Electrolytic Cells
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CHXII03:ELECTROCHEMISTRY

330164 How many Faraday of electricity is required to deposit \(0.8 \mathrm{~g}\) of calcium at cathode by the electrolysis of \(\mathrm{CaCl}_{2}\) ?
(Molar mass of \(\mathrm{Ca}=40 \mathrm{~g} \mathrm{~mol}^{-1}\) )

1 \(4 \mathrm{~F}\)
2 \(0.04 \mathrm{~F}\)
3 \(2.5 \mathrm{~F}\)
4 \(2 \mathrm{~F}\)
MHTCET - 2021
CHXII03:ELECTROCHEMISTRY

330165 When during electrolysis of a solution of \({\rm{AgN}}{{\rm{O}}_{\rm{3}}}{\rm{,9650}}\) coulombs of charge pass through the electroplating bath, the mass of silver deposited on the cathode will be:

1 108 g
2 10.8 g
3 1.08 g
4 21.6 g
CHXII03:ELECTROCHEMISTRY

330166 A current of \(96.5 \mathrm{~A}\) is passed for \(18 \mathrm{~min}\) between nickel electrodes in \(500 \mathrm{~mL}\) solution of \(2{\text{M Ni}}{\left( {{\text{N}}{{\text{O}}_3}} \right)_2}\). The molarity of solution after electrolysis would be

1 \(0.46 \mathrm{M}\)
2 \(0.92 \mathrm{M}\)
3 \(0.625 \mathrm{M}\)
4 \(1.25 \mathrm{M}\)
AIIMS - 2007
CHXII03:ELECTROCHEMISTRY

330167 In the electrolysis of acidulated water, it is desired to obtain 1.12 cc of hydrogen per second under S.T.P condition. The current to be passed is

1 9.65 A
2 19.3 A
3 0.965 A
4 1.93 A
KCET - 2009
CHXII03:ELECTROCHEMISTRY

330168 The number of Faradays needed to reduce \(4 \mathrm{~g}\) equivalents of \(\mathrm{Cu}^{2+}\) to \(\mathrm{Cu}\) metal will be

1 1
2 2
3 \(1 / 2\)
4 4
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CHXII03:ELECTROCHEMISTRY

330164 How many Faraday of electricity is required to deposit \(0.8 \mathrm{~g}\) of calcium at cathode by the electrolysis of \(\mathrm{CaCl}_{2}\) ?
(Molar mass of \(\mathrm{Ca}=40 \mathrm{~g} \mathrm{~mol}^{-1}\) )

1 \(4 \mathrm{~F}\)
2 \(0.04 \mathrm{~F}\)
3 \(2.5 \mathrm{~F}\)
4 \(2 \mathrm{~F}\)
MHTCET - 2021
CHXII03:ELECTROCHEMISTRY

330165 When during electrolysis of a solution of \({\rm{AgN}}{{\rm{O}}_{\rm{3}}}{\rm{,9650}}\) coulombs of charge pass through the electroplating bath, the mass of silver deposited on the cathode will be:

1 108 g
2 10.8 g
3 1.08 g
4 21.6 g
CHXII03:ELECTROCHEMISTRY

330166 A current of \(96.5 \mathrm{~A}\) is passed for \(18 \mathrm{~min}\) between nickel electrodes in \(500 \mathrm{~mL}\) solution of \(2{\text{M Ni}}{\left( {{\text{N}}{{\text{O}}_3}} \right)_2}\). The molarity of solution after electrolysis would be

1 \(0.46 \mathrm{M}\)
2 \(0.92 \mathrm{M}\)
3 \(0.625 \mathrm{M}\)
4 \(1.25 \mathrm{M}\)
AIIMS - 2007
CHXII03:ELECTROCHEMISTRY

330167 In the electrolysis of acidulated water, it is desired to obtain 1.12 cc of hydrogen per second under S.T.P condition. The current to be passed is

1 9.65 A
2 19.3 A
3 0.965 A
4 1.93 A
KCET - 2009
CHXII03:ELECTROCHEMISTRY

330168 The number of Faradays needed to reduce \(4 \mathrm{~g}\) equivalents of \(\mathrm{Cu}^{2+}\) to \(\mathrm{Cu}\) metal will be

1 1
2 2
3 \(1 / 2\)
4 4
For More Updates join with Us
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CHXII03:ELECTROCHEMISTRY

330164 How many Faraday of electricity is required to deposit \(0.8 \mathrm{~g}\) of calcium at cathode by the electrolysis of \(\mathrm{CaCl}_{2}\) ?
(Molar mass of \(\mathrm{Ca}=40 \mathrm{~g} \mathrm{~mol}^{-1}\) )

1 \(4 \mathrm{~F}\)
2 \(0.04 \mathrm{~F}\)
3 \(2.5 \mathrm{~F}\)
4 \(2 \mathrm{~F}\)
MHTCET - 2021
CHXII03:ELECTROCHEMISTRY

330165 When during electrolysis of a solution of \({\rm{AgN}}{{\rm{O}}_{\rm{3}}}{\rm{,9650}}\) coulombs of charge pass through the electroplating bath, the mass of silver deposited on the cathode will be:

