ELECTROLYSIS CELL QUIZ Part III

1.An electrolysis of a titanium fluoride complex ion using 1.20 A for 20 min produces 0.179 g of titanium metal. What is the charge of titanium in the material? (Ar: Ti = 48)
a)6
b)4
c)3
d)2
e)1
2.It is possible to extract many metals via the electrolysis of aqueous solutions of their ions. Such an experiment is carried out by passing 3.00 Amps, for 2.00 hours, through a solution of metal ions that carry a 2+ charge. 7.11 grams of the metal was produced. Identify the metal.
a) Ba
b) Cu
c) Ni
d) Sr
e) Zn
3.How long would it take in minutes, to produce 5.60 g of Zinc metal from a solution of zinc nitrate using a current of 2.00 Amps?
a) 138
b) 826
c) 65.4
d) 6.54
e) 2.00
4.When molten Copper (II) chloride is electrolyzed by passing 4.00 Amps for 400. seconds what is the maximum mass of copper metal that can be deposited?
a) 0.526 g
b) 63.5 g
c) 6.35 g
d) 1600 g
e) 96500 g
5.With a current of 20 amps, how long would it take to generate 1.00 kilograms of aluminum by the reaction:
Al3+ + 3e- → Al(s)
a)2.19 x 104 sec
b)1.68 x 102 sec
c)1.78 x 105 sec
d)5.35 x 105 sec
e)3.90 x 103 sec
6.This picture of an electrochemical cell can best be described as:
a)a complete galvanic cell
b)a complete electrolytic cell
c)an electrolytic cell, but missing at least one essential component
d)a galvanic cell, but missing at least one essential component
7.A mole of electrons has a charge of 96,485 coulombs per mole of electrons. This quantity is known to chemists as ….
a)1 joule
b)1 watt
c)1 ampere
d)1 volt
e)1 faraday
8.In the electrolytic decomposition of water ….
2H2O → 2H2 + O2
a)hydrogen is formed at both the anode and the cathode
b)hydrogen is formed at the cathode and oxygen is formed at the anode
c)hydrogen is formed at the anode and oxygen is formed at the cathode
9.oxygen is formed at both the anode and the cathode
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?
a)1.25 g
b)1.47 g
c)0.736 g
d)0.368 g
e)2.65 g
10.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?
a)19.5 g
b)39.0 g
c)1.43 x 103 g
d)126 g
e)0.985 g
11.In an electrolytic cell, the negative electrode is called the ….
a) anode, at which oxidation occurs
b) anode, at which reduction occurs
c) cathode, at which oxidation occurs
d) cathode, at which reduction occurs
12.If the electrolytically driven reaction below, how many grams of material will be produced at the anode by a current of 3.0 A flowing for 1 hour?
Au3+(aq) + Fe(s) <=> Au+(aq) + Fe2+(aq)
a) 5.5 g
b) 22.0 g
c) 3.13 g
d) 6.26 g
e) 11.0 g
13.Identify the INCORRECT statement in the following:
a) In a voltaic cell a spontaneous reaction is taking place and producing electric current.
b) The gain of electrons takes place at the cathode.
c) Measuring the potential of a cell provides a direct determination of the free energy of the cell reaction.
d) Sodium metal and chlorine gas are produced in an electrolytic cell containing aqueous NaCl.
e) Faraday¹s number is the amount of charge in Coulombs of one mole of electrons.
14.How many grams of gold could be plated out on the cathode of an electrolytic cell by the passage of 0.5 Amps of current through AuNO3 solution for 30 minutes?
a) 3.07 x 10-2 g
b) 2.41 g
c) 1.84 g
d) 3.68 g
e) 17.9 g
15.What is the charge on an ion of tin if 7.42 g of metallic tin is plated out by the passage of 24125 Coulombs through a solution containing the ion?
a) +4
b) +3
c) +2
d) +1
e) 0