CHEMISTRY

(Q&A Bank for CEE & JEE Mains)

Assam Electronics Development Corporation Limited

(AMTRON) (A Government of Assam Undertaking)

Name of the textbook

Chemistry

Name of the Chapter

Redox Reactions (Unit 8)

Questions – Redox Reaction CEE & JEE Mains Exams

1

LEVEL 1

1. EMF of a cell in terms of reduction potential

of its left and right electrodes is

(a) E = Eleft – Eright (b) E = Eleft + Eright

(c) E = Eright – Eleft (d) E = –(Eright + Eleft).

2. When KMnO4 acts as an oxidising agent

and ultimately forms [MnO4]–1, MnO2,

Mn2O3, Mn2+ then the number of electrons

transferred in each case respectively is

(a) 4, 3, 1, 5

(b) 1, 5, 3, 7

(c) 1, 3, 4, 5

(d) 3, 5, 7, 1.

3. Which of the following is a redox reaction?

(a) NaCl + KNO3 → NaNO3 + KCl

(b) CaC2O4 + 2HCl → CaCl2 + H2C2O4

(c) Mg(OH)2 + 2NH4Cl → MgCl2 + 2NH4OH

(d) Zn + 2AgCN → 2Ag + Zn(CN)2.

4. Conductivity (unit Siemen's S) is directly

proportional to area of the vessel and the

concentration of the solution in it and is

inversely proportional to the length of the

vessel then the unit of the constant of

proportionality is

(a) Smmol–1

(b) Sm2mol–1

(c) S–2m2mol

(d) S2m2mol–2.

5. If denotes reduction potential, then which

is true?

(a) E°cell = right – left

(b) E°cell = left + right

(c) E°cell = left – right

(d) E°cell = –( left + right).

6. What will be the emf for the given cell

Pt | H2 (P1) | H+(aq) | | H2 (P2) | Pt

(a) RT/F log P1/P2

(b) RT/2F log P1/P2

(c) RT/F log P2/P1

(d) None of these.

7. Which of the following reaction is possible

at anode?

(a) 2 Cr3+ + 7H2O → Cr2O72– + 14H+

(b) F2 → 2F–

(c) (1/2) O2 + 2H+→ H2O

(d) none of these.

8. The heat required to raise the temperature of

body by 1ºC is called

(a) specific heat

(b) thermal capacity

(c) water equivalent

(d) none of these.

9. When during electrolysis of a solution of

AgNO3, 9650 coulombs of charge pass

through the electroplating bath, the mass of

silver deposited on the cathode will be

(a) 1.08 g

(b) 10.8 g

(c) 21.6 g

(d) 108 g.

LEVEL 2

10. For the redox reaction:

Zn(s) + Cu2+ (0.1 M)Zn+ (1M) + Cu(s)

taking place in a cell, E°cell is 1.10 volt. Ecell

for the cell will be (2.303RT/F = 0.0591)

(a) 2.14 V

(b) 1.80 V

(c) 1.07 V

(d) 0.82 V.

11. For a cell reaction involving a two electron

change, the standard e.m.f. of the cell is found

to be 0.295 V at 25°C. The equilibrium

constant of the reaction at 25°C will be

(a) 1 × 10–10

(b) 29.5 × 10–2

(c) 10

(d) 1 × 1010

Questions – Redox Reaction CEE & JEE Mains Exams

2

12. Standard reduction electrode potentials of

three metals A, B and C are +0.5 V, –3.0 V

and –1.2 V respectively. The reducing power

of these metals are

(a) B > C > A

(b) A > B > C

(c) C > B > A

(d) A > C > B.

13. The standard e.m.f. of a cell, involving one

electron change is found to be 0.591 V at

25°C. The equilibrium constant of the reaction

is (F = 96,500 C mol–1, R = 8.314 JK–1mol–1)

(a) 1.0 × 101

(b) 1.0 × 105

(c) 1.0 × 1010

(d) 1.0 × 1030.

14. The limiting molar conductivities L° for

NaCl, KBrand KCl are 126, 152 and 150 S

cm2mol–1respectively. The ° for NaBr is

(a) 128 S cm2mol–1

(b) 176 S cm2mol–1

(c) 278 S cm2mol–1

(d) 302 S cm2mol–1.

15. In a cell that utilizes the reaction

Zn(s) + 2H+(aq) → Zn2+(aq) + H2(g)

addition of H2SO4 to cathode compartment,

will

(a) lower the E and shift equilibrium to the left

(b) lower theE and shift the equilibrium to the

right

(c) increase the E and shift the equilibrium to

the right

(d) increase the E and shift the equilibrium to

the left.

16. The highest electrical conductivity of the

following aqueous solutions is of

(a) 0.1 M acetic acid

(b) 0.1 M chloroacetic acid

(c) 0.1 M fluoroacetic acid

(d) 0.1 M difluoroacetic acid

17. Aluminium oxide may be electrolysed at

1000°C to furnish aluminium metal (At. Mass

= 27 amu; 1 Faraday = 96,500 Coulombs). The

cathode reaction is

Al3+ + 3e- → Al0

To prepare 5.12 kg of aluminium metal by this

method would require

(a) 5.49 × 107 C of electricity

(b) 1.83 × 107 C of electricity

(c) 5.49 × 104 C of electricity

(d) 5.49 × 1010 C of electricity

18.. Which of the following chemical reactions

depicts the oxidising behaviour of H2SO4?

