JEE Main & Advanced Chemistry Electrochemistry / विद्युत् रसायन Question Bank

done Faraday's law of electrolysis Total Questions - 94

• question_answer1)
  Amount of electricity that can deposit 108 gm of silver from AgNO3 solution is    [AFMC 1993; MP PMT 2004]
  A)
                  1 ampere             done clear
  B)
                  1 coulomb done clear
  C)
                  1 faraday             done clear
  D)
                  None of the above done clear
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• question_answer2)
  When 9.65 coulombs of electricity is passed through a solution of silver nitrate (atomic weight of \[Ag=107.87\] taking as 108) the amount of silver deposited is [EAMCET 1992; KCET 2000]
  A)
                  10.8 mg                done clear
  B)
                  5.4 mg done clear
  C)
                  16.2 mg                done clear
  D)
                  21.2 mg done clear
  View Solution play_arrow

• question_answer3)
  Three faradays 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           done clear
  B)
                  84 done clear
  C)
                  112 done clear
  D)
                  168 done clear
  View Solution play_arrow

• question_answer4)
  A silver cup is plated with silver by passing 965 coulombs of electricity, the amount of silver deposited is [EAMCET 1990; MP PET 1994, 97]
  A)
                  9.89 g    done clear
  B)
                  107.87 g done clear
  C)
                  1.0787 g               done clear
  D)
                  1.002 g done clear
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• question_answer5)
  The atomic weight of \[Al\] is 27. When a current of 5 Faradays is passed through a solution of \[A{{l}^{+++}}\]ions, the weight of \[Al\] deposited is                                               [NCERT 1984]
  A)
                  27 gm    done clear
  B)
                  36 gm done clear
  C)
                  45 gm    done clear
  D)
                  39 gm done clear
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• question_answer6)
  An apparatus used for the measurement of quantity of electricity is known as a                [BHU 1979]
  A)
                  Calorimeter        done clear
  B)
                  Cathetometer done clear
  C)
                  Coulometer        done clear
  D)
                  Colorimeter done clear
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• question_answer7)
  The unit of electrochemical equivalent is              [EAMCET 1980]
  A)
                  Gram    done clear
  B)
                  Gram/ampere done clear
  C)
                  Gram/coulomb done clear
  D)
                  Coulomb/gram done clear
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• question_answer8)
  A certain current liberated 0.504 gm of hydrogen in 2 hours. How many grams of copper can be liberated by the same current flowing for the same time in a copper sulphate solution [NCERT 1973, 77; CPMT 1979, 89; AIIMS 1998]
  A)
                  12.7 gm                done clear
  B)
                  15.9 gm done clear
  C)
                  31.8 gm                done clear
  D)
                  63.5 gm done clear
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• question_answer9)
  What weight of copper will be deposited by passing 2 Faradays of electricity through a cupric salt (Atomic weight of Cu = 63.5)  [NCERT 1975; CPMT 1977, 79]
  A)
                  2.0 gm  done clear
  B)
                  3.175 gm done clear
  C)
                  63.5 gm                done clear
  D)
                  127.0 gm done clear
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• question_answer10)
  If the current is passed into the solution of an electrolyte [AIIMS 1979]
  A)
                  Anions move towards anode, cations towards cathode done clear
  B)
                  Anions and cations both move towards anode done clear
  C)
                  Anions move towards cathode, cations towards anode done clear
  D)
                  No movement of ions takes place done clear
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• question_answer11)
  Unit of Faraday is
  A)
                  Ampere               done clear
  B)
                  Coulomb done clear
  C)
                  Coulomb \[mol{{e}^{-1}}\]          done clear
  D)
                  Coulomb \[Se{{c}^{-1}}\] done clear
  View Solution play_arrow

• question_answer12)
  On passing 0.1 Faraday of electricity through aluminium chloride, the amount of aluminium metal deposited on cathode is \[(Al=27)\]      [MP PMT 1991]
  A)
                  0.9 gm  done clear
  B)
                  0.3 gm done clear
  C)
                  0.27 gm                done clear
  D)
                  2.7 gm done clear
  View Solution play_arrow

• question_answer13)
  Which of the following represents the first law of Faraday [MP PMT 1991]
  A)
                  \[E=m{{c}^{2}}\]               done clear
  B)
                  \[E=hv\] done clear
  C)
                  \[m=ect\]            done clear
  D)
                  \[PV=nRT\] done clear
  View Solution play_arrow

