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question_answer1)
Water cannot be made conducting by adding small amount of any of the following except
A)
Sodium chloride done
clear
B)
Copper sulphate done
clear
C)
Ammonium chloride done
clear
D)
Sugar done
clear
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question_answer2)
The electrochemical equivalent Z of any element can be obtained by multiplying the electrochemical equivalent of hydrogen with
A)
Atomic weight done
clear
B)
Molecular weight done
clear
C)
Chemical equivalent done
clear
D)
A constant done
clear
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question_answer3)
A silver and zinc voltameter are connected in series and a current i is passed through them for a time t liberating W gm of zinc. The weight of silver deposited is nearly [NCERT 1973, 76]
A)
W done
clear
B)
1.7 W done
clear
C)
2.4 W done
clear
D)
3.5 W done
clear
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question_answer4)
To deposit one gm equivalent of an element at an electrode, the quantity of electricity needed is [IIT 1984; DPMT 1982; MP PET 1998; MP PMT 1998; 2003]
A)
One ampere done
clear
B)
96000 amperes done
clear
C)
96500 farads done
clear
D)
96500 coulombs done
clear
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question_answer5)
In an electrolysis experiment, a current i passes through two different cells in series, one containing a solution of \[CuS{{O}_{4}}\] and the other a solution of\[AgN{{O}_{3}}\]. The rate of increase of the weight of the cathodes in the two cells will be [NCERT 1972]
A)
In the ratio of the densities of Cu and Ag done
clear
B)
In the ratio of the at weights of Cu and Ag done
clear
C)
In the ratio of half the atomic weight of Cu to the atomic weight of Ag done
clear
D)
In the ratio of half the atomic weight of Cu to half the atomic weight of Ag done
clear
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question_answer6)
To deposit one litre of hydrogen at 22.4 atmosphere from acidulaled water, the quantity of electricity that must pass through is [BVP 2003]
A)
1 coulomb done
clear
B)
22.4 coulomb done
clear
C)
96500 coulomb done
clear
D)
193000 coulomb done
clear
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question_answer7)
The amount of substance liberated on electrodes during electrolysis when 1 coulomb of electricity is passed, is
A)
Chemical equivalent done
clear
B)
Electrochemical equivalent done
clear
C)
Equivalent weight done
clear
D)
One mol done
clear
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question_answer8)
For goldplating on a copper chain, the substance required in the form of solution is
A)
Copper sulphate done
clear
B)
Copper chloride done
clear
C)
Potassium cyanide done
clear
D)
Potassium aurocyanide done
clear
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question_answer9)
On passing the current in water voltameter, the hydrogen
A)
Liberated at anode done
clear
B)
Liberated at cathode done
clear
C)
Does not liberate done
clear
D)
Remains in the solution done
clear
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question_answer10)
In water voltameter, the electrolysis of ...... takes place [DPMT 1999]
A)
\[{{H}_{2}}O\] done
clear
B)
\[{{H}_{2}}S{{O}_{4}}\] done
clear
C)
\[{{H}_{2}}O\] and \[{{H}_{2}}S{{O}_{4}}\] both done
clear
D)
\[{{H}_{2}}\] and \[{{O}_{2}}\] done
clear
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question_answer11)
For depositing 1 gm of Cu in copper voltameter on passing 2 amperes of current, the time required will be (For copper Z = 0.00033 gm/C)
A)
Approx. 20 minutes done
clear
B)
Approx. 25 minutes done
clear
C)
Approx. 30 minutes done
clear
D)
Approx. 35 minutes done
clear
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question_answer12)
A battery of e.m.f. 3 volt and internal resistance 1.0 ohm is connected in series with copper voltameter. The current flowing in the circuit is 1.5 amperes. The resistance of voltameter will be
A)
Zero done
clear
B)
1.0 ohm done
clear
C)
1.5 ohm done
clear
D)
2.0 ohm done
clear
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question_answer13)
According to Faraday's laws of electrolysis, the amount of decomposition is proportional to [MP PMT 1993]
