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

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

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

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

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

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

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

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

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

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

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

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

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

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

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

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