• question_answer14)
  5 amperes is passed through a solution of zinc sulphate for 40 minutes. Find the amount of zinc deposited at the cathode               [CBSE PMT 1996]
  A)
                  40.65 gm              done clear
  B)
                  4.065 gm done clear
  C)
                  0.4065 gm           done clear
  D)
                  65.04 gm done clear
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• question_answer15)
  In an electroplating experiment \[m\,\,g\]of silver is deposited, when 4 amperes of current flows for 2 minutes. The amount (in \[gms\]) of silver deposited by 6 amperes of current flowing for 40 seconds will be [MNR 1991]
  A)
                  \[4m\]  done clear
  B)
                  \[m/2\] done clear
  C)
                  \[m/4\] done clear
  D)
                  \[2m\] done clear
  View Solution play_arrow

• question_answer16)
  On passing 3 ampere of electricity for 50 minutes, 1.8 gram metal deposits. The equivalent mass of metal is [MP PMT 1992]
  A)
                  20.5        done clear
  B)
                  25.8 done clear
  C)
                  19.3        done clear
  D)
                  30.7 done clear
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• question_answer17)
  The desired amount of charge for obtaining one mole of \[Al\] from \[A{{l}^{3+}}\]
  A)
                  \[3\times 96500\,\,C\]   done clear
  B)
                  \[96500\,\,C\] done clear
  C)
                  \[\frac{96500}{3}C\]        done clear
  D)
                  \[\frac{96500}{2}C\] done clear
  View Solution play_arrow

• question_answer18)
  On passing one faraday of electricity through the electrolytic cells containing \[A{{g}^{+}},\,\,N{{i}^{+2}}\]and \[C{{r}^{+3}}\]ions solution, the deposited \[Ag\,(At.\,\,wt.=108),\,\,Ni\,(At.\,wt.=59)\] and \[Cr\,(At.\,wt.=52)\] is                [AIIMS 1982]
  A)
                  \[Ag\]                   \[Ni\]                    \[Cr\]                 108 gm                29.5 gm                17.3 gm done clear
  B)
                  108 gm 59.0 gm                52.0 gm done clear
  C)
                  108.0 gm              108.0 gm              108.0 gm done clear
  D)
                  108 gm                 117.5 gm              166.0 gm done clear
  View Solution play_arrow

• question_answer19)
  One Faraday of electricity when passed through a solution of copper sulphate deposits [CPMT 1978]
  A)
                  1 mole of \[Cu\]                done clear
  B)
                  1 gm atom of \[Cu\] done clear
  C)
                  1 molecule of \[Cu\]        done clear
  D)
                  1 gm equivalent of \[Cu\] done clear
  View Solution play_arrow

• question_answer20)
  When 1 coulomb of charge is passed through electrolyte solution, then the mass deposited is equal to
  A)
                  Equivalent weight done clear
  B)
                  Atomic weight done clear
  C)
                  Electrochemical equivalent done clear
  D)
                  Chemical equivalent done clear
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• question_answer21)
  The platinum electrodes were immersed in a solution of cupric sulphate and electric current passed through the solution. After some time it was found that colour of copper sulphate disappeared with evolution of gas at the electrode. The colourless solution contains          [NCERT 1984]
  A)
                  Platinum sulphate           done clear
  B)
                  Copper hydroxide done clear
  C)
                  Copper sulphate              done clear
  D)
                  Sulphuric acid done clear
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• question_answer22)
  On passing \[C\] ampere of electricity through a electrolyte solution for \[t\] second, \[m\]gram metal deposits on cathode. The equivalent weight \[E\] of the metal is       [MP PMT 1990]
  A)
                  \[E=\frac{C\times t}{m\times 96500}\]   done clear
  B)
                  \[E=\frac{C\times m}{t\times 96500}\] done clear
  C)
                  \[E=\frac{96500\times m}{C\times t}\]   done clear
  D)
                  \[E=\frac{C\times t\times 96500}{m}\] done clear
  View Solution play_arrow

• question_answer23)
  How many Faradays are required to generate one gram atom of magnesium from \[MgC{{l}_{2}}\]         [MADT Bihar 1982]
  A)
                  1              done clear
  B)
                  2 done clear
  C)
                  3              done clear
  D)
                  4 done clear
  View Solution play_arrow

• question_answer24)
  To deposit 0.6354 gm of copper by electrolysis of aqueous cupric  sulphate solution, the amount of electricity required (in coulombs) is                                [MP PMT 1989]
  A)
                  9650       done clear
  B)
                  4825 done clear
  C)
                  3860       done clear
  D)
                  1930 done clear
  View Solution play_arrow