A)
\[\frac{1}{\text{Time for which curent passes}}\] done
clear
B)
Electrochemical equivalent of the substance done
clear
C)
\[\frac{1}{\text{Current}}\] done
clear
D)
\[\frac{1}{\text{Electrochemical equivalent}}\] done
clear
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question_answer14)
If in a voltaic cell 5 gm of zinc is consumed, then we get how many ampere hours ? (Given that E.C.E. of Zn is \[3.387\times {{10}^{-7}}\] kg/coulomb)
A)
2.05 done
clear
B)
8.2 done
clear
C)
4.1 done
clear
D)
\[5\times 3.387\times {{10}^{-7}}\] done
clear
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question_answer15)
The current flowing in a copper voltameter is 1.6 A. The number of \[C{{u}^{++}}\] ions deposited at the cathode per minute are [MP PMT 1994; MP PET 2000]
A)
\[1.5\times {{10}^{20}}\] done
clear
B)
\[3\times {{10}^{20}}\] done
clear
C)
\[6\times {{10}^{20}}\] done
clear
D)
\[1\times {{10}^{19}}\] done
clear
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question_answer16)
In a copper voltameter experiment, current is decreased to one-fourth of the initial value but it is passed for four times the earlier duration. Amount of copper deposited will be [MP PMT 1993]
A)
Same done
clear
B)
One-fourth the previous value done
clear
C)
Four times the previous value done
clear
D)
\[\frac{1}{16}th\] of the previous value done
clear
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question_answer17)
A certain charge liberates 0.8 gm of\[{{O}_{2}}\]. The same charge will liberate how many gm of silver [MP PET 1999]
A)
108 gm done
clear
B)
10.8 gm done
clear
C)
0.8 gm done
clear
D)
\[\frac{108}{0.8}gm\] done
clear
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question_answer18)
In charging a battery of motor-car, the following effect of electric current is used [MP PET 1993; AFMC 2003]
A)
Magnetic done
clear
B)
Heating done
clear
C)
Chemical done
clear
D)
Induction done
clear
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question_answer19)
The Avogadro's number is \[6\times {{10}^{23}}\] per gm mole and electronic charge is \[1.6\times {{10}^{-19}}C\]. The Faraday's number is [DPMT 2001]
A)
\[6\times {{10}^{23}}\times 1.6\times {{10}^{-19}}\] done
clear
B)
\[\frac{6\times {{10}^{23}}}{1.6\times {{10}^{-19}}}\] done
clear
C)
\[\frac{2}{6\times {{10}^{23}}\times 1.6\times {{10}^{-19}}}\] done
clear
D)
\[\frac{1.6\times {{10}^{-19}}}{6\times {{10}^{23}}}\] done
clear
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question_answer20)
In \[CuS{{O}_{4}}\] solution when electric current equal to 2.5 faraday is passed, the gm equivalent deposited on the cathode is
A)
1 done
clear
B)
1.5 done
clear
C)
2 done
clear
D)
2.5 done
clear
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question_answer21)
The atomic weight of silver and copper are 108 and 64. A silver voltameter and a copper voltameter are connected in series and when current is passed 10.8 gm of silver is deposited. The mass of copper deposited will be
A)
6.4 gm done
clear
B)
12.8 gm done
clear
C)
3.2 gm done
clear
D)
10.8 gm done
clear
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question_answer22)
Faraday's laws of electrolysis are related to [IIT 1983]
A)
The atomic number of positive ion done
clear
B)
The equivalent weight of electrolyte done
clear
C)
The atomic number of negative ion done
clear
D)
The velocity of positive ion done
clear
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question_answer23)
In the process of electrolysis, the current is carried out inside the electrolyte by [AMU (Engg.) 1999]
A)
Electrons done
clear
B)
Atoms done
clear
C)
Positive and negative ions done
clear
D)
All the above done
clear
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question_answer24)
The mass of ions deposited during a given interval of time in the process of electrolysis depends on [DPMT 2002]
A)
The current done
clear
B)
The resistance done
clear
C)
The temperature done
clear
D)
The electric power done
clear
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question_answer25)
The amount of charge required to liberate 9 gm of aluminium (atomic weight = 27 and valency = 3) in the process of electrolysis is (Faraday's number = 96500 coulombs/gm equivalent)
