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15. Basic Chemistry: Redox Reaction

Total questions: 25

Worksheet time: 2hrs 14mins

Name
Class
Date
1.

In the following unbalanced equations, indicate the reactant oxidized.

Al + HCl → AlCl3 + H2Al\ +\ HCl\ \rightarrow\ AlCl_3\ +\ H_2

a)

Al

b)

HCl

c)

AlCl3

d)

H2

2.

Which of the following reactions are oxidation–

reduction reactions?

a)

(a)

b)

(b)

c)

(c)

d)

(d)

e)

(e)

3.

Predict whether the following reactions occur in aqueous solution. 2Na+2H2O ⟶ H2+2NaOH2Na+2H_2O\ \longrightarrow\ H_2+2NaOH

a)

Reaction predicted to be

favourable

b)

No reaction

c)

Can not be defined

4.

Predict whether the following reactions occur in aqueous solution. Fe+2H2O → Fe2++2OH−+H2Fe+2H_2O\ \rightarrow\ Fe^{2+}+2OH^-+H_2

a)

Reaction predicted to be

favourable

b)

No reaction

c)

Can not be defined

5.

In an alkaline battery, the following two half reactions occur. Which reaction takes place at the anode?

a)

Zn(s)

b)

MnO2(s)

c)

both reaction

d)

no reaction happened

e)

can not be defined

6.

The nickel–cadmium (nicad) battery is used as a replacement for a dry cell because it is rechargeable. The overall reaction that takes place is NiO2(s)+Cd(s)+2H2O(l) → Ni(OH)2(s)+Cd(OH)2(s)NiO_{2(s)}+Cd_{(s)}+2H_2O_{(l)}\ \rightarrow\ Ni(OH)_{2(s)}+Cd(OH)_{2(s)}

What is the half-reactions that take place at the anode and the cathode?

a)

anode: Cd

cathode: H2O

b)

anode: NiO2

cathode: Cd

c)

anode: NiO2

cathode: H2O

d)

anode: Cd

cathode: NiO2

e)

there's no correct answer

7.

In basic solution, Se2- and SO32- ions react spontaneously as seen on picture. If E°sulfite is -0.57 V, calculate E°selenium.

a)

-0.22

b)

0.92

c)

-0.92

d)

we can not calculate E°selenium

e)

0.22

8.

A voltaic cell houses the reaction between aqueous bromine and zinc metal as shown in picture. if given E°zinc is -0.74V, calculate E°bromine.

a)

2.57 V

b)

-2.57 V

c)

-1.07 V

d)

can not be calculated

e)

1.07 V

9.

Certain metals can be purified by electrolysis. For example, a mixture of Ag, Zn, and Fe can be dissolved so that the metal ions are present in an aqueous solution. If a solution containing these ions is electrolysed, which metal ion will be reduced to metal first?

a)

Ag and Zn together

b)
Zn
c)
Fe
d)
Ag
e)

All three metals cannot be reduced.

10.

In a Galvanic Cell, the charge of anode and cathode respectively are ...............

a)
Anode: positive, Cathode: positive
b)
Anode: neutral, Cathode: neutral
c)
Anode: negative, Cathode: positive
d)
Anode: positive, Cathode: negative
e)
Anode: negative, Cathode: neutral
11.

In a Galvanic Cell, reduction and oxidation reaction take place in...............

a)

Oxidation: anode

Reduction: cathode

b)

Oxidation: cathode

Reduction: anode

c)

Oxidation: external circuit

Reduction: internal circuit

d)

Oxidation: electrolyte solution

Reduction: salt bridge

e)

Both reaction happen in the cell

12.

In any Galvanic Cell, which half cell will undergo reduction?

a)

The half cell with the higher standard electrode potential.

b)
The entire cell undergoes reduction.
c)
The electrolyte solution undergoes reduction.
d)
Both half-cells undergo reduction equally.
e)

The half cell with the lower standard electrode potential.

13.

Consider the galvanic cell reaction Zn(s) + Cu2+(aq) → Cu(s) + Zn2+(aq) When the cell is running spontaneously, which is the only true statement?

a)
Zinc is oxidized and acts as the anode.
b)

The zinc electrode loses mass and the zinc electrode is the cathode.

c)

The copper electrode gains mass and the copper electrode is the cathode.

d)
Zinc is reduced and acts as the cathode.
e)
Copper is oxidized and acts as the anode.
14.