• question_answer25)
  In electrolysis of a fused salt, the weight of the deposit on an electrode will not depend on         [CPMT 1973]
  A)
                  Temperature of the bath done clear
  B)
                  Current intensity done clear
  C)
                  Electrochemical equivalent of ions done clear
  D)
                  Time for electrolysis done clear
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• question_answer26)
  Faraday's laws of electrolysis will fail when           [NCERT 1971]
  A)
                  Temperature is increased            done clear
  B)
                  Inert electrodes are used done clear
  C)
                  A mixture of electrolytes is used done clear
  D)
                  In none of these cases done clear
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• question_answer27)
  According to the first law of Faraday, the weight of a substance discharge at the electrode is
  A)
                  \[W=ZQ\]            done clear
  B)
                  \[W=eF\] done clear
  C)
                  \[W=\frac{Z}{F}\,It\]      done clear
  D)
                  \[W=ZI\] done clear
  View Solution play_arrow

• question_answer28)
  When 0.04 faraday of electricity is passed through a solution of \[CaS{{O}_{4}}\], then the weight of \[C{{a}^{2+}}\] metal deposited at the cathode is            [BHU 1996]
  A)
                  0.2 gm  done clear
  B)
                  0.4 gm done clear
  C)
                  0.6 gm  done clear
  D)
                  0.8 gm done clear
  View Solution play_arrow

• question_answer29)
  A current 2.0 A is passed for 5 hours through a molten metal salt deposits 22 g of metal (At. wt. =177). The oxidation state of the metal in the metal salt is      [KCET 1996]
  A)
                  + 1          done clear
  B)
                  + 2 done clear
  C)
                  + 3          done clear
  D)
                  + 4 done clear
  View Solution play_arrow

• question_answer30)
  How many atoms of calcium will be deposited from a solution of \[CaC{{l}_{2}}\] by a current of 25 milliamperes flowing for 60 seconds                                   [BHU 1999]
  A)
                  \[4.68\times {{10}^{18}}\]            done clear
  B)
                  \[4.68\times {{10}^{15}}\] done clear
  C)
                  \[4.68\times {{10}^{12}}\]            done clear
  D)
                  \[4.68\times {{10}^{9}}\] done clear
  View Solution play_arrow

• question_answer31)
  On passing 0.5 faraday of electricity through \[NaCl\], the amount of \[Cl\] deposited on cathode is [BHU 1997; RPET 1999]
  A)
                  35.5 gm                done clear
  B)
                  17.75 gm done clear
  C)
                  71 gm    done clear
  D)
                  142 gm done clear
  View Solution play_arrow

• question_answer32)
  What is the amount of chlorine evolved when 2 amperes of current is passed for 30 minutes in an aqueous solution of \[NaCl\]          [BHU 1998; AIIMS 1999]
  A)
                  66 g        done clear
  B)
                  1.32 g done clear
  C)
                  33 g        done clear
  D)
                  99 g done clear
  View Solution play_arrow

• question_answer33)
  On passing a current through \[KCl\] solution, \[19.5\,g\] of potassium is deposited. If the same quantity of electricity is passed through a solution of aluminium chloride, the amount of aluminium deposited is           [EAMCET 1997]
  A)
                  4.5 g      done clear
  B)
                  9.0 g done clear
  C)
                  13.5 g    done clear
  D)
                  27 g done clear
  E)
                  None is correct done clear
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• question_answer34)
  Electrolysis rules of Faraday?s states that mass deposited on electrode is proportional to               [CBSE PMT 2000]
  A)
                  \[m\,\,\propto {{I}^{2}}\]             done clear
  B)
                  \[m\,\,\propto Q\] done clear
  C)
                  \[m\,\,\propto \,\,{{Q}^{2}}\]    done clear
  D)
                  None of these done clear
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• question_answer35)
  A current being passed for two hour through a solution of an acid liberating 11.2 litre of oxygen at NTP at anode. What will be the amount of copper deposited at the cathode by the same current when passed through a solution of copper sulphate for the same time         [BVP 2003]
  A)
                  16 g        done clear
  B)
                  63 g done clear
  C)
                  31.5 g    done clear
  D)
                  8 g done clear
  View Solution play_arrow

• question_answer36)
  In a metal oxide, there is 20% oxygen by weight. Its equivalent weight is                                               [Pb. PMT 2000]
  A)
                  40           done clear
  B)
                  64 done clear
  C)
                  72           done clear
  D)
                  32 done clear
  View Solution play_arrow