A)
321660 coulombs done
clear
B)
69500 coulombs done
clear
C)
289500 coulombs done
clear
D)
96500 coulombs done
clear
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question_answer26)
In an electroplating experiment, m gm of silver is deposited when 4 ampere of current flows for 2 minute. The amount (in gm) of silver deposited by 6 ampere of current for 40 second will be [MNR 1991; UPSEAT 2000; MP PET 2002; Pb. PET 2004; Orissa JEE 2005]
A)
4 m done
clear
B)
\[m/2\] done
clear
C)
\[m/4\] done
clear
D)
2 m done
clear
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question_answer27)
In electrolysis, if the duration of the passage of current is doubled, the mass liberated is [EAMCET 1979]
A)
Doubled done
clear
B)
Halved done
clear
C)
Increased four times done
clear
D)
Remains the same done
clear
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question_answer28)
A current of 16 ampere flows through molten NaCl for 10 minute. The amount of metallic sodium that appears at the negative electrode would be [EAMCET 1984]
A)
0.23 gm done
clear
B)
1.15 gm done
clear
C)
2.3 gm done
clear
D)
11.5 gm done
clear
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question_answer29)
The mass of a substance liberated when a charge ?q? flows through an electrolyte is proportional to [EAMCET 1984]
A)
q done
clear
B)
\[1/q\] done
clear
C)
\[{{q}^{2}}\] done
clear
D)
\[1/{{q}^{2}}\] done
clear
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question_answer30)
A steady current of 5 amps is maintained for 45 mins. During this time it deposits 4.572 gms of zinc at the cathode of a voltameter. E.C.E. of zinc is [MP PET 1994]
A)
\[3.387\times {{10}^{-4}}gm/C\] done
clear
B)
\[3.387\times {{10}^{-4}}C/gm\] done
clear
C)
\[3.384\times {{10}^{-3}}gm/C\] done
clear
D)
\[3.394\times {{10}^{-3}}C/gm\] done
clear
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question_answer31)
The relation between faraday constant F, electron charge e and avogadro number N is [MP PET 1995]
A)
\[F=N/e\] done
clear
B)
\[F=Ne\] done
clear
C)
\[N={{F}^{2}}\] done
clear
D)
\[F={{N}^{2}}e\] done
clear
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question_answer32)
The electrochemical equivalent of magnesium is \[0.126\,mg/C\]. A current of 5 A is passed in a suitable solution for 1 hour. The mass of magnesium deposited will be [MP PMT 1995]
A)
0.0378 gm done
clear
B)
0.227 gm done
clear
C)
0.378 gm done
clear
D)
2.27 gm done
clear
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question_answer33)
Two electrolytic cells containing \[CuS{{O}_{4}}\] and \[AgN{{O}_{3}}\] respectively are connected in series and a current is passed through them until 1 mg of copper is deposited in the first cell. The amount of silver deposited in the second cell during this time is approximately [Atomic weights of copper and silver are respectively 63.57 and 107.88] [MP PMT 1996]
A)
1.7 mg done
clear
B)
3.4 mg done
clear
C)
5.1 mg done
clear
D)
6.8 mg done
clear
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question_answer34)
A current I is passed for a time t through a number of voltameters. If m is the mass of a substance deposited on an electrode and z is its electrochemical equivalent, then [MP PMT 1997]
A)
\[\frac{zIt}{m}=\text{constant}\] done
clear
B)
\[\frac{z}{mIt}=\text{constant}\] done
clear
C)
\[\frac{I}{zmt}=\text{constant}\] done
clear
D)
\[\frac{It}{zm}=\text{constant}\] done
clear
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question_answer35)
For electroplating a spoon, it is placed in the voltameter at [MP PMT/PET 1998]
A)
The position of anode done
clear
B)
The position of cathode done
clear
C)
Exactly in the middle of anode and the cathode done
clear
D)
Anywhere in the electrolyte done
clear
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question_answer36)
If nearly \[{{10}^{5}}\]coulomb liberate 1 gm equivalent of aluminium, then the amount of aluminium (equivalent weight 9) deposited through electrolysis in 20 minutes by a current of 50 amp will be [CBSE PMT 1998]
A)
0.6 gm done
clear
B)
0.09 gm done
clear
C)
5.4 gm done
clear
D)
10.8 gm done
clear
