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Electrochemistry Practice Questions - DPP for NEET

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 Page 1


PART-I (Single Correct MCQs)
1. The mathematical expression for law of independent migration of ions
and Ostwald’s dilution law are given by
(a )
(b)
(c)
(d)
2. The equivalent conductance of  solution of a weak monobasic acid
is 8.0 mho cm
2
 and at infinite dilution is 400 mho cm
2
. The dissociation
constant of this acid is: (a) 1.25 × 10
–6
(b) 6.25 × 10
–4
(c) 1.25 × 10
–4
Page 2


PART-I (Single Correct MCQs)
1. The mathematical expression for law of independent migration of ions
and Ostwald’s dilution law are given by
(a )
(b)
(c)
(d)
2. The equivalent conductance of  solution of a weak monobasic acid
is 8.0 mho cm
2
 and at infinite dilution is 400 mho cm
2
. The dissociation
constant of this acid is: (a) 1.25 × 10
–6
(b) 6.25 × 10
–4
(c) 1.25 × 10
–4
(d) 1.25 × 10
–5
3. Molar ionic conductivities of a two-bivalent electrolytes x
2+
 and y
2–
 are
57 and 73 respectively. The molar conductivity of the solution formed
by them will be
(a) 130 S cm
2
 mol
–1
(b) 65 S cm
2
 mol
–1
(c) 260 S cm
2
 mol
–1
(d) 187 S cm
2
 mol
–1
4. If the E°
cell
 for a given reaction has a negative value, then which of the
following gives the correct relationships for the values of ?G° and K
eq
?
(a) ?G° > 0 ; K
eq
 > 1
(b) ?G° < 0 ; K
eq
 > 1
(c) ?G° < 0 ; K
eq
 < 1
(d) ?G° > 0 ; K
eq
 < 1
5. Standard electrode potentials are : Fe
+2
/Fe [ Eº = –0.44]; Fe
+3
/Fe
+2
  Eº =
+ 0.77 ; If Fe
+2
, Fe
+3
 and Fe blocks are kept together, then
(a) Fe
+3
 increases
(b) Fe
+3
 decreases
(c) remains unchanged
(d) Fe
+2
 decreases
6. An electrolytic cell contains a solution of Ag
2
SO
4
 and has platinum
electrodes. A current is passed until 1.6 gm of O
2
 has been liberated at
anode. The amount of silver deposited at cathode would be
(a) 107.88 g
(b) 1.6 g
(c) 0.8 g
(d) 21.60 g
7. For the cell reaction,
Page 3


PART-I (Single Correct MCQs)
1. The mathematical expression for law of independent migration of ions
and Ostwald’s dilution law are given by
(a )
(b)
(c)
(d)
2. The equivalent conductance of  solution of a weak monobasic acid
is 8.0 mho cm
2
 and at infinite dilution is 400 mho cm
2
. The dissociation
constant of this acid is: (a) 1.25 × 10
–6
(b) 6.25 × 10
–4
(c) 1.25 × 10
–4
(d) 1.25 × 10
–5
3. Molar ionic conductivities of a two-bivalent electrolytes x
2+
 and y
2–
 are
57 and 73 respectively. The molar conductivity of the solution formed
by them will be
(a) 130 S cm
2
 mol
–1
(b) 65 S cm
2
 mol
–1
(c) 260 S cm
2
 mol
–1
(d) 187 S cm
2
 mol
–1
4. If the E°
cell
 for a given reaction has a negative value, then which of the
following gives the correct relationships for the values of ?G° and K
eq
?
(a) ?G° > 0 ; K
eq
 > 1
(b) ?G° < 0 ; K
eq
 > 1
(c) ?G° < 0 ; K
eq
 < 1
(d) ?G° > 0 ; K
eq
 < 1
5. Standard electrode potentials are : Fe
+2
/Fe [ Eº = –0.44]; Fe
+3
/Fe
+2
  Eº =
+ 0.77 ; If Fe
+2
, Fe
+3
 and Fe blocks are kept together, then
(a) Fe
+3
 increases
(b) Fe
+3
 decreases
(c) remains unchanged
(d) Fe
+2
 decreases
6. An electrolytic cell contains a solution of Ag
2
SO
4
 and has platinum
electrodes. A current is passed until 1.6 gm of O
2
 has been liberated at
anode. The amount of silver deposited at cathode would be
(a) 107.88 g
(b) 1.6 g
(c) 0.8 g
(d) 21.60 g
7. For the cell reaction,
Cu
2+
 (C
1
, aq) + Zn(s) = Zn
2+
 (C
2
, aq) + Cu(s) of an electrochemical cell,
the change in free energy, ?G, at a given temperature is a function of
(a) ln (C
1
)
(b) ln (C
2
/C
1
)
(c) ln (C
2
)
(d) ln (C
1
 + C
2
)
8. The electrode potential  of a zinc electrode at 25°C with an
aqueous solution of 0.1 M ZnSO
4
 is [ = – 0.76 V. Assume 
 = 0.06 at 298 K].
(a) + 0.73
(b) – 0.79
(c) – 0.82
(d) – 0.70
9. A gas X at 1 atm is bubbled through a solution containing a mixture of
1 M Y
–
 and M Z
–
 at 25 °C. If the reduction potential of Z > Y > X, then,
(a) Y will oxidize X and not Z
(b) Y will oxidize Z and  not X
(c) Y will oxidize both X and Z
(d) Y will reduce both X and Z
10. For the electrochemical cell, 
= 0.44V and 
 