• question_answer37)
  On the basis of the information available from the reaction \[\frac{4}{3}Al+{{O}_{2}}\to \frac{2}{3}A{{l}_{2}}{{O}_{3}},\Delta G=-827kJmo{{l}^{-1}}\] of \[{{O}_{2}}\], the minimum emf required to carry out an electrolysis of \[A{{l}_{2}}{{O}_{3}}\] is (F = 96500C \[mo{{l}^{-1}}\])  [CBSE PMT 2003]
  A)
                  8.56 V    done clear
  B)
                  2.14 V done clear
  C)
                  4.28 V    done clear
  D)
                  6.42 V done clear
  View Solution play_arrow

• question_answer38)
  Then during electrolysis of a solution of AgNO3, 9650 coulombs of charge pass through the electroplating bath, the mass of silver deposited in the cathode will be [AIEEE 2003]
  A)
                  1.08 g    done clear
  B)
                  10.8 g done clear
  C)
                  21.6 g    done clear
  D)
                  108 g done clear
  View Solution play_arrow

• question_answer39)
  Total charge on 1 mole of a monovalent metal ion is equal to [DPMT 2001]
  A)
                  \[9.65\times {{10}^{4}}\,\,\,Coulomb\]  done clear
  B)
                  \[6.28\times {{10}^{18}}\,\,\,Coulomb\] done clear
  C)
                  \[1.6\times {{10}^{-19}}\,\,\,Coulomb\] done clear
  D)
                  None of these done clear
  View Solution play_arrow

• question_answer40)
  When an electric current is passed through acidulated water 112 ml of hydrogen gas at N.T.P. collect at the cathode in 965 seconds. The current passed, in amperes is [MNR 1991; UPSEAT 2001]
  A)
                  1.0          done clear
  B)
                  0.5 done clear
  C)
                  0.1          done clear
  D)
                  2.0 done clear
  View Solution play_arrow

• question_answer41)
  How much chlorine will be liberated on passing one ampere current for 30 minutes through NaCl solution            [BVP 2003]
  A)
                  0.66 mole             done clear
  B)
                  0.33 mole done clear
  C)
                  0.66 gm                done clear
  D)
                  0.33 gm done clear
  View Solution play_arrow

• question_answer42)
  The number of electrons involved in redox reactions when a Faraday of electricity is passed through an electrolyte in solution is            [NCERT 1982; Pb. PMT 2002]
  A)
                  \[6\times {{10}^{23}}\]  done clear
  B)
                  \[6\times {{10}^{-23}}\] done clear
  C)
                  96500    done clear
  D)
                  \[8\times {{10}^{19}}\] done clear
  View Solution play_arrow

• question_answer43)
  Coulomb is equal to        [Orissa JEE 2002]
  A)
                  ampere ´ second             done clear
  B)
                  ampere ´ minute done clear
  C)
                  watt ´ second   done clear
  D)
                  volt ´ second done clear
  View Solution play_arrow

• question_answer44)
  The energy required to release 1 electron from \[H{{e}^{+}}\]is??. [Orissa JEE 2002]
  A)
                  + 54.4 eV              done clear
  B)
                  ? 13.6 eV done clear
  C)
                  + 27.2 eV done clear
  D)
                  Cannot be predicted done clear
  View Solution play_arrow

• question_answer45)
  Faraday's laws of electrolysis are related to the [IIT 1983]
  A)
                  Atomic number of cation done clear
  B)
                  Atomic number of anion done clear
  C)
                  Equivalent weight of the electrolyte done clear
  D)
                  Speed of the cation done clear
  View Solution play_arrow

• question_answer46)
  The electric charge for electrode decomposition of one gram equivalent of a substance is            [IIT 1984; KCET 1992]
  A)
                  One ampere per second done clear
  B)
                  96500 coulombs per second done clear
  C)
                  One ampere for one hour done clear
  D)
                  Charge on one mole of electrons done clear
  View Solution play_arrow

• question_answer47)
  The number of electrons passing per second through a cross-section of copper wire carrying \[{{10}^{-6}}\] amperes of current per second is found to be       [EAMCET 1985]
  A)
                  \[1.6\times {{10}^{-19}}\]             done clear
  B)
                  \[6\times {{10}^{-35}}\] done clear
  C)
                  \[6\times {{10}^{-16}}\]                done clear
  D)
                  \[6\times {{10}^{12}}\] done clear
  View Solution play_arrow