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question_answer37)
Electroplating does not help in [AIIMS 1998]
A)
Fine finish to the surface done
clear
B)
Shining appearance done
clear
C)
Metals to become hard done
clear
D)
Protect metal against corrosion done
clear
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question_answer38)
When a current is passed through water, acidified with a dilute sulphuric acid, the gases formed at the platinum electrodes are [KCET 1994]
A)
1 vol. hydrogen (cathode) and 2 vol. oxygen (anode) done
clear
B)
2 vol. hydrogen (cathode) and 1 vol. oxygen (anode) done
clear
C)
1 vol. hydrogen (cathode) and 1 vol. oxygen (anode) done
clear
D)
1 vol. oxygen (cathode) and 2 vol. hydrogen (anode) done
clear
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question_answer39)
The negative Zn pole of a Daniel cell, sending a constant current through a circuit, decreases in mass by 0.13g in 30 minutes. If the electrochemical equivalent of Zn and Cu are 32.5 and 31.5 respectively, the increase in the mass of the positive Cu pole in this time is [AIEEE 2003]
A)
0.242 g done
clear
B)
0.190 g done
clear
C)
0.141 g done
clear
D)
0.126 g done
clear
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question_answer40)
When a copper voltameter is connected with a battery of e.m.f. 12 volts. 2 gms of copper is deposited in 30 minutes. If the same voltameter is connected across a 6 volt battery, then the mass of copper deposited in 45 minutes would be [SCRA 1994]
A)
1 gm done
clear
B)
1.5 gm done
clear
C)
2 gm done
clear
D)
2.5 gm done
clear
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question_answer41)
The value of current required to deposit 0.972 gm of chromium in 3 hours if the E.C.E. of chromium is 0.00018 gm per coulomb, is [SCRA 1994]
A)
1 amp done
clear
B)
1.5 amp done
clear
C)
0.5 amp done
clear
D)
2 amp done
clear
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question_answer42)
The current inside a copper voltameter [Roorkee 1992]
A)
Is half the outside value done
clear
B)
Is the same as the outside value done
clear
C)
Is twice the outside value done
clear
D)
Depends on the concentration of \[CuS{{O}_{4}}\] done
clear
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question_answer43)
The resistance of a cell does not depend on [RPET 1996]
A)
Current drawn from the cell done
clear
B)
Temperature of electrolyte done
clear
C)
Concentration of electrolyte done
clear
D)
The e.m.f. of the cell done
clear
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question_answer44)
The electrochemical equivalent of a metal is \[3.3\times {{10}^{-7}}\,kg/coulomb\]. The mass of the metal liberated at the cathode when a 3 A current is passed for 2 seconds will be [SCRA 1998; AIEEE 2004; DCE 2005]
A)
\[19.8\times {{10}^{-7}}kg\] done
clear
B)
\[9.39\times {{10}^{-7}}kg\] done
clear
C)
\[6.6\times {{10}^{-7}}kg\] done
clear
D)
\[1.1\times {{10}^{-7}}kg\] done
clear
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question_answer45)
Faraday?s 2nd law states that mass deposited on the electrode is directly proportional to [DCE 1999]
A)
Atomic mass done
clear
B)
Atomic mass × Velocity done
clear
C)
Atomic mass/Valency done
clear
D)
Valency done
clear
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question_answer46)
The relation between Faraday constant (F), chemical equivalent (E) and electrochemical equivalent (Z) is [SCRA 1994; AFMC 2000]
A)
\[F=EZ\] done
clear
B)
\[F=\frac{Z}{E}\] done
clear
C)
\[F=\frac{E}{Z}\] done
clear
D)
\[F=\frac{E}{{{Z}^{2}}}\] done
clear
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question_answer47)
The electrochemical equivalent of a material in an electrolyte depends on [MP PET 2001]
A)
The nature of the material done
clear
B)
The current through the electrolyte done
clear
C)
The amount of charge passed through electrolyte done
clear
D)
The amount of material present in electrolyte done
clear
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question_answer48)
On passing 96500 coulomb of charge through a solution \[CuS{{O}_{4}}\] the amount of copper liberated is [MP PMT 2001]
A)
64 gm done
clear
B)
32 gm done
clear
C)
32 kg done
clear
D)
64 kg done
clear
