Q.1
For measuring the conductivity of an electrolyte, its solution should be prepared is [ Bihar CEE 1990]
  • a) tap water
  • b) distilled water
  • c) conductivity water
  • d) polywater
Q.2
In an electroplating experiment m gm silver is deposited when 4 amp current flows for 2 minutes. The amount (in gram) of silver deposited by 6ampof current flowing for 40sec will be [ MLNR 1991]
  • a) 4m
  • b) m/2
  • c) 2m
  • d) m/4
Q.3
One faraday is equal to ..[ AFMC 1989]
  • a)69500 coulombs
  • b) 99500 coulombs
  • c)96500 coulombs approximately
  • d)none of the above
Q.4
NaOH is manufactured by the electrolysis of brine solution. the products of the reaction are ..[ KCET 1990]
  • a) Cl2 and H2
  • b) Cl2 and Na-Hg
  • c)Cl2 and Na
  • d)Cl2 and O2
Q.5
A current of strength 2.5 amp was passed through CuSO4 solution for 6 minutes 26 seconds. the amount of copper deposited is ( At. Wt of Cu=63.5) [ EAMCET 1989]
  • a) 0.3175 g
  • b) 3.175g
  • c)0.635 g
  • d)6.35g
Q.6
The amount of charge that must be passed through a solution containing Cu2+ in order to deposited 1gm atom of copper (65.5) is .. [ EAMCET 1991]
  • a) 1520 Coulomb
  • b) 3040 coulomb
  • c) 96500 coulomb
  • d) 193000 coulomb
Q.7
2H+(aq) + 2e- → H2(g) Standard electrode potential for the above reaction ( in volts ) is [ CPMT 1988]
  • a)0
  • b) +1
  • c)-1
  • d)None of these
Q.8
The amount of electricity required to deposit 1 mole of aluminum from a solution of AlCl3 would be ..[ haryana CEET 1991]
  • a) 0.33 Faraday
  • b) 1 Faraday
  • c)3 Faraday
  • d)1 Ampere
Q.9
Select the strongest reducing agent from amongst the substances involved in the following half-reactions.Cl2(g) + e- → 2Cl-(aq) +1.36 VBr2+e- → 2Br- (aq) +1.09VSn2+ +2e- → Sn -0.14V[Pb. CET 1989]
  • a) Cl-
  • b) Br-
  • c)Sn
  • d)Sn2+
Q.10
The electrochemical equivalent of silver is 0.001118 g. When an electric current of 0.5 ampere is passed through an aqueous solver nitrate solution for 200 seconds, the amount of silver deposited is [ BHU 1987]
  • a) 1.118 g
  • b) 0.1118 g
  • c) 5.590 g
  • d) 0.5590 g
Q.11
The cathodic reaction in electrolysis of dilute H2SO4 with platinum electrodes is [ MLNR 1988]
  • a)Oxidation
  • b) reduction
  • c)Both
  • d)Neutralization
Q.12
When an electric current is passed through acidulated water, 112 ml of hydrogen gas at NTP is collected at the cathode in 965 second. the current passed in amperes is ..[ MLNR 1991]
  • a) 1.0
  • b)0.5
  • c)0.1
  • d)2.0
Q.13
Given electrode potentials: Ag+/Ag=0.80V, Co2+/Co=0.28VCu2+/Cu=0.34V, Zn2+/Zn=-0.76VThe most reactive metal which displaces other metals from their salts in solution is [ Pb. CET 1990]
  • a) Ag
  • b) Cu
  • c)Co
  • d)Zn
Q.14
How many coulombs of electricity are consumed when 100 mA current is passed through a solution of AgNO3 for half an hour during an electrolysis experiment? [ Pb CET 1989]
  • a) 108
  • b) 180
  • c) 1800
  • d) 18000
Q.15
The most powerful reducing agent is[ MLNR 1989]
  • a)Mg
  • b) K
  • c)Na
  • d)Ba
Q.16