• question_answer48)
  The electrolytic cells, 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 cells will be [CPMT 1989]
  A)
                  3 : 1        done clear
  B)
                  2 : 1 done clear
  C)
                  1 : 1        done clear
  D)
                  3 : 2 done clear
  View Solution play_arrow

• question_answer49)
  When 96500 coulomb of electricity is passed through a copper sulphate solution, the amount of copper deposited will be           [MP PMT 1996]
  A)
                  0.25 mol               done clear
  B)
                  0.50 mol done clear
  C)
                  1.00 mol               done clear
  D)
                  2.00 mol done clear
  View Solution play_arrow

• question_answer50)
  During electrolysis of fused aluminium chloride \[0.9\,gm\] of aluminium was deposited on the cathode. The volume of chlorine liberated at the anode will be
  A)
                  2.24 litres             done clear
  B)
                  11.2 litres done clear
  C)
                  1.12 litres             done clear
  D)
                  5.6 litres done clear
  View Solution play_arrow

• question_answer51)
  Faraday has the dimensions of  [MP PET 1995]
  A)
                  Coulombs done clear
  B)
                  Coulomb equivalent done clear
  C)
                  Coulomb per equivalent done clear
  D)
                  Coulomb per degree Kelvin done clear
  View Solution play_arrow

• question_answer52)
  The required charge for one equivalent weight of silver deposite on cathode is                                 [Roorkee 1995]
  A)
                  \[9.65\times {{10}^{7}}C\]            done clear
  B)
                  \[9.65\times {{10}^{4}}C\] done clear
  C)
                  \[9.65\times {{10}^{3}}C\]            done clear
  D)
                  \[9.65\times {{10}^{5}}C\] done clear
  View Solution play_arrow

• question_answer53)
  96500 coulombs of electric current liberates from \[CuS{{O}_{4}}\] solution         [MP PMT 1995]
  A)
                  \[63.5\,gm\,Cu\]              done clear
  B)
                  \[31.75\,gm\,Cu\] done clear
  C)
                  \[96500\,gm\,Cu\]           done clear
  D)
                  \[100\,gm\,Cu\] done clear
  View Solution play_arrow

• question_answer54)
  A current of strength 2.5 amp was passed through \[CuS{{O}_{4}}\] solution for 6 minutes 26 seconds. The amount of copper deposited is                 (Atomic weight of \[Cu=63.5\])                 (1 faraday = 96500 coulombs) [EAMCET 1989; MP PET 1994]
  A)
                  0.3175 g               done clear
  B)
                  3.175 g done clear
  C)
                  0.635 g  done clear
  D)
                  6.35 g done clear
  View Solution play_arrow

• question_answer55)
  A certain quantity of electricity is passed through an aqueous solution of \[AgN{{O}_{3}}\] and cupric salt solution connected in series. The amount of \[Ag\] deposited is \[1.08\,gm\], the amount of copper deposited is (atomic weight of Cu = 63.5; Ag = 108)                                    [EAMCET 1986]
  A)
                  0.6454 g               done clear
  B)
                  6.354 g done clear
  C)
                  0.3177 g               done clear
  D)
                  3.177 g done clear
  View Solution play_arrow

• question_answer56)
  The number of electrons required to deposit 1gm  atom of aluminium (at. wt. = 27) from a solution of aluminium chloride will be (where N is Avogadro's number) [AIIMS 1992]
  A)
                  1 N         done clear
  B)
                  2 N done clear
  C)
                  3 N         done clear
  D)
                  4 N done clear
  View Solution play_arrow

• question_answer57)
  Three faradays of electricity are passed through molten \[A{{l}_{2}}{{O}_{3}}\], aqueous solution of \[CuS{{O}_{4}}\] and molten \[NaCl\] taken in different electrolytic cells. The amount of \[Al,\,Cu\] and \[Na\] deposited at the cathodes will be in the ratio of [BHU 1990]
  A)
                  1 mole : 2 mole : 3 mole done clear
  B)
   3 mole : 2 mole : 1mole done clear
  C)
   1 mole : 1.5 mole : 3 mole done clear
  D)
   1.5 mole : 2 mole : 3 mole done clear
  View Solution play_arrow

• question_answer58)
  An electrolytic cell contains a solution of \[A{{g}_{2}}S{{O}_{4}}\] and have 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 [CPMT 1971]
  A)
                  107.88 gm           done clear
  B)
                  1.6 gm done clear
  C)
                  0.8 gm  done clear
  D)
                  21.60 gm done clear
  View Solution play_arrow

