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It contains objective and assertion- reason type questions with detailed solutions.
Typology: Exercises
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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
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 HO CrO 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)
(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
Fe e Fe V
2 ( 0. 25 )
2
Ni e Ni V
2
Sn e Sn V
( 0. 77 )
3 2
Fe e Fe V
[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) Hg Cu Hg Cu
2 2
(b)
Hg Cu Cu Hg
2
(c) Cu Hg CuHg
(d) Cu Hg Cu Hg
2 2
10. The specific conductivity of N /10 KCl solution at
C
o
20 is
1 1
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
[JIPMER 1999]
(a) Ag O
2
(b) KO
2
(c)
2 3
FeO (d)
4 10
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
of copper therefore 4825
coulombs will deposit
= 1. 5875 g
96500 2
2. (b) Q I t ; 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 Q I t= 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
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
o
Al Al
O E
/
3
or
E V
Al Al
/
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
Cu Hg Cu Hg
2 2
10. (a)
R
K
1
cell constant
1
K R cm.
11. (b) On the basis of electrochemical series KO
2
is
not reduced by hydrogen.
Oxidation
Reduction