(X/X
–
) = 0.33V .
From this data one can deduce that
(a) M+X?M
+
+X
–
 is the spontaneous reaction
(b) M
+
+X
–
?M+X is the spontaneous reaction
(c) E
cell
 = 0.77 V
(d) E
cell
 = –0.77 V
11. Standard electrode potential data are useful for understanding the
Page 4


PART-I (Single Correct MCQs)
1. The mathematical expression for law of independent migration of ions
and Ostwald’s dilution law are given by
(a )
(b)
(c)
(d)
2. The equivalent conductance of  solution of a weak monobasic acid
is 8.0 mho cm
2
 and at infinite dilution is 400 mho cm
2
. The dissociation
constant of this acid is: (a) 1.25 × 10
–6
(b) 6.25 × 10
–4
(c) 1.25 × 10
–4
(d) 1.25 × 10
–5
3. Molar ionic conductivities of a two-bivalent electrolytes x
2+
 and y
2–
 are
57 and 73 respectively. The molar conductivity of the solution formed
by them will be
(a) 130 S cm
2
 mol
–1
(b) 65 S cm
2
 mol
–1
(c) 260 S cm
2
 mol
–1
(d) 187 S cm
2
 mol
–1
4. If the E°
cell
 for a given reaction has a negative value, then which of the
following gives the correct relationships for the values of ?G° and K
eq
?
(a) ?G° > 0 ; K
eq
 > 1
(b) ?G° < 0 ; K
eq
 > 1
(c) ?G° < 0 ; K
eq
 < 1
(d) ?G° > 0 ; K
eq
 < 1
5. Standard electrode potentials are : Fe
+2
/Fe [ Eº = –0.44]; Fe
+3
/Fe
+2
  Eº =
+ 0.77 ; If Fe
+2
, Fe
+3
 and Fe blocks are kept together, then
(a) Fe
+3
 increases
(b) Fe
+3
 decreases
(c) remains unchanged
(d) Fe
+2
 decreases
6. An electrolytic cell contains a solution of Ag
2
SO
4
 and has platinum
electrodes. A current is passed until 1.6 gm of O
2
 has been liberated at
anode. The amount of silver deposited at cathode would be
(a) 107.88 g
(b) 1.6 g
(c) 0.8 g
(d) 21.60 g
7. For the cell reaction,
Cu
2+
 (C
1
, aq) + Zn(s) = Zn
2+
 (C
2
, aq) + Cu(s) of an electrochemical cell,
the change in free energy, ?G, at a given temperature is a function of
(a) ln (C
1
)
(b) ln (C
2
/C
1
)
(c) ln (C
2
)
(d) ln (C
1
 + C
2
)
8. The electrode potential  of a zinc electrode at 25°C with an
aqueous solution of 0.1 M ZnSO
4
 is [ = – 0.76 V. Assume 
 = 0.06 at 298 K].
(a) + 0.73
(b) – 0.79
(c) – 0.82
(d) – 0.70
9. A gas X at 1 atm is bubbled through a solution containing a mixture of
1 M Y
–
 and M Z
–
 at 25 °C. If the reduction potential of Z > Y > X, then,
(a) Y will oxidize X and not Z
(b) Y will oxidize Z and  not X
(c) Y will oxidize both X and Z
(d) Y will reduce both X and Z
10. For the electrochemical cell, 
= 0.44V and 
 