• question_answer59)
  The aqueous solution of which of the following decomposes on passing electric current                [EAMCET 1973]
  A)
                  Canesugar           done clear
  B)
                  Urea done clear
  C)
                  Methanol            done clear
  D)
                  Potassium iodide done clear
  View Solution play_arrow

• question_answer60)
  The number of Faradays needed to reduce 4 gram equivalents of \[C{{u}^{++}}\] to \[Cu\] metal will be              [BHU 1981]
  A)
                  1              done clear
  B)
                  2 done clear
  C)
                  1/2         done clear
  D)
                  4 done clear
  View Solution play_arrow

• question_answer61)
  When electricity is passed through the solution of \[AlC{{l}_{3}},\,\,13.5\,\,gm\] of \[Al\] are deposited. The number of Faraday must be [NCERT 1974; MP PET 1992; MP PMT 1994]
  A)
                  0.50        done clear
  B)
                  1.00 done clear
  C)
                  1.50        done clear
  D)
                  2.00 done clear
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• question_answer62)
  The value of one Faraday is [AMU 1983; AFMC 1989; MP PET 2001]
  A)
                  \[95500\,\,C\,\,mo{{l}^{-1}}\]     done clear
  B)
                  \[96550\,\,C\,\,mo{{l}^{-1}}\] done clear
  C)
                  \[96500\,\,C\,\,mo{{l}^{-1}}\]     done clear
  D)
                  \[98500\,\,C\,\,mo{{l}^{-1}}\] done clear
  View Solution play_arrow

• question_answer63)
  The quantity of electricity needed to liberate 0.5 gram equivalent of an element is           [CPMT 1988; MP PMT 1997]
  A)
                  48250 Faradays done clear
  B)
                  48250 Coulombs done clear
  C)
                  193000 Faradays              done clear
  D)
                  193000 Coulombs done clear
  View Solution play_arrow

• question_answer64)
  The number of coulombs required for the deposition of 107.870 g of silver is      [MP PET/PMT 1998]
  A)
                  96,500   done clear
  B)
                  48,250 done clear
  C)
                  1,93,000               done clear
  D)
                  10,000 done clear
  View Solution play_arrow

• question_answer65)
  When one of ampere current flows for \[1\,\sec \]through a conductor, this quantity of electricity is known as [MP PMT 1993]
  A)
                  Faraday                done clear
  B)
                  Coulomb done clear
  C)
                  E.M.F.   done clear
  D)
                  Ohm done clear
  View Solution play_arrow

• question_answer66)
  The mass deposited at an electrode is directly proportional to [CPMT 1974; AFMC 1987; MP PET 2000]
  A)
                  Atomic weight   done clear
  B)
                  Equivalent weight done clear
  C)
                  Molecular weight             done clear
  D)
                  Atomic number done clear
  View Solution play_arrow

• question_answer67)
  From the solution of which of the following one faraday of electricity will liberate one gram atom of metal [MHCET 1999; MP PET 1993,2000; AFMC 2000]
  A)
                  \[NaCl\]               done clear
  B)
                  \[BaC{{l}_{2}}\] done clear
  C)
                  \[CuS{{O}_{4}}\]               done clear
  D)
                  \[AlC{{l}_{3}}\] done clear
  View Solution play_arrow

• question_answer68)
  On electrolysis, 1 mole of aluminium will be deposited from its molten salt by     [MH CET 2000]
  A)
                  3 moles of electrons       done clear
  B)
                  4 moles of electrons done clear
  C)
                  2 moles of electrons       done clear
  D)
                  1 mole of electrons done clear
  View Solution play_arrow

• question_answer69)
  The atomic weight of \[Fe\] is 56.  The weight of Fe deposited from \[FeC{{l}_{3}}\]solution by passing 0.6 Faraday of electricity is [MH CET 2000]
  A)
                  5.6 g      done clear
  B)
                  11.2 g done clear
  C)
                  22.4 g    done clear
  D)
                  33.6 g done clear
  View Solution play_arrow

• question_answer70)
  2.5 F of electricity are passed through a \[CuS{{O}_{4}}\] solution. The number of gm equivalent of Cu deposited on anode is [CPMT 1973; DPMT 1982; MP PMT 2001]
  A)
                  Zero       done clear
  B)
                  1.25 done clear
  C)
                  2.5          done clear
  D)
                  5.0 done clear
  View Solution play_arrow

• question_answer71)
  The equivalent weight of a certain trivalent element is 20. Molecular weight of its oxide is            [KCET 2003]
  A)
                  152         done clear
  B)
                  56 done clear
  C)
                  168         done clear
  D)
                  68 done clear
  View Solution play_arrow