1 108 g
2 10.8 g
3 1.08 g
4 21.6 g
CHXII03:ELECTROCHEMISTRY

330166 A current of \(96.5 \mathrm{~A}\) is passed for \(18 \mathrm{~min}\) between nickel electrodes in \(500 \mathrm{~mL}\) solution of \(2{\text{M Ni}}{\left( {{\text{N}}{{\text{O}}_3}} \right)_2}\). The molarity of solution after electrolysis would be

1 \(0.46 \mathrm{M}\)
2 \(0.92 \mathrm{M}\)
3 \(0.625 \mathrm{M}\)
4 \(1.25 \mathrm{M}\)
AIIMS - 2007
CHXII03:ELECTROCHEMISTRY

330167 In the electrolysis of acidulated water, it is desired to obtain 1.12 cc of hydrogen per second under S.T.P condition. The current to be passed is

1 9.65 A
2 19.3 A
3 0.965 A
4 1.93 A
KCET - 2009
CHXII03:ELECTROCHEMISTRY

330168 The number of Faradays needed to reduce \(4 \mathrm{~g}\) equivalents of \(\mathrm{Cu}^{2+}\) to \(\mathrm{Cu}\) metal will be

1 1
2 2
3 \(1 / 2\)
4 4
NEET DIGITAL LIBRARY
CHXII03:ELECTROCHEMISTRY

330164 How many Faraday of electricity is required to deposit \(0.8 \mathrm{~g}\) of calcium at cathode by the electrolysis of \(\mathrm{CaCl}_{2}\) ?
(Molar mass of \(\mathrm{Ca}=40 \mathrm{~g} \mathrm{~mol}^{-1}\) )

1 \(4 \mathrm{~F}\)
2 \(0.04 \mathrm{~F}\)
3 \(2.5 \mathrm{~F}\)
4 \(2 \mathrm{~F}\)
MHTCET - 2021
CHXII03:ELECTROCHEMISTRY

330165 When during electrolysis of a solution of \({\rm{AgN}}{{\rm{O}}_{\rm{3}}}{\rm{,9650}}\) coulombs of charge pass through the electroplating bath, the mass of silver deposited on the cathode will be:

1 108 g
2 10.8 g
3 1.08 g
4 21.6 g
CHXII03:ELECTROCHEMISTRY

330166 A current of \(96.5 \mathrm{~A}\) is passed for \(18 \mathrm{~min}\) between nickel electrodes in \(500 \mathrm{~mL}\) solution of \(2{\text{M Ni}}{\left( {{\text{N}}{{\text{O}}_3}} \right)_2}\). The molarity of solution after electrolysis would be

1 \(0.46 \mathrm{M}\)
2 \(0.92 \mathrm{M}\)
3 \(0.625 \mathrm{M}\)
4 \(1.25 \mathrm{M}\)
AIIMS - 2007
CHXII03:ELECTROCHEMISTRY

330167 In the electrolysis of acidulated water, it is desired to obtain 1.12 cc of hydrogen per second under S.T.P condition. The current to be passed is

1 9.65 A
2 19.3 A
3 0.965 A
4 1.93 A
KCET - 2009
CHXII03:ELECTROCHEMISTRY

330168 The number of Faradays needed to reduce \(4 \mathrm{~g}\) equivalents of \(\mathrm{Cu}^{2+}\) to \(\mathrm{Cu}\) metal will be

1 1
2 2
3 \(1 / 2\)
4 4
Join With Us for More Updates
CHXII03:ELECTROCHEMISTRY

330164 How many Faraday of electricity is required to deposit \(0.8 \mathrm{~g}\) of calcium at cathode by the electrolysis of \(\mathrm{CaCl}_{2}\) ?
(Molar mass of \(\mathrm{Ca}=40 \mathrm{~g} \mathrm{~mol}^{-1}\) )

1 \(4 \mathrm{~F}\)
2 \(0.04 \mathrm{~F}\)
3 \(2.5 \mathrm{~F}\)
4 \(2 \mathrm{~F}\)
MHTCET - 2021
CHXII03:ELECTROCHEMISTRY

330165 When during electrolysis of a solution of \({\rm{AgN}}{{\rm{O}}_{\rm{3}}}{\rm{,9650}}\) coulombs of charge pass through the electroplating bath, the mass of silver deposited on the cathode will be:

1 108 g
2 10.8 g
3 1.08 g
4 21.6 g
CHXII03:ELECTROCHEMISTRY

330166 A current of \(96.5 \mathrm{~A}\) is passed for \(18 \mathrm{~min}\) between nickel electrodes in \(500 \mathrm{~mL}\) solution of \(2{\text{M Ni}}{\left( {{\text{N}}{{\text{O}}_3}} \right)_2}\). The molarity of solution after electrolysis would be

1 \(0.46 \mathrm{M}\)
2 \(0.92 \mathrm{M}\)
3 \(0.625 \mathrm{M}\)
4 \(1.25 \mathrm{M}\)
AIIMS - 2007
CHXII03:ELECTROCHEMISTRY

330167 In the electrolysis of acidulated water, it is desired to obtain 1.12 cc of hydrogen per second under S.T.P condition. The current to be passed is

1 9.65 A
2 19.3 A
3 0.965 A
4 1.93 A
KCET - 2009
CHXII03:ELECTROCHEMISTRY

330168 The number of Faradays needed to reduce \(4 \mathrm{~g}\) equivalents of \(\mathrm{Cu}^{2+}\) to \(\mathrm{Cu}\) metal will be

1 1
2 2
3 \(1 / 2\)
4 4