CHEMISTRY
(Q&A Bank for CEE & JEE Mains)
Assam Electronics Development Corporation Limited
(AMTRON) (A Government of Assam Undertaking)
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.