Worksheets11ElectrochemistryPracticeTest
Total questions: 23
Worksheet time: 46mins
Which of the following is the correct cell notation for the reaction
Hg22+ + Cd(s) → Cd2+ + 2Hg(l)
Cd2+ | Cd | | Hg22+ | Hg
Cd2+ | Hg22+ | | Cd | Hg
Cd | Cd2+ | | Hg22+ | Hg
Cd2+ | Hg | | Hg22+ | Cd
Hg | Cd | | Hg22+ | Cd2+
Consider an electrochemical cell where the following reaction takes place:
3Sn2+(aq) + 2Al(s) → 3Sn(s) + 2Al3+(aq)
Which of the following is the correct cell notation for this cell?
Al | Al3+ | | Sn2+ | Sn
Al3+ | Al | | Sn | Sn2+
Sn | Sn2+ | | Al3+ | Al
Sn | Al3+ | | Al | Sn2+
Al | Sn2+ | | Sn | Al3+
An early method of producing aluminum metal was the reaction of aluminum salts with sodium metal:
Al3+ + 3Na(s) ↔ Al(s) + 3Na+ E° = +1.05 V
What is ΔG° for this reaction
-304 kJ
-101 kJ
+101 kJ
+202 kJ
+304 kJ
Calculate ΔG for the following reaction:
I2(s) + 2Br-(aq) → 2I-(aq) + Br2(l)
+105 kJ
-105 kJ
+312 kJ
+52 kJ
-312 kJ
If ΔG of the following reaction is -203 kJ, what is E°?
2Ag+(aq) + Ni(s) → 2Ag(s) + Ni2+(aq)
-1.05 V
+2.10 V
+0.0011 V
-0.011 V
+1.05 V
Given the two half reactions and their potentials, which net reaction is spontaneous?
Mg2+(aq) + 2e- → Mg(s) E° = -2.37 V
Ni2+(aq) + 2e- → Ni(s) E° = -0.25 V
Ni(s) + Mg2+(aq) → Mg(s) + Ni2+(aq)
Ni2+(aq) + Mg(s) → Mg2+(aq) + Ni(s)
Ni(s) + Mg(s) → Mg2+(aq) + Ni2+(aq)
Mg2+(aq) + Ni2+(aq) → Mg(s) + Ni(s)
Mg2+(aq) + Mg(s) → Ni(s) + Ni2+(aq)
Calculate E° for the following reaction:
Sn4+(aq) + 2K(s) → Sn2+(aq) + 2K+(aq)
+6.00 V
-3.08 V
+3.08 V
+2.78 V
-2.78 V
Calculate E° for the following reaction:
2Al3+(aq) + 3Cd(s) → 2Al(s) + 3Cd2+(aq)
-2.06 V
+4.52 V
+2.06 V
-4.52 V
-1.26 V
Using data from the reduction potential table and the reaction
2Ag(s) + Pt2+(aq) → Pt(s) + 2Ag+(aq) E° = 0.38 V
calculate the standard reduction potential of the half-reaction
Pt2+(aq) + 2e- → Pt(s)
-1.18 V
-0.40 V
0.40 V
1.18 V
2.00 V
An electrochemical cell of notation Pd | Pd2+ | | Cu2+ | Cu has an E° = -0.65 V. If we know that the standard reduction potential of Cu2+/Cu is E° = 0.34 V, what is the standard reduction potential for Pd2+/Pd?
-0.99 V
-0.31 V
+0.31 V
0.62 V
+0.99 V
What is the equilibrium constant for the following reaction at 298 K?
2Ag+(aq) + 2I-(aq) → I2(s) + 2Ag(s); E° = +0.265 V
2.99 x 104
9.04 x 108
7.73 x 103
87.9
1.60 x 107
What is the equilibrium constant for the following reaction at 20C?
Fe(s) + Cu2+(aq) → Fe2+(aq) + Cu(s); E° = +0.78 V
2.3 x 1026
6.9 x 1026
1.4 x 1027
1.8 x 1028
1.2 x 10-21
What is the cell potential for
3Sn4+(aq) + 2Al(s) → 3Sn2+(aq) + 2Al3+(aq)
E° = 1.81 V when [Sn4+] = 1.0, [Sn2+] = 1.0 x 10-2, and
[Al3+] = 1.5 x 10-3 at 298 K.
1.70 V
1.76 V
1.81 V
1.86 V
1.93 V
If the potential cell is +1.32 V at Q = 0.0969 with n = 2, what is the standard potential of the cell?
+1.35 V
+1.48 V
+1.31 V
+1.34 V
+1.29 V
Predict the product at the anode when electric current is passed through a solution of KI.
I2(l)
K+(aq)
H2(g)
K(s)
O2(g)
If electric current is passed through aqueous LiBr, the product at the cathode would be __________ and the product at the anode would be __________.
H2O(l), Li+(aq)
Br2(l), Li(s)
Li(s), Br2(l)
Br2(l), H2(g)
H2(g), Br2(l)
How long would it take to deposit 1.36 g of copper from an aqueous solution of copper(II) sulfate by passing a current of two amperes through the solution?
2070 sec
1.11 x 10-5 sec
2570 sec
736 sec
1030 sec
If a current of 6.0 amps is passed through a solution of Ag+ for 1.5 hours, how many grams of silver are produced?
0.60 g
36 g
0.34 g
3.0 g
1.0 g
How many kilowatt hours of electrical energy are required to plate 2.00 grams of silver from an aqueous solution of silver nitrate on to a necklace using 3.00V? (1 joule = 1 volt-coulomb and 1 kwh = 3.60 x 106 J)
0.00135 kwh
0.000165 kwh
32.4 kwh
0.00149 kwh
2.07 kwh
Using data from the reduction potential table, predict which of the following is the best oxidizing agent.
F2
Ag
Sn4+
Ag+
Al3+
Under acidic conditions the bromate ion is reduced to the bromide ion. Write the balanced half-reaction for this process.
BrO3- + 6H+ + 6e → Br- + 3H2O
2BrO3- + 6H+ → Br2- +6H2O + 3e
BrO3- + 6H2O + 10e → Br2- + 12H+ + 3 O2
2BrO3- + 6H2O → 2Br- + 12H+ + 6 O2 + 8e
2BrO3- + 6H+ → Br2- + 3H2O + 3e
Balance the following redox equation which occurs in acidic solution.
N2H4(g) + BrO3-(aq) → Br-(aq) + N2(g)
3N2H4 + BrO3- → 3N2 + Br- + 3H2O + 6H+
N2H4 + BrO3- + 2H+ → 2Br- + N2 +3H2O
3N2H4 + 2BrO3- + 12H+ → 3N2 + 2Br- + 6H2O + 12H+
N2H4 + 2BrO3- + 8H+ → 2Br- + N2 + 6H2O
3N2H4 + 2BrO3- → 3N2 + 2Br- + 6H2O
Which of the following reactions is NOT a redox reaction?
2HgO(s) → 2 Hg(l) + O2(g)
H2(g) + Br2(g) → 2HBr(g)
2HCl(aq) + Zn(s) → H2(g) + ZnCl2(aq)
H2CO3(aq) → H2O(l) + CO2(g)
2KClO3 → 2KCl(s) + 3 O2(g)