• question_answer72)
  Silver is removed electrically from 200 ml of a 0.1 N solution of \[AgN{{O}_{3}}\] by a current of 0.1 ampere. How long will it take to remove half of the silver from the solution               [AMU 1999]
  A)
                  16 sec    done clear
  B)
                  96.5 sec done clear
  C)
                  100 sec  done clear
  D)
                  10 sec done clear
  View Solution play_arrow

• question_answer73)
  In order to separate oxygen from one mole of \[{{H}_{2}}O\] the required quantity of coulomb would be            [RPET 1999]
  A)
                  \[1.93\times {{10}^{5}}\]              done clear
  B)
                  \[9.6\times {{10}^{4}}\] done clear
  C)
                  1.8          done clear
  D)
                  3.2 done clear
  View Solution play_arrow

• question_answer74)
  A current of 0.25A is passed through \[CuS{{O}_{4}}\] solution placed in voltameter for 45 minutes. The amount of  Cu deposited on cathode is (At weight of \[Cu=63.6\]) [BHU 2001]
  A)
                  0.20 g    done clear
  B)
                  0.22 g done clear
  C)
                  0.25 g    done clear
  D)
                  0.30 g done clear
  View Solution play_arrow

• question_answer75)
  Faraday constant                                             [KCET (Med.) 2001]
  A)
                  Is a numerical constant done clear
  B)
                  Depends on equivalent done clear
  C)
                  Depends upon the current passed done clear
  D)
                  Depends on the number of electrons done clear
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• question_answer76)
  If 0.5 amp current is passed through acidified silver nitrate solution for 10 minutes. The mass of silver deposited on cathode, is (eq. wt. of silver nitrate = 108)            [AFMC 2001]
  A)
                  0.235 g  done clear
  B)
                  0.336 g done clear
  C)
                  0.536 g  done clear
  D)
                  0.636 g done clear
  View Solution play_arrow

• question_answer77)
  The unit for the electric current is             [KCET (Med.) 2001]
  A)
                  Ohm      done clear
  B)
                  Volt done clear
  C)
                  Ampere                done clear
  D)
                  Coulomb done clear
  View Solution play_arrow

• question_answer78)
  The quantity of electricity required to liberate  \[112\,\,\,c{{m}^{3}}\] of hydrogen at STP from acidified water is [KCET (Med.) 2001]
  A)
                  0.1 Faraday        done clear
  B)
                  1 Faraday done clear
  C)
                  965 Coulomb      done clear
  D)
                  96500 Coulomb done clear
  View Solution play_arrow

• question_answer79)
  Which solution will show highest resistance during the passage of current                                            [BHU 2001]
  A)
                  0.05 N \[NaCl\] done clear
  B)
                  2 N \[NaCl\] done clear
  C)
                  0.1 N \[NaCl\]    done clear
  D)
                  1 N \[NaCl\] done clear
  View Solution play_arrow

• question_answer80)
  4 g of copper was dissolved in concentrated nitric acid. The copper nitrate solution on strong heating gave 5 g of its oxide. The equivalent weight of copper is            [KCET 2004]
  A)
                  23           done clear
  B)
                  32 done clear
  C)
                  12           done clear
  D)
                  20 done clear
  View Solution play_arrow

• question_answer81)
  The amount of silver deposited by passing 241.25 coulomb of current through silver nitrate solution is    [MHCET 2003]
  A)
                  2.7 g      done clear
  B)
                  2.7 mg done clear
  C)
                  0.27 g    done clear
  D)
                  0.54 g done clear
  View Solution play_arrow

• question_answer82)
  When 1F of electricity is passed through acidulated water, \[{{O}_{2}}\]evolved is                                            [MHCET 2004]
  A)
                  \[11.2\ d{{m}^{3}}\]        done clear
  B)
                  \[5.6\,d{{m}^{3}}\] done clear
  C)
                  \[22.4\ d{{m}^{3}}\]        done clear
  D)
                  \[1.0\ d{{m}^{3}}\] done clear
  View Solution play_arrow

• question_answer83)
  Charge required to liberate 11.5 g sodium is [AIIMS 1992; DCE 2002]
  A)
                  0.5 F       done clear
  B)
                  0.1 F done clear
  C)
                  1.5 F       done clear
  D)
                  96500 coulombs done clear
  View Solution play_arrow

