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WorksheetsElectrochemistry
Total questions: 28
Worksheet time: 5hrs 0mins
It is referred as the study of the interchange of chemical and electrical energy.
Electrochemical energy
Electrochemistry
Redox reaction
Electrolysis
Electricity
It is defined as energy that converts from electrical to chemical energy vice versa.
Electrochemical energy
Electrochemistry
Redox Reaction
Electrolysis
Electricity
The driving force behind the electron transfer is called the cell potential (Voltage).
True
False
The substance that is oxidized is referred to as a oxidizing agent.
True
False
In any redox reaction, both oxidation and reduction must occur.
True
False
An acidic solution contains H+ ions and H2O-.
True
False
A basic solution contains OH- ions and H2O.
True
False
Reduction is the process of gaining electron.
True
Flase
F2 + 2e− ⟶ 2F
Oxidation Reaction
Reduction Reaction
H2O2→ H2O
Oxidation Reaction
Reduction Reaction
Ag ⟶ Ag+ + e−
Oxidation Reaction
Reduction Reaction
Fe ⟶ Fe3+
Oxidation Reaction
Reduction Reaction
(Balancing Half-Reaction Method in acidic solution)
Hg2+(aq) + N2H4 (aq) ⟶ Hg (l) + N2 (g)
2Hg2+(aq) + N2H4 (aq) ⟶ 2 Hg (l) + N2 (g) + H2O(l) +4H+(aq)
Hg2+(aq) + N2H4 (aq) ⟶ Hg (l) + N2 (g) + 4H+(aq)
2Hg2+(aq) + N2H4 (aq) ⟶ 2 Hg (l) + N2 (g) + 4H+(aq)
2Hg2+(aq) + N2H4 (aq) ⟶ 2Hg (l) + N2(g) + H2O(l) +4H-(aq)
Balancing Half-reaction in Basic solution
H2O2 (aq) + Cl2O7 (g) ⟶ ClO2-(aq) + O2(g)
3 H2O2(aq) + Cl2O7 (g) + 2OH-(aq) ⟶ 2ClO2-(aq) + 5H2O(l) + O2(g)
4 H2O2(aq) + Cl2O7 (g) + 2OH-(aq) ⟶ 2ClO2-(aq) + 4H2O(l) + O2(g)
4 H2O2 (aq) + Cl2O7 (g) + OH-(aq) ⟶ 2ClO2-(aq) + 4H2O(l) + O2(g)
4 H2O2 (aq) + Cl2O7 (g) + 2OH-(aq) ⟶ 2ClO2-(aq) + 5H2O(l) + 4O2(g)
Determine the ΔG, use F= 96458 J/V mol e-:
+0.434 V, n = 2
83748.98 J/mol
-83748.98 J/mol
-83.760 kJ/mol
84 kJ/mol
Determine the ΔG, use F= 96458 J/V mol e-:
-0.311 V, n = 3
89.980 kJ/mol
89.995 kJ/mol
91 kJ/mol
89.994 kJ/mol
In the Mg(s) + Ni2+(aq) ⟶ Mg2+ (aq) + Ni(s) equation which is reduction half reaction?
Mg(s) ⟶ Mg2+ (aq)
Ni2+(aq) ⟶ Ni(s)
Determine the standard cell potential for the cell:
Mg(s) + Ni2+(aq) ⟶ Mg2+ (aq) + Ni(s)
E ocell = 2.60 V
E ocell = 2.14 V
E ocell = -2.60 V
E ocell = -2.14 V
Determine the nonstandard cell potential for the cell
Mg(s) + Ni2+(aq, 1.22 M ) ⟶ Mg2+ (aq, 0.67 M) + Ni(s)
E cell = - 2.1554 V
E cell = - 2.6154V
E cell = 2.1554 V
E cell = - 2.6154V
In the Ag+(aq) + Cu+(s) ⟶ Ag(s) + Cu2+(aq) equation which is reducing agent?
Cu+(s) ⟶ Cu2+(aq)
Ag+(aq) ⟶ Ag(s)
Determine the standard cell potential for the cell:
Ag+(aq) + Cu+(s) ⟶ Ag(s) + Cu2+(aq)
E ocell = 0.64 V
E ocell = 0.96 V
E ocell = -0.64 V
E ocell = -0.96 V
Determine the nonstandard cell potential for the cell
Ag+(aq, 0.20 M) + Cu+(s) ⟶ Ag(s) + Cu2+ (aq, 0.12 M)
E cell = 0.6118 V
E cell = - 0.6118 V
E cell = - 0.9718 V
E cell = 0.9718 V
Calculate the cell potentials-Standard potential:
Fe(s)│Fe2+(aq) ││Hg22+(aq) │Hg2+ (l)
E ocell = 0.47 V
E ocell = - 0.47 V
E ocell = 1.35 V
E ocell = - 1.35 V
What is the value of n in the Fe(s)│Fe2+(aq) ││Hg22+(aq) │Hg2+ (l) ? (just write the number)
(a)
Calculate the cell Potentials-Standard potential
Pt(s) │Cl2(g) │Cl-(aq) ││Au3+(aq) │Au(s)
E ocell = 0.14 V
E ocell = - 0.14 V
E ocell = 2.86 V
E ocell = - 2.86 V
What is the value of n in the Pt(s) │Cl2(g) │Cl-(aq) ││Au3+(aq) │Au(s)? (just write the number)
(a)
In a process called flash electroplating, a current of 2.90 x 103 A passes through an electrolytic cell for 8.00 minutes. How many moles of electrons are driven through the cell? (use 96,485 C)
-14.4271 mol e-
14.4271 mol e-
-14.4272 mol e-
14.4272 mol e-
An electrolysis cell that deposits gold (from Au+(aq)) operates for 15.0 minutes at a current of 2.30 A. What mass of gold is deposited?
(a)