(X/X
–
) = 0.33V .
From this data one can deduce that
(a) M+X?M
+
+X
–
 is the spontaneous reaction
(b) M
+
+X
–
?M+X is the spontaneous reaction
(c) E
cell
 = 0.77 V
(d) E
cell
 = –0.77 V
11. Standard electrode potential data are useful for understanding the
suitability of an oxidant in a redox titration. Some half cell reactions
and their standard potentials are given below:
  E° = 1.51 V
 E° = 1.38 V
E° = 0.77 V
E° = 1.40 V
Identify the only incorrect statement regarding the quantitative estimation of
aqueous Fe(NO
3
)
2
(a) can be used in aqueous HCl
(b) can be used in aqueous HCl
(c) can be used in aqueous H
2
SO
4
(d) can be used in aqueous H
2
SO
4
? 12. Conductance of 0.1 M KCl (conductivity = X ) filled in a
conductivity cell is Y . If the conductance of 0.1 M NaOH filled
in the same cell is Z , the molar conductance of NaOH will be
(a)
(b)
(c)
(d) 0.1
13. On the basis of the following E° values, the strongest oxidizing agent is
: 
Fe(CN)
6
]
4–
 ?[Fe(CN)
6
]
3–
 + e
– 
; E° = – 0.35 V
Fe
2+
 ? Fe
3+
 + e
–
;                            E° = – 0.77 V
(a) [Fe(CN)
6
]
4–
Page 5


PART-I (Single Correct MCQs)
1. The mathematical expression for law of independent migration of ions
and Ostwald’s dilution law are given by
(a )
(b)
(c)
(d)
2. The equivalent conductance of  solution of a weak monobasic acid
is 8.0 mho cm
2
 and at infinite dilution is 400 mho cm
2
. The dissociation
constant of this acid is: (a) 1.25 × 10
–6
(b) 6.25 × 10
–4
(c) 1.25 × 10
–4
(d) 1.25 × 10
–5
3. Molar ionic conductivities of a two-bivalent electrolytes x
2+
 and y
2–
 are
57 and 73 respectively. The molar conductivity of the solution formed
by them will be
(a) 130 S cm
2
 mol
–1
(b) 65 S cm
2
 mol
–1
(c) 260 S cm
2
 mol
–1
(d) 187 S cm
2
 mol
–1
4. If the E°
cell
 for a given reaction has a negative value, then which of the
following gives the correct relationships for the values of ?G° and K
eq
?
(a) ?G° > 0 ; K
eq
 > 1
(b) ?G° < 0 ; K
eq
 > 1
(c) ?G° < 0 ; K
eq
 < 1
(d) ?G° > 0 ; K
eq
 < 1
5. Standard electrode potentials are : Fe
+2
/Fe [ Eº = –0.44]; Fe
+3
/Fe
+2
  Eº =
+ 0.77 ; If Fe
+2
, Fe
+3
 and Fe blocks are kept together, then
(a) Fe
+3
 increases
(b) Fe
+3
 decreases
(c) remains unchanged
(d) Fe
+2
 decreases
6. An electrolytic cell contains a solution of Ag
2
SO
4
 and has platinum
electrodes. A current is passed until 1.6 gm of O
2
 has been liberated at
anode. The amount of silver deposited at cathode would be
(a) 107.88 g
(b) 1.6 g
(c) 0.8 g
(d) 21.60 g
7. For the cell reaction,
Cu
2+
 (C
1
, aq) + Zn(s) = Zn
2+
 (C
2
, aq) + Cu(s) of an electrochemical cell,
the change in free energy, ?G, at a given temperature is a function of
(a) ln (C
1
)
(b) ln (C
2
/C
1
)
(c) ln (C
2
)
(d) ln (C
1
 + C
2
)
8. The electrode potential  of a zinc electrode at 25°C with an
aqueous solution of 0.1 M ZnSO
4
 is [ = – 0.76 V. Assume 
 = 0.06 at 298 K].
(a) + 0.73
(b) – 0.79
(c) – 0.82
(d) – 0.70
9. A gas X at 1 atm is bubbled through a solution containing a mixture of
1 M Y
–
 and M Z
–
 at 25 °C. If the reduction potential of Z > Y > X, then,
(a) Y will oxidize X and not Z
(b) Y will oxidize Z and  not X
(c) Y will oxidize both X and Z
(d) Y will reduce both X and Z
10. For the electrochemical cell, 
= 0.44V and 
 