The electrolytic sells, one containing acidified ferrous chloride and another acidified ferric chloride are connected in series. the ratio of iron deposited at cathodes in the two cells when electricity is passed through the cell will be [ CPMT 1989]
  • a) 3:1
  • b) 2:1
  • c)1:1
  • d)3:2
Q.17
Three faraday electricity was passed through an aqueous solution of iron(II) bromide. the weight of iron metal (At wt=56) deposited at the cathode ( in gm) is [ EAMCET 1991]
  • a) 56
  • b) 84
  • c)112
  • d)168
Q.18
Of the following metals that cannot be obtained by electrolysis of the aqueous solution of their salts are [ IIT 1990]
  • a) Ag and Mg
  • b) Ag and Al
  • c) Mg and Al
  • d) Cu and Cr
Q.19
Electrolytic cell is used to convert .. [ AFMC 1989]
  • a)chemical energy to electrical energy
  • b) electrical energy to chemical energy
  • c)chemical energy to mechanical energy
  • d)electrical energy to mechanical energy
Q.20
The charge required to liberate 11.5 g sodium from fused sodium chloride is [ AIIMS 1992]
  • a) 0.5 faraday
  • b) 1.0 faraday
  • c)1.5 faraday
  • d)96500 coulomb
Q.21
K, Ca and Li metals may be arranged in the decreasing order of their standard electrode potential as [ CPMT 1990]
  • a) K, Ca, Li
  • b) Li, K, Ca
  • c)Li, Ca, K
  • d)Ca, K, Li
Q.22
Electrolysis of molten NaCl leads to the formation of [ KCET 1990]
  • a) Sodium and Hydrogen
  • b) Sodium and Oxygen
  • c) Hydrogen and Oxygen
  • d) Sodium and Chlorine
Q.23
On the basis of position in the electrochemical series, the metal which does not displace hydrogen from water and acid is [ MP PMT 1988]
  • a)Hg
  • b) Al
  • c)Pb
  • d)Ba
Q.24
A certain current deposit 0.50 of hydrogen in 2 hrs. The amount of copper liberated from a solution of copper sulphate by the same current flowing for the same time would be.. [ CPMT 1991]
  • a) 31.8 g
  • b) 63.6 g
  • c)15.9 g
  • d)6.36g
Q.25
The emf of the following three galvanic cells I) Zn|Zn2+(1M)|| Cu2+(1M)|CuII) Zn|Zn2+(0.1M)|| Cu2+(1M)|CuIII) Zn|Zn2+(1m)|| Cu2+(0.1M)|Cu are represented by E1, E2, EWhich of the following statement is true? [ Pb CET 1990]
  • a) E1 > E2 > E3
  • b)E3 > E2 > E1
  • c)E3 > E1 > E2
  • d) E1 > E3 > E2
Q.26
The quantity of electricity needed to liberated 0.5 gram equivalent of an element is [ CPMT 1988]
  • a) 48250 faraday
  • b) 48250 coulomb
  • c) 19300 faraday
  • d) 19300 coulomb
Q.27
Eo value of Mg2+/Mg is -2.37V of Zn2+/Zn is -0.76V and Fe2+/Fe is -0.44V. Which of the following statement is correct? [ EAMCET 1989]
  • a)Zn will reduce Fe2+
  • b) Zn will reduce Mg2+
  • c)Mg oxidises Fe
  • d)Zn oxidizes Fe
Q.28
When 9650 coulombs of electricity is passed through a solution of copper sulphate, the amount of copper deposited is [ At Wt of Cu=63.6) [ Pb CET 1990]
  • a) 0.318 g
  • b) 3.18 g
  • c)31.8g
  • d)63.6 g
Q.29
During electrolysis of NaCl solution, the gas liberated at the anode is [ Pb CET 1990]
  • a) H2
  • b) O2
  • c)Cl2
  • d)None of these
Q.30
To deposited 0.6354 g of copper by electrolysis of aqueous cupric sulphate solution
  • a) 9650
  • b) 4825
  • c) 3860
  • d) 1930
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