(a) 2HI + H2SO4 → I2 + SO2 + 2H2O

(b) Ca(OH)2 + H2SO4 → CaSO4 + 2H2O

(c) NaCl + H2SO4 → NaHSO4 + HCl

(d) 2PCl5 + H2SO4 → 2POCl3 + 2HCl +

SO2Cl2.

19. The molar conductivities °NaOAc and

°HCl at infinite dilution in water at 25°C are

91.0 and 426.2 S cm2/mol respectively. To

calculate °HOAc, the additional value required

is

(a) °H2O

(b) °KCl

(c) °NaOH

(d) °NaCl.

20. Resistance of a conductivity cell filled with

a solution of an electrolyte of concentration

0.1 M is 100 W. The conductivity of this

solution is 1.29 Sm–1. Resistance of the same

cell when filled with 0.2 M of the same

solution is 520 W. The molar conductivity of

0.02 M solution of the electrolyte will be

(a) 124 × 10–4 S m2mol–1

(b) 1240 × 10–4 S m2mol–1

(c) 1.24 × 10–4 S m2mol–1

(d) 12.4 × 10–4 S m2mol–1.

21. The equivalent conductances of two strong

electrolytes at infinite dilution in H2O (where

ions move freely through a solution) at 25°C

are given below:

°CH3COONa = 91.0 S cm2/equiv.

°HCl = 426.2 Scm2/equiv.

What additional information/quantity one

needs to calculate ° of an aqueous solution

Questions – Redox Reaction CEE & JEE Mains Exams

3

of acetic acid?

(a) ° of chloroacetic acid (ClCH2COOH)

(b) ° of NaCl

(c) ° of CH3COOK

(d) the limiting equivalent conductance of

H+ ( °H+).

22. Given E°Cr3+/Cr = –0.72 V, E°Fe2+/Fe = –0.42

V. The potential for the cell

Cr | Cr3+(0.1 M) | | Fe2+(0.01 M) | Fe is

(a) –0.26 V

(b) 0.26 V

(c) 0.339 V

(d) –0.339 V

23 Amount of oxalic acid present in a solution

can be determined by its titration with KMnO4

solution in the presence of H2SO4. The

titration gives unsatisfactory result when

carried out in the presence of HCl, because

HCl

(a) oxidises oxalic acid to carbon dioxide and

water

(b) gets oxidised by oxalic acid to chlorine

(c) furnishes H+ ions in addition to those from

oxalic acid

(d) reduces permanganate to Mn2+

Hints & Solutions – Redox Reaction CEE & JEE Mains Exams

1

1. (c) : Ecell = Reduction potential of cathode

(right) – reduction potential of anode (left)=

Eright – Eleft.

2. (c)

3. (d) : The oxidation states show a change

only in reaction (d).

4. (b) : S α A (A = area)

S α C (C = concentration)

Sα 1/ L ( length)

Combining we get,

L

ACKS

Calculating the dimensions we get the desired

solutions.

5. (a) :Ecell = Eright (cathode) – Eleft (anode).

6. (b)

7. (a) : Here Cr3+ is oxidised to Cr2O72–.

8. (b) : It is also known as heat capacity.

9. (b) : The mass of silver deposited on the

cathode=108*9650/96500=10.8 kg

10. (c)1.0

1log

0591.0

ncellEEcell

11. (d) ckn

cellE log0591.0

12. (a) : More is the value of reduction

potential, more is the tendency to get reduced,

i.e. less is the reducing power.

The reducing power follows the following

order: B > C > A

13. (c) ccell kn

cellEE log0591.0

14. (a) 0Nacl= 0

Na+ + 0Cl-

Similarly calculating for KBr&Kcl, and adding

we get the desired solution.

15. (c)

16. (d) : Higher the acidity, higher will be the

tendency to release protons and hence lighter

will be the electrical conductivity.

Difluoroacetic acid will

be strongest acid due to electron withdrawing

effect of two fluorine atoms so as it will show

maximum electrical conductivity.

17. (a) : From Faraday's 1st law,

W = Z × Q [W = weight, Z = electrochemical

equivalent, Q = quantity of electricity]

Now E = Z × F

[E = equivalent weight , F = faraday]

18. (a) : In the reaction,

2 HI + H2S O 4 → I 2 + S O 2 + 2 H 2O

Ist half reaction : 2HI → I

In this reaction oxidation number of I

increases by one, thus this is an oxidation

reaction and HI behaves as a reducing agent.

IInd half reaction : H2SO4 → SO2

In this reaction oxidation number of S

decreases by two, thus this is a reduction

reaction and H2SO4 behaves as oxidising

agent.

19. (d)

20. (a) K=1/R(l/a)

21. (b) : According to Kohlrausch’s law, the

molar

conductivity at infinite dilution ( °) for weak

electrolyte, CH3COOH is

NaclHClCOONACHCOOHCH

33

22. (b)

Hints & Solutions – Redox Reaction CEE & JEE Mains Exams

2

23. (d) : Oxalic acid present in a solution can

be determined by its titration with KMnO4

solutionin the presence of H2SO4.

Titration cannot be done in the presence of

HClbecause KMnO4 being a strong oxidizing

agent oxidises HCl to Cl2 and get itself

reduced to Mn2+.So actual amount of oxalic

acid in solution cannot be determined.