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question_answer49)
If 96500 coulombs of electricity liberates one gram equivalent of any substance, the time taken for a current of 0.15 amperes to deposite 20mg of copper from a solution of copper sulphate is (Chemical equivalent of copper = 32) [Kerala (Engg.) 2002]
A)
5 min 20 sec done
clear
B)
6 min 42 sec done
clear
C)
4 min 40 sec done
clear
D)
5 min 50 sec done
clear
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question_answer50)
How much current should be passed through acidified water for 100 s to liberate 0.224 litre of \[{{H}_{2}}\] [DCE 2002]
A)
22.4 A done
clear
B)
\[19.3\,\,A\] done
clear
C)
9.65 A done
clear
D)
1 A done
clear
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question_answer51)
Who among the following scientists made the statement ?"Chemical change can produce electricity" [DCE 2004]
A)
Galvani done
clear
B)
Faraday done
clear
C)
Coulomb done
clear
D)
Thomson done
clear
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question_answer52)
If a steady current of 4 amp maintained for 40 minutes, deposits 4.5 gm of zinc at the cathode and then the electro chemical equivalent will be [MH CET 2003]
A)
\[51\times {{10}^{-17}}\,gm/C\] done
clear
B)
\[28\times {{10}^{-6}}\,gm/C\] done
clear
C)
\[32\times {{10}^{-5}}\,gm/C\] done
clear
D)
\[47\times {{10}^{-5}}\,gm/C\] done
clear
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question_answer53)
The current flowing in a copper voltameter is 3.2 A. The number of copper ions \[(C{{u}^{2+}})\] deposited at the cathode per minute is [Pb. PET 2001]
A)
\[0.5\times {{10}^{20}}\] done
clear
B)
\[1.5\times {{10}^{20}}\] done
clear
C)
\[3\times {{10}^{20}}\] done
clear
D)
\[6\times {{10}^{20}}\] done
clear
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question_answer54)
A copper voltameter is connected in series with a heater coil of resistance \[0.1\,\Omega \]. A steady current flows in the circuit for twenty minutes and mass of 0.99 g of copper is deposited at the cathode. If electrochemical equivalent of copper is 0.00033 gm/C, then heat generated in the coil is [Pb. PET 2002]
A)
750 J done
clear
B)
650 J done
clear
C)
350 J done
clear
D)
250 J done
clear
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question_answer55)
E.C.E. of Cu and Ag are \[7\times {{10}^{-6}}\] and \[1.2\times {{10}^{-6}}.\]A certain current deposits 14 gm of Cu. Amount of Ag deposited is [Orissa PMT 2004]
A)
1.2 gm done
clear
B)
1.6 gm done
clear
C)
2.4 gm done
clear
D)
1.8 gm done
clear
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question_answer56)
The chemical equivalent of silver is 108. If the current in a silver voltameter is 2 Amp., the time required to deposit 27 grams of silver will be [MP PMT 2004]
A)
8.57 hrs done
clear
B)
6.70 hrs done
clear
C)
3.35 hrs done
clear
D)
12.50 hrs done
clear
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question_answer57)
Two voltameters, one of copper and another of silver, are joined in parallel. When a total charge q flows through the voltameters, equal amount of metals are deposited. If the electrochemical equivalents of copper and silver are \[{{z}_{1}}\] and \[{{z}_{2}}\] respectively the charge which flows through the silver voltameter is [AIEEE 2005]
A)
\[q\frac{{{z}_{1}}}{{{z}_{2}}}\] done
clear
B)
\[q\frac{{{z}_{2}}}{{{z}_{1}}}\] done
clear
C)
\[\frac{q}{1+\frac{{{z}_{1}}}{{{z}_{2}}}}\] done
clear
D)
\[\frac{q}{1+\frac{{{z}_{2}}}{{{z}_{1}}}}\] done
clear
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question_answer58)
The chemical equivalent of copper and zinc are 32 and 108 respectively. When copper and silver voltameter are connected in series and electric current is passed through for sometimes, 1.6 g of copper is deposited. Then, the mass of silver deposited will be [J & K CET 2005]
A)
3.5 g done
clear
B)
2.8 g done
clear
C)
5.4 g done
clear
D)
None of these done
clear
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question_answer59)
Ampere hour is the unit of [Orissa JEE 2005]
A)
Quantity of charge done
clear
B)
Potential done
clear
C)
Energy done
clear
D)
Current done
clear
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