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self evaluation test on ELECTROCHEMISTRY with answers., Exercises of Electrochemistry

It contains objective and assertion- reason type questions with detailed solutions.

Typology: Exercises

2021/2022

Available from 05/24/2022

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Electrochemistry 539
1. The mass of copper deposited from a solution of
4
CuSO
by passage of 5 A current for 965 second is
(Mol. wt. of Copper = 63.5) [AIIMS 2001]
(a) 15.875 g (b) 1.5875 g
(c) 4825 g (d) 96500 g
2. The current in a given wire is 1.8 A. The number
of coulombs that flow in 1.36 minutes will be [AIIMS 2001]
(a) 100 C (b) 147 C
(c) 247 C (d) 347 C
3. A solution of a salt of a metal was electrolysed
for 150 minutes with a current of 0.15 ampere s.
The weight of metal deposited was 0.783 gm.
The equivalent wei ght of the metal is [AFMC 2001]
(a) 55.97 gm (b) 65.97 gm
(c) 75.97 gm (d) 85.97 gm
4. The resistance of 0.01N
NaCl
solution at
C
o
25
is
200 . Cell constant of conductivity cell is 1 cm1.
The equivalent conductance is [CBSE PMT 1999]
(a)
1212
105
eqcm
(b)
1213
106
eqcm
(c)
1214
107
eqcm
(d)
1215
108
eqcm
5. Which of the following reaction is possible at
anode
[AIEEE 2002]
(a)
HOCrOHCr 1472 2
722
3
(b)
FF 2
2
(c)
(d) None of these
6. What is the standard cell potential for the cell
CuMCuMZnZn /)1(||)1(/ 22
o
E
for
VCuCuVMZnZn 34.0/&76.0)1(/ 22
[AIIMS 1980]
(a)
V42.0)34.0(76.0
(b)
V42.076.034.0
(c)
V10.1)76.0(34.0
(d)
V10.1)34.0(76.0
7. Normal aluminium electrode coupled with normal
hydrogen electrode gives an
emf
of
volts66.1
. So
the standard electrode potential of aluminium is[KCET 1987]
(a) 1.66 V (b) + 1.66 V
(c) 0.83 V (d) + 0.83 V
8. Which one among the following is the strongest
reducing agent
)44.0(2
2VFeeFe
)25.0(2
2VNieNi
)14.0(2
2VSneSn
)77.0(
23 VFeeFe
[BHU 1998]
(a)
Fe
(b)
2
Fe
(c)
Ni
(d)
Sn
9. The cell reaction of the galvanic cell
)(
)(
2
)(
2
)( ||||l
aqaq
sHgHgCuCu
is [EAMCET 2003]
(a)
CuHgCuHg 22
(b)
HgCuCuHg 2
(c)
CuHgHgCu
(d)
HgCuHgCu 22
10. The specific conductivity of N/10
KCl
solution at
C
o
20
is
11
0212.0 cmohm
and the resistance of
cell containing this solution at
C
o
20
is 55 ohm.
The cell constant is
[AIIMS 1999]
(a) 1.166
1
cm
(b) 2.173
1
cm
(c) 3.324
1
cm
(d) 4.616
1
cm
11. The oxide which is not reduced by hydrogen is
pf2

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Electrochemistry 539

1. The mass of copper deposited from a solution of

4

CuSO

by passage of 5 A current for 965 second is

( Mol. wt. of Copper = 63.5) [AIIMS 2001]

(a) 15.875 g (b) 1.5875 g

(c) 4825 g (d) 96500 g

2. The current in a given wire is 1.8 A. The number

of coulombs that flow in 1.36 minutes will be [AIIMS 2001]

(a) 100 C (b) 147 C

(c) 247 C (d) 347 C

3. A solution of a salt of a metal was electrolysed

for 150 minutes with a current of 0.15 amperes.

The weight of metal deposited was 0.783 gm.

