Electrolytic Cells
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CHXII03:ELECTROCHEMISTRY

330206 How many electrons flow through the wire if a current of 1.5 ampere flow through it for 3hours?

1 \(1.60 \times 10^{19}\)
2 \(1.01 \times 10^{23}\)
3 \(1.01 \times 10^{19}\)
4 \(1.60 \times 10^{23}\)
MHTCET - 2021
CHXII03:ELECTROCHEMISTRY

330207 Calculate mass of a divalent metal produced at cathode by passing \(5\,\,{\text{amp}}\) current through its salt solution for 100 minutes.
\({\text{( molar mass of metal = x)}}\)

1 \(\frac{{{\text{15}}}}{{{\text{193}}}}{\text{x}}\)
2 \(\frac{{{\text{193}}}}{{{\text{30}}}}{\text{x}}\)
3 \(\frac{{{\text{193}}}}{{{\text{30}}}}{\text{x}}\)
4 \(\frac{{{\text{193}}}}{{{\text{15}}}}{\text{x}}\)
MHTCET - 2022
CHXII03:ELECTROCHEMISTRY

330208 The amount of current in faraday required for the reduction of 1 mol of \({\rm{C}}{{\rm{r}}_{\rm{2}}}{\rm{O}}_{\rm{7}}^{{\rm{2 - }}}\,\,{\rm{ions}}\,\,{\rm{to}}\,\,{\rm{C}}{{\rm{r}}^{{\rm{3 + }}}}\) is

1 1 F
2 2 F
3 6 F
4 4 F
KCET - 2018
CHXII03:ELECTROCHEMISTRY

330209 An electrolytic cell contains a solution of \(\mathrm{Ag}_{2} \mathrm{SO}_{4}\) and has platinum electrodes. A current is passed until 1.6 g of \(\mathrm{O}_{2}\) has been liberated at anode. The amount of silver deposited at cathode would be

1 107.88 g
2 1.6 g
3 0.8 g
4 21.60 g
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CHXII03:ELECTROCHEMISTRY

330206 How many electrons flow through the wire if a current of 1.5 ampere flow through it for 3hours?

1 \(1.60 \times 10^{19}\)
2 \(1.01 \times 10^{23}\)
3 \(1.01 \times 10^{19}\)
4 \(1.60 \times 10^{23}\)
MHTCET - 2021
CHXII03:ELECTROCHEMISTRY

330207 Calculate mass of a divalent metal produced at cathode by passing \(5\,\,{\text{amp}}\) current through its salt solution for 100 minutes.
\({\text{( molar mass of metal = x)}}\)

1 \(\frac{{{\text{15}}}}{{{\text{193}}}}{\text{x}}\)
2 \(\frac{{{\text{193}}}}{{{\text{30}}}}{\text{x}}\)
3 \(\frac{{{\text{193}}}}{{{\text{30}}}}{\text{x}}\)
4 \(\frac{{{\text{193}}}}{{{\text{15}}}}{\text{x}}\)
MHTCET - 2022
CHXII03:ELECTROCHEMISTRY

330208 The amount of current in faraday required for the reduction of 1 mol of \({\rm{C}}{{\rm{r}}_{\rm{2}}}{\rm{O}}_{\rm{7}}^{{\rm{2 - }}}\,\,{\rm{ions}}\,\,{\rm{to}}\,\,{\rm{C}}{{\rm{r}}^{{\rm{3 + }}}}\) is

1 1 F
2 2 F
3 6 F
4 4 F
KCET - 2018
CHXII03:ELECTROCHEMISTRY

330209 An electrolytic cell contains a solution of \(\mathrm{Ag}_{2} \mathrm{SO}_{4}\) and has platinum electrodes. A current is passed until 1.6 g of \(\mathrm{O}_{2}\) has been liberated at anode. The amount of silver deposited at cathode would be

1 107.88 g
2 1.6 g
3 0.8 g
4 21.60 g
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CHXII03:ELECTROCHEMISTRY

