Electrolytic Cells
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CHXII03:ELECTROCHEMISTRY

330198 Number of electrons involved in the reaction, when 1 Faraday of electricity is passed through an electrolytic solution is

1 \({\rm{12 \times 1}}{{\rm{0}}^{{\rm{46}}}}\)
2 \({\rm{96500}}\)
3 \({\rm{6}}{\rm{.022 \times 1}}{{\rm{0}}^{{\rm{23}}}}\)
4 \({\rm{8 \times 1}}{{\rm{0}}^{{\rm{16}}}}\)
MHTCET - 2020-3
CHXII03:ELECTROCHEMISTRY

330199 How many Faradays are required to reduce 1 mol of \({\rm{Br}}{{\rm{O}}_{\rm{3}}}^ \ominus {\mkern 1mu} {\rm{to}}\,{\mkern 1mu} {\rm{B}}{{\rm{r}}^ \ominus }\) in basic medium ?

1 6
2 \(1/6\)
3 3
4 \(1/3\)
CHXII03:ELECTROCHEMISTRY

330200 How many Coulombs of electricity are required for the reduction of 1 mole of \(\mathrm{MnO}_{4}^{-}\) to \(\mathrm{Mn}^{2+}\) ?

1 \(96500 \mathrm{C}\)
2 \(9.65 \times 10^{6} \mathrm{C}\)
3 \(4.83 \times 10^{5} \mathrm{C}\)
4 \(1.93 \times 10^{5} \mathrm{C}\)
CHXII03:ELECTROCHEMISTRY

330201 A current of 2.0 A passed for 5 hours through a molten metal salt deposits 22.2 g of metal (At wt.=177) . The oxidation state of the metal in the metal salt is

1 \({\rm{ + 1}}\)
2 \({\rm{ + 2}}\)
3 \({\rm{ + 3}}\)
4 \({\rm{ + 4}}\)
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CHXII03:ELECTROCHEMISTRY

330198 Number of electrons involved in the reaction, when 1 Faraday of electricity is passed through an electrolytic solution is

1 \({\rm{12 \times 1}}{{\rm{0}}^{{\rm{46}}}}\)
2 \({\rm{96500}}\)
3 \({\rm{6}}{\rm{.022 \times 1}}{{\rm{0}}^{{\rm{23}}}}\)
4 \({\rm{8 \times 1}}{{\rm{0}}^{{\rm{16}}}}\)
MHTCET - 2020-3
CHXII03:ELECTROCHEMISTRY

330199 How many Faradays are required to reduce 1 mol of \({\rm{Br}}{{\rm{O}}_{\rm{3}}}^ \ominus {\mkern 1mu} {\rm{to}}\,{\mkern 1mu} {\rm{B}}{{\rm{r}}^ \ominus }\) in basic medium ?

1 6
2 \(1/6\)
3 3
4 \(1/3\)
CHXII03:ELECTROCHEMISTRY

330200 How many Coulombs of electricity are required for the reduction of 1 mole of \(\mathrm{MnO}_{4}^{-}\) to \(\mathrm{Mn}^{2+}\) ?

1 \(96500 \mathrm{C}\)
2 \(9.65 \times 10^{6} \mathrm{C}\)
3 \(4.83 \times 10^{5} \mathrm{C}\)
4 \(1.93 \times 10^{5} \mathrm{C}\)
CHXII03:ELECTROCHEMISTRY

330201 A current of 2.0 A passed for 5 hours through a molten metal salt deposits 22.2 g of metal (At wt.=177) . The oxidation state of the metal in the metal salt is

1 \({\rm{ + 1}}\)
2 \({\rm{ + 2}}\)
3 \({\rm{ + 3}}\)
4 \({\rm{ + 4}}\)
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CHXII03:ELECTROCHEMISTRY

330198 Number of electrons involved in the reaction, when 1 Faraday of electricity is passed through an electrolytic solution is

1 \({\rm{12 \times 1}}{{\rm{0}}^{{\rm{46}}}}\)
2 \({\rm{96500}}\)
3 \({\rm{6}}{\rm{.022 \times 1}}{{\rm{0}}^{{\rm{23}}}}\)
4 \({\rm{8 \times 1}}{{\rm{0}}^{{\rm{16}}}}\)
MHTCET - 2020-3
CHXII03:ELECTROCHEMISTRY

330199 How many Faradays are required to reduce 1 mol of \({\rm{Br}}{{\rm{O}}_{\rm{3}}}^ \ominus {\mkern 1mu} {\rm{to}}\,{\mkern 1mu} {\rm{B}}{{\rm{r}}^ \ominus }\) in basic medium ?

1 6
2 \(1/6\)
3 3
4 \(1/3\)
CHXII03:ELECTROCHEMISTRY

330200 How many Coulombs of electricity are required for the reduction of 1 mole of \(\mathrm{MnO}_{4}^{-}\) to \(\mathrm{Mn}^{2+}\) ?

1 \(96500 \mathrm{C}\)
2 \(9.65 \times 10^{6} \mathrm{C}\)
3 \(4.83 \times 10^{5} \mathrm{C}\)
4 \(1.93 \times 10^{5} \mathrm{C}\)
CHXII03:ELECTROCHEMISTRY

330201 A current of 2.0 A passed for 5 hours through a molten metal salt deposits 22.2 g of metal (At wt.=177) . The oxidation state of the metal in the metal salt is

1 \({\rm{ + 1}}\)
2 \({\rm{ + 2}}\)
3 \({\rm{ + 3}}\)
4 \({\rm{ + 4}}\)
For More Updates join with Us
CHXII03:ELECTROCHEMISTRY

330198 Number of electrons involved in the reaction, when 1 Faraday of electricity is passed through an electrolytic solution is

1 \({\rm{12 \times 1}}{{\rm{0}}^{{\rm{46}}}}\)
2 \({\rm{96500}}\)
3 \({\rm{6}}{\rm{.022 \times 1}}{{\rm{0}}^{{\rm{23}}}}\)
4 \({\rm{8 \times 1}}{{\rm{0}}^{{\rm{16}}}}\)
MHTCET - 2020-3
CHXII03:ELECTROCHEMISTRY

330199 How many Faradays are required to reduce 1 mol of \({\rm{Br}}{{\rm{O}}_{\rm{3}}}^ \ominus {\mkern 1mu} {\rm{to}}\,{\mkern 1mu} {\rm{B}}{{\rm{r}}^ \ominus }\) in basic medium ?

1 6
2 \(1/6\)
3 3
4 \(1/3\)
CHXII03:ELECTROCHEMISTRY

330200 How many Coulombs of electricity are required for the reduction of 1 mole of \(\mathrm{MnO}_{4}^{-}\) to \(\mathrm{Mn}^{2+}\) ?

1 \(96500 \mathrm{C}\)
2 \(9.65 \times 10^{6} \mathrm{C}\)
3 \(4.83 \times 10^{5} \mathrm{C}\)
4 \(1.93 \times 10^{5} \mathrm{C}\)
CHXII03:ELECTROCHEMISTRY

330201 A current of 2.0 A passed for 5 hours through a molten metal salt deposits 22.2 g of metal (At wt.=177) . The oxidation state of the metal in the metal salt is

1 \({\rm{ + 1}}\)
2 \({\rm{ + 2}}\)
3 \({\rm{ + 3}}\)
4 \({\rm{ + 4}}\)