The equivalent weight of the metal is [AFMC 2001]

(a) 55.97 gm (b) 65.97 gm

(c) 75.97 gm (d) 85.97 gm

4. The resistance of 0.01 N NaCl solution at C

o

25 is

200 . Cell constant of conductivity cell is 1 cm

  • 1

The equivalent conductance is [CBSE PMT 1999]

(a)

2 1 2 1

 

  cmeq (b)

3 1 2 1

 

  cmeq

(c)

4 1 2 1

 

  cmeq (d)

5 1 2 1

 

  cmeq

5. Which of the following reaction is possible at

anode

[AIEEE 2002]

(a)

  

2 Cr  7 HOCrO  14 H

2

2 2 7

3

(b)

F  2 F

2

(c) O H HO

2 2

2

2

1

 

(d) None of these

6. What is the standard cell potential for the cell

Zn / Zn ( 1 M )|| Cu ( 1 M )/ Cu

2  2 

o

E for Zn / Zn ( 1 M ) 0. 76 V & Cu / Cu 0. 34 V

2 2

  

 

[AIIMS 1980]

(a)  0. 76 ( 0. 34 ) 0. 42 V

(b) 0. 34  0. 76  0. 42 V

(c)

  1. 34 ( 0. 76 ) 1. 10 V

(d) 0. 76 ( 0. 34 ) 1. 10 V

7. Normal aluminium electrode coupled with normal

hydrogen electrode gives an emf of 1. 66 volts. So

the standard electrode potential of aluminium is [KCET 1987]

(a) – 1.66 V (b) + 1.66 V

(c) – 0.83 V (d) + 0.83 V

8. Which one among the following is the strongest

reducing agent

2 ( 0. 44 )

2

FeeFeV

 

2 ( 0. 25 )

2

NieNiV

 

2

SneSnV

 

( 0. 77 )

3 2

FeeFeV

  

[BHU 1998]

(a) Fe (b)

2 

Fe

(c) Ni (d) Sn

9. The cell reaction of the galvanic cell

()

( )

2

( )

2

( )

l

aq aq s

Cu Cu Hg Hg

 

is [EAMCET 2003]

(a) HgCuHgCu

2  2 

(b)

  

HgCuCuHg

2

(c) CuHgCuHg

(d) CuHgCuHg

2  2 

10. The specific conductivity of N /10 KCl solution at

C

o

20 is

1 1

  1. 0212

 

ohm cm and the resistance of

cell containing this solution at C

o

20 is 55 ohm.

The cell constant is

[AIIMS 1999]

(a) 1.

 1

cm

(b) 2.

 1

cm

(c) 3.

 1

cm

(d) 4.

 1

cm

11. The oxide which is not reduced by hydrogen is

538 Electrochemistry

[JIPMER 1999]

(a) Ag O

2

(b) KO

2

(c)

2 3

FeO (d)

4 10

PO

1. (b) Current (I) = 5A and time (t) = 965 sec.

We know that equivalent weight of copper

Valancy

Molecular weight

  and quantity of

electricity passed in coulomb = current × time

= 5 × 965 = 4825 C. Since 96500 coulombs will

deposit g

2

  1. 5

of copper therefore 4825

coulombs will deposit

= 1. 5875 g

96500 2

  1. 5 4825

2. (b) QIt ; 1. 8  1. 36  60  147 C. 3. (a) Time (t) = 150 min = 9000 sec

Current (I) = 0.15 A

Weight of metal (w) = 0.783 g.

We know QIt= 0. 15  9000  1350 C. Since

1350 C of electricity will deposited 0.783 g of

metal, so, 96500 C of electricity will

deposited 55. 97 g

1350

  1. 783 96500

4. (a) 1 10 , 000

200

1 1

     V   

a

l

R

k V

2 1 2 1

 

   cmeq

5. (a) Oxidation always occurs at anode. 6. (c)

cathode anode

E E E

o

 

o

E ; E volt

o

7. (a)

o

Al Al

o

H H

o

E E E

/ /

cell

3

2

  1. 66  

  

o

Al Al

O E

/

3 

  or

E V

Al Al

  1. 66

/

3



8. (a) The reduction potential of Fe is very high, so

it is a strongest reducing agent.

9. (b)

cathodereduction

()

2

( )

anodeoxidation

2

( ) ( )

s Ag Ag l

Cu Cu Hg Hg

 

CuHgCuHg

2  2 

10. (a)  

R

K

1

cell constant

1

  1. 0212 55 1. 166

KR    cm.

11. (b) On the basis of electrochemical series KO

2

is

not reduced by hydrogen.

Oxidation

Reduction

(SET - 12)