(X/X
–
) = 0.33V .
From this data one can deduce that
(a) M+X?M
+
+X
–
 is the spontaneous reaction
(b) M
+
+X
–
?M+X is the spontaneous reaction
(c) E
cell
 = 0.77 V
(d) E
cell
 = –0.77 V
11. Standard electrode potential data are useful for understanding the
suitability of an oxidant in a redox titration. Some half cell reactions
and their standard potentials are given below:
  E° = 1.51 V
 E° = 1.38 V
E° = 0.77 V
E° = 1.40 V
Identify the only incorrect statement regarding the quantitative estimation of
aqueous Fe(NO
3
)
2
(a) can be used in aqueous HCl
(b) can be used in aqueous HCl
(c) can be used in aqueous H
2
SO
4
(d) can be used in aqueous H
2
SO
4
? 12. Conductance of 0.1 M KCl (conductivity = X ) filled in a
conductivity cell is Y . If the conductance of 0.1 M NaOH filled
in the same cell is Z , the molar conductance of NaOH will be
(a)
(b)
(c)
(d) 0.1
13. On the basis of the following E° values, the strongest oxidizing agent is
: 
Fe(CN)
6
]
4–
 ?[Fe(CN)
6
]
3–
 + e
– 
; E° = – 0.35 V
Fe
2+
 ? Fe
3+
 + e
–
;                            E° = – 0.77 V
(a) [Fe(CN)
6
]
4–
(b) Fe
2+
(c) Fe
3+
(d) [Fe(CN)
6
]
3–
14. The variation of molar conductance of strong electrolyte with
(concentration)
½
 is represented by
(a)
(b)
(c)
(d)
15. A device that converts energy of combustion of fuels like hydrogen and
methane, directly into electrical energy is known as :
(a) Electrolytic cell
(b) Dynamo
(c) Ni-Cd cell
(d) Fuel cell
16. In acidic medium  is an oxidant as
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FAQs on Electrochemistry Practice Questions - DPP for NEET

1. What is electrochemistry?
Ans. Electrochemistry is the branch of chemistry that deals with the relationship between electricity and chemical reactions. It involves the study of how chemical reactions can produce or consume electrical energy.
2. What are the applications of electrochemistry?
Ans. Electrochemistry has various applications in our everyday lives. Some of the common applications include electroplating, batteries, corrosion prevention, electrolysis, fuel cells, and sensors.
3. What is the difference between anode and cathode in electrochemistry?
Ans. In electrochemistry, the anode is the electrode where oxidation occurs, meaning it loses electrons. On the other hand, the cathode is the electrode where reduction occurs, meaning it gains electrons. In simple terms, the anode is the positive electrode, while the cathode is the negative electrode.
4. What is electrolysis?
Ans. Electrolysis is a process that uses an electric current to drive a non-spontaneous chemical reaction. It involves the decomposition of a compound into its constituent elements or ions using electricity.
5. How does a battery work in electrochemistry?
Ans. A battery works by utilizing an electrochemical reaction to generate a flow of electrons. The chemical reaction inside the battery produces a potential difference between the positive and negative terminals, allowing the electrons to flow through an external circuit, creating an electric current.
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