A certain galvanic cell has for its spontaneous cell reaction: Zn + HgO → ZnO + Hg

Which is the half-reaction occurring at the anode?

a)
ZnO + 2e- → Zn
b)
Zn + 2e- → ZnO
c)
Zn → ZnO + 2e-
d)
HgO + 2e- → Hg
e)
Hg → HgO + 2e-
15.

E0cell = ................

a)
E0cell = E0cathode + E0anode
b)

E0cell = E0cathode x E0anode

c)
E0cell = E0anode - E0cathode
d)
E0cell = E0cathode / E0anode
e)
E0cell = E0cathode - E0anode
16.

A galvanic cell is established to power a torch, as shown. For this cell, the overall equation will be 2Al(s) + 6H+(aq) → 2Al3+ (aq) + 3H2(g). For this cell, select the correct statement/s about this cell.

a)
Aluminum is reduced and hydrogen ions are oxidized in the galvanic cell.
b)

Hydrogen ions are oxidized and aluminum is reduced in the galvanic cell.

c)
Aluminum is oxidized and hydrogen ions are reduced in the galvanic cell.
d)

Concentration of aluminium ions in solution will be falling.

e)

Electrons will flow from the aluminium to the hydrogen half-cell.

17.

Calculate the cell potential of voltaic cell.

a)

–1.51

b)

-0.03

c)

+0.03

d)

+1.51

e)

there's no correct answer

18.

Calculate the cell potential of voltaic cell.

a)

–1.60 V

b)

+1.60 V

c)

–3.12 V

d)

+3.12 V

e)

there's no correct answer

19.

What is the equation and cell potential?

a)

2Al3+ + 3Ni → 2Al + 3Ni2+ E0 = 1.89 V

b)

2Al + 3Ni2+ → 2Al3+ + 3Ni E0 = 1.89 V

c)

2Al3+ + 3Ni → 2Al + 3Ni2+ E0 = 1.43 V

d)

2Al + 3Ni2+ → 2Al3+ + 3Ni E0 = 1.43 V

e)

2Al + 3Ni2+ → 2Al3+ + 3Ni E0 = -1.43 V

20.

Given the standard reduction potentials, E0 of iron is -0.44V and E0 of oxygen is +1.23V.

What will be the emf of the cell?

a)
1.67V
b)

-0.79V

c)

-1.67V

d)
-0.44V
e)

+0.79V

21.

Nernst equation for an electrode is based on the variation of electrode potential of an electrode with .......

a)
pH level of the solution
b)
temperature of the solution
c)
volume of the solution
d)
pressure of the gas
e)
concentration of ions
22.

Given their standard reduction potentials, which of the species is going to be oxidized?

Cu2+/Cu = 0.34V

Zn2+/Zn = -0.76V

a)

CuSO4

b)
Zn
c)
Fe
d)
Cu
e)

ZnSO4

23.

Nernst equation for

Mg(s) | Mg2+(aq, 0.001M) || Al3+(aq, 0.001 M) | Al (s)

a)

E = E° - (0.0592/3) log[Mg2+]3/ [Al3+]2

b)

E = E° - (0.0592/2) log[Al3+]2/ [Mg2+]2

c)

E = E° -(0.0592/2) log[Al3+]3/ [Mg2+]2

d)

E = E° - (0.0592/6) log[Mg2+]3/ [Al3+]2

e)

E = E° - (0.0592/2) log[Mg2+] /[Al3+]

24.

Calculate the Ecell for the following galvanic cell.

Zn(s) | Zn2+ (aq, 1.0M) || Ag+ (aq, 1.5M) | Ag(s)

EAg+ | Ag = +1.08V and EZn2+ | Zn = -0.76V

a)

0.32V

b)
-0.76V
c)

1.85V

d)
2.00V
e)

1.84V

25.

Calculate the cell potential, Ecell of the electrochemical cell in which reaction

Pb2+ (aq) + Cd (s) → Pb (s) + Cd2+ (aq)

Given that Eocell = +0.277 V,

[Cd2+] = 0.02M, and [Pb2+] = 0.2M.

a)

0.307 V

b)
0.295 V
c)

0.355 V

d)
0.300 V
e)
0.250 V

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