction half-reactions occur at electrodes in electrochemical cells.
(b) All electrochemical reactions involve the transfer of electrons.
(c) Reduction occurs at the cathode.
(d) Oxidation occurs at the anode.
(e) All voltaic (galvanic) cells involve the use of electricity to initiate nonspontaneous chemical reactions.
3.
The half-reaction that occurs at the anode during the electrolysis of molten sodium bromide is:
(a) 2 Br- Br2 + 2 e-
(b) Br2 + 2 e- 2 Br-
(c) Na+ + e- Na
(d) Na Na+ + e-
(e) 2 H2O + 2 e- 2 OH- + H2
4.
During the electrolysis of aqueous KCl solution using inert electrodes, gaseous hydrogen is evolved at one electrode and gaseous chlorine at the other electrode. The solution around the electrode at which hydrogen gas is evolved becomes basic as the electrolysis proceeds. Which of the following responses describe or are applicable to the cathode and the reaction that occurs at the cathode?
(1) the positive electrode (2) the negative electrode
(3) 2 Cl- Cl2 + 2 e- (4) Cl2 + 2 e- 2 Cl-
(5) 2 H2O O2 + 4 H+ + 4 e- (6) 2 H2O + 2 e- H2 + 2 OH-
(7) electrons flow from the electrode to the external circuit (8) electrons flow into the electrode from the external circuit
(9) oxidation (10) reduction
(a) 2, 6, 8, 9
(b) 1, 5, 7, 9
(c) 2, 5, 7, 9
(d) 1, 6, 8, 10
(e) 2, 6, 8, 10
5.
What mass (in grams) of nickel could be electroplated from a solution of nickel(II) chloride by a current of 0.25 amperes flowing for 10 hours?
(a) 12 g
(b) 5.5 g
(c) 0.046 g
(d) 2.7 g
(e) 6.0 g
6.
Molten AlCl3 is electrolyzed for 5.0 hours with a current of 0.40 amperes. Metallic aluminum is produced at one electrode and chlorine gas, Cl2, is produced at the other. How many liters of Cl2 measured at STP are produced when the electrode efficiency is only 65%?
(a) 0.55 L
(b) 0.63 L
(c) 0.84 L
(d) 0.98 L
(e) 1.02 L
7.
How long (in hours) must a current of 5.0 amperes be maintained to electroplate 60 g of calcium from molten CaCl2?
(a) 27 hours
(b) 8.3 hours
(c) 11 hours
(d) 16 hours
(e) 5.9 hours
8.
How long, in hours, would be required for the electroplating of 78 g of platinum from a solution of [PtCl6]2-, using an average current of 10 amperes at an 80% electrode efficiency?
(a) 8.4
(b) 5.4
(c) 16.8
(d) 11.2
(e) 12.4
9.
How many faradays are required to reduce 1.00 g of aluminum(III) to the aluminum metal?
(a) 1.00
(b) 1.50
(c) 3.00
(d) 0.111
(e) 0.250
10.
Which of the following is the strongest oxidizing agent?
(a) Pb2+
(b) I2
(c) Ag+
(d) Pb
(e) Cu2+