• question_answer84)
  In the electrolysis of water, one Faraday of electrical energy would evolve                                           [DCE 2004]
  A)
                  One mole of oxygen       done clear
  B)
                  One g atom of oxygen   done clear
  C)
                  8 g of oxygen     done clear
  D)
                  22.4 litres of oxygen done clear
  View Solution play_arrow

• question_answer85)
  In a galvanic cell, the electrons flow from              [KCET 2004]
  A)
                  Anode to cathode through the solution done clear
  B)
                  Cathode to anode through the solution  done clear
  C)
                  Anode to cathode through the external circuit done clear
  D)
                  Cathode to anode through the external circuit done clear
  View Solution play_arrow

• question_answer86)
  An electric current is passed through silver nitrate solution using silver electrodes. 10.79 g of silver was found to be deposited on the cathode if the same amount of electricity is passed through copper sulphate solution using copper electrodes, the weight of copper deposited on the cathode is [Kerala PMT 2004]
  A)
                  6.4 g      done clear
  B)
                  2.3 g done clear
  C)
                  12.8 g    done clear
  D)
                  1.6 g done clear
  E)
                  3.2 g done clear
  View Solution play_arrow

• question_answer87)
  The law of electrolysis were proposed by [CPMT 1982;Pb.CET 2003]
  A)
                  Kohlraush            done clear
  B)
                  Faraday   done clear
  C)
                  Nernst  done clear
  D)
                  Berthelot done clear
  View Solution play_arrow

• question_answer88)
  How many atoms of calcium will be deposited from a solution of \[CaC{{l}_{2}}\]by a current 0.25 mA following for 60 seconds                                               [BHU 2004]
  A)
                  \[4.68\times {{10}^{18}}\]            done clear
  B)
                  \[4.68\times {{10}^{15}}\] done clear
  C)
                  \[4.68\times {{10}^{12}}\]            done clear
  D)
                  \[4.68\times {{10}^{9}}\] done clear
  View Solution play_arrow

• question_answer89)
  The number of coulombs required to reduce 12.3 g of nitrobenzene to aniline                                   [UPSEAT 2003]
  A)
                  115800 C              done clear
  B)
                  5790 C done clear
  C)
                  28950 C done clear
  D)
                  57900 C done clear
  View Solution play_arrow

• question_answer90)
  During the process of electrolytic refining of copper, some metals present as impurity settle as 'anode mud'. These are [AIEEE 2005]
  A)
                  Sn and Ag            done clear
  B)
                  Pb and Zn done clear
  C)
                  Ag and Au           done clear
  D)
                  Fe and Ni done clear
  View Solution play_arrow

• question_answer91)
  A galvanic cell is set up from a zinc bar weighing 50g and 1.0litre, 1.0M, \[CuS{{O}_{4}}\] solution. How long would the cell run, assuming it delivers a steady current of 1.0 ampere [Roorkee 2000] 
  A)
                  48 hrs    done clear
  B)
                  41 hrs done clear
  C)
                  21 hrs    done clear
  D)
                  1 hr done clear
  View Solution play_arrow

• question_answer92)
  On passing electric current through molten aluminium chloride, 11.2 litre of \[C{{l}_{2}}\] is liberated at NTP at anode. The quantity of aluminium deposited at cathode is (at. wt. of Al = 27)                                     [JIPMER 2002]
  A)
                  9 g          done clear
  B)
                  18 g done clear
  C)
                  27 g        done clear
  D)
                  36 g done clear
  View Solution play_arrow

• question_answer93)
  An electric current is passed through silver voltameter connected to a water voltameter. The cathode of the silver voltameter weighed 0.108 g more at the end of the electrolysis. The volume of oxygen evolved at STP is [Kerala (Med.) 2003]
  A)
                  56 \[c{{m}^{3}}\]              done clear
  B)
                  550 \[c{{m}^{3}}\] done clear
  C)
                  5.6 \[c{{m}^{3}}\] done clear
  D)
                  11.2 \[c{{m}^{3}}\] done clear
  E)
                  22.4 \[c{{m}^{3}}\] done clear
  View Solution play_arrow

• question_answer94)
  During electrolysis of aqueous \[NaOH,\,4\,g\] of \[{{O}_{2}}\] gas is liberated at \[NTP\] at anode, \[{{H}_{2}}\] gas liberated at cathode is [CBSE PMT 1998]
  A)
                  2.8 litres               done clear
  B)
                  5.6 litres done clear
  C)
                  11.2 litres             done clear
  D)
                  22.4 litres done clear
  View Solution play_arrow