330206 How many electrons flow through the wire if a current of 1.5 ampere flow through it for 3hours?

1 \(1.60 \times 10^{19}\)
2 \(1.01 \times 10^{23}\)
3 \(1.01 \times 10^{19}\)
4 \(1.60 \times 10^{23}\)
MHTCET - 2021
CHXII03:ELECTROCHEMISTRY

330207 Calculate mass of a divalent metal produced at cathode by passing \(5\,\,{\text{amp}}\) current through its salt solution for 100 minutes.
\({\text{( molar mass of metal = x)}}\)

1 \(\frac{{{\text{15}}}}{{{\text{193}}}}{\text{x}}\)
2 \(\frac{{{\text{193}}}}{{{\text{30}}}}{\text{x}}\)
3 \(\frac{{{\text{193}}}}{{{\text{30}}}}{\text{x}}\)
4 \(\frac{{{\text{193}}}}{{{\text{15}}}}{\text{x}}\)
MHTCET - 2022
CHXII03:ELECTROCHEMISTRY

330208 The amount of current in faraday required for the reduction of 1 mol of \({\rm{C}}{{\rm{r}}_{\rm{2}}}{\rm{O}}_{\rm{7}}^{{\rm{2 - }}}\,\,{\rm{ions}}\,\,{\rm{to}}\,\,{\rm{C}}{{\rm{r}}^{{\rm{3 + }}}}\) is

1 1 F
2 2 F
3 6 F
4 4 F
KCET - 2018
CHXII03:ELECTROCHEMISTRY

330209 An electrolytic cell contains a solution of \(\mathrm{Ag}_{2} \mathrm{SO}_{4}\) and has platinum electrodes. A current is passed until 1.6 g of \(\mathrm{O}_{2}\) has been liberated at anode. The amount of silver deposited at cathode would be

1 107.88 g
2 1.6 g
3 0.8 g
4 21.60 g
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CHXII03:ELECTROCHEMISTRY

330206 How many electrons flow through the wire if a current of 1.5 ampere flow through it for 3hours?

1 \(1.60 \times 10^{19}\)
2 \(1.01 \times 10^{23}\)
3 \(1.01 \times 10^{19}\)
4 \(1.60 \times 10^{23}\)
MHTCET - 2021
CHXII03:ELECTROCHEMISTRY

330207 Calculate mass of a divalent metal produced at cathode by passing \(5\,\,{\text{amp}}\) current through its salt solution for 100 minutes.
\({\text{( molar mass of metal = x)}}\)

1 \(\frac{{{\text{15}}}}{{{\text{193}}}}{\text{x}}\)
2 \(\frac{{{\text{193}}}}{{{\text{30}}}}{\text{x}}\)
3 \(\frac{{{\text{193}}}}{{{\text{30}}}}{\text{x}}\)
4 \(\frac{{{\text{193}}}}{{{\text{15}}}}{\text{x}}\)
MHTCET - 2022
CHXII03:ELECTROCHEMISTRY

330208 The amount of current in faraday required for the reduction of 1 mol of \({\rm{C}}{{\rm{r}}_{\rm{2}}}{\rm{O}}_{\rm{7}}^{{\rm{2 - }}}\,\,{\rm{ions}}\,\,{\rm{to}}\,\,{\rm{C}}{{\rm{r}}^{{\rm{3 + }}}}\) is

1 1 F
2 2 F
3 6 F
4 4 F
KCET - 2018
CHXII03:ELECTROCHEMISTRY

330209 An electrolytic cell contains a solution of \(\mathrm{Ag}_{2} \mathrm{SO}_{4}\) and has platinum electrodes. A current is passed until 1.6 g of \(\mathrm{O}_{2}\) has been liberated at anode. The amount of silver deposited at cathode would be

1 107.88 g
2 1.6 g
3 0.8 g
4 21.60 g
For More Updates join with Us