330210 The charge required for the reduction of 1 mole of \({\rm{MnO}}_{\rm{4}}^{\rm{ - }}\,\,{\rm{to}}\,\,{\rm{Mn}}{{\rm{O}}_{\rm{2}}}\)

330211 A current of 2 A was passed for one hour through a solution of \({\rm{CuS}}{{\rm{O}}_{\rm{4}}}{\rm{.0}}{\rm{.237g}}\,\,{\rm{of}}\,\,{\rm{C}}{{\rm{u}}^{{\rm{2 + }}}}\) ions was discharged at cathode. The current efficiency is

330212 Three electrolytic cells A, B, C containing solutions of \({\rm{ZnS}}{{\rm{O}}_{\rm{4}}}{\rm{,}}\,\,{\rm{AgN}}{{\rm{O}}_{\rm{3}}}\,\,{\rm{and}}\,\,{\rm{CuS}}{{\rm{O}}_{\rm{4}}}\) respectively are connected in series. A steady current of 1.5 amperes was passed through them until 1.45 g of silver deposited at the cathode of cell B. What mass of zinc was deposited? (At. Mass of Ag = 108 amu, At. Mass of Zn = 65.3 amu)

330213 When 0.1 mol \({\rm{MnO}}_{\rm{4}}^{{\rm{2 - }}}\) is oxidised the quantity of electricity required to completely oxidise \({\rm{MnO}}_{\rm{4}}^{{\rm{2 - }}}\,\,{\rm{to}}\,\,{\rm{MnO}}_{\rm{4}}^{\rm{ - }}\) is

330214 The number of moles of electrons passed when currect of 2 A is passed through a solution of electrolyte for 20 minutes is

330210 The charge required for the reduction of 1 mole of \({\rm{MnO}}_{\rm{4}}^{\rm{ - }}\,\,{\rm{to}}\,\,{\rm{Mn}}{{\rm{O}}_{\rm{2}}}\)

330211 A current of 2 A was passed for one hour through a solution of \({\rm{CuS}}{{\rm{O}}_{\rm{4}}}{\rm{.0}}{\rm{.237g}}\,\,{\rm{of}}\,\,{\rm{C}}{{\rm{u}}^{{\rm{2 + }}}}\) ions was discharged at cathode. The current efficiency is

330212 Three electrolytic cells A, B, C containing solutions of \({\rm{ZnS}}{{\rm{O}}_{\rm{4}}}{\rm{,}}\,\,{\rm{AgN}}{{\rm{O}}_{\rm{3}}}\,\,{\rm{and}}\,\,{\rm{CuS}}{{\rm{O}}_{\rm{4}}}\) respectively are connected in series. A steady current of 1.5 amperes was passed through them until 1.45 g of silver deposited at the cathode of cell B. What mass of zinc was deposited? (At. Mass of Ag = 108 amu, At. Mass of Zn = 65.3 amu)

330213 When 0.1 mol \({\rm{MnO}}_{\rm{4}}^{{\rm{2 - }}}\) is oxidised the quantity of electricity required to completely oxidise \({\rm{MnO}}_{\rm{4}}^{{\rm{2 - }}}\,\,{\rm{to}}\,\,{\rm{MnO}}_{\rm{4}}^{\rm{ - }}\) is

330214 The number of moles of electrons passed when currect of 2 A is passed through a solution of electrolyte for 20 minutes is

330210 The charge required for the reduction of 1 mole of \({\rm{MnO}}_{\rm{4}}^{\rm{ - }}\,\,{\rm{to}}\,\,{\rm{Mn}}{{\rm{O}}_{\rm{2}}}\)

330211 A current of 2 A was passed for one hour through a solution of \({\rm{CuS}}{{\rm{O}}_{\rm{4}}}{\rm{.0}}{\rm{.237g}}\,\,{\rm{of}}\,\,{\rm{C}}{{\rm{u}}^{{\rm{2 + }}}}\) ions was discharged at cathode. The current efficiency is

330212 Three electrolytic cells A, B, C containing solutions of \({\rm{ZnS}}{{\rm{O}}_{\rm{4}}}{\rm{,}}\,\,{\rm{AgN}}{{\rm{O}}_{\rm{3}}}\,\,{\rm{and}}\,\,{\rm{CuS}}{{\rm{O}}_{\rm{4}}}\) respectively are connected in series. A steady current of 1.5 amperes was passed through them until 1.45 g of silver deposited at the cathode of cell B. What mass of zinc was deposited? (At. Mass of Ag = 108 amu, At. Mass of Zn = 65.3 amu)

330213 When 0.1 mol \({\rm{MnO}}_{\rm{4}}^{{\rm{2 - }}}\) is oxidised the quantity of electricity required to completely oxidise \({\rm{MnO}}_{\rm{4}}^{{\rm{2 - }}}\,\,{\rm{to}}\,\,{\rm{MnO}}_{\rm{4}}^{\rm{ - }}\) is

330214 The number of moles of electrons passed when currect of 2 A is passed through a solution of electrolyte for 20 minutes is

330210 The charge required for the reduction of 1 mole of \({\rm{MnO}}_{\rm{4}}^{\rm{ - }}\,\,{\rm{to}}\,\,{\rm{Mn}}{{\rm{O}}_{\rm{2}}}\)

330211 A current of 2 A was passed for one hour through a solution of \({\rm{CuS}}{{\rm{O}}_{\rm{4}}}{\rm{.0}}{\rm{.237g}}\,\,{\rm{of}}\,\,{\rm{C}}{{\rm{u}}^{{\rm{2 + }}}}\) ions was discharged at cathode. The current efficiency is

330212 Three electrolytic cells A, B, C containing solutions of \({\rm{ZnS}}{{\rm{O}}_{\rm{4}}}{\rm{,}}\,\,{\rm{AgN}}{{\rm{O}}_{\rm{3}}}\,\,{\rm{and}}\,\,{\rm{CuS}}{{\rm{O}}_{\rm{4}}}\) respectively are connected in series. A steady current of 1.5 amperes was passed through them until 1.45 g of silver deposited at the cathode of cell B. What mass of zinc was deposited? (At. Mass of Ag = 108 amu, At. Mass of Zn = 65.3 amu)

330213 When 0.1 mol \({\rm{MnO}}_{\rm{4}}^{{\rm{2 - }}}\) is oxidised the quantity of electricity required to completely oxidise \({\rm{MnO}}_{\rm{4}}^{{\rm{2 - }}}\,\,{\rm{to}}\,\,{\rm{MnO}}_{\rm{4}}^{\rm{ - }}\) is

330214 The number of moles of electrons passed when currect of 2 A is passed through a solution of electrolyte for 20 minutes is

330210 The charge required for the reduction of 1 mole of \({\rm{MnO}}_{\rm{4}}^{\rm{ - }}\,\,{\rm{to}}\,\,{\rm{Mn}}{{\rm{O}}_{\rm{2}}}\)

330211 A current of 2 A was passed for one hour through a solution of \({\rm{CuS}}{{\rm{O}}_{\rm{4}}}{\rm{.0}}{\rm{.237g}}\,\,{\rm{of}}\,\,{\rm{C}}{{\rm{u}}^{{\rm{2 + }}}}\) ions was discharged at cathode. The current efficiency is

330212 Three electrolytic cells A, B, C containing solutions of \({\rm{ZnS}}{{\rm{O}}_{\rm{4}}}{\rm{,}}\,\,{\rm{AgN}}{{\rm{O}}_{\rm{3}}}\,\,{\rm{and}}\,\,{\rm{CuS}}{{\rm{O}}_{\rm{4}}}\) respectively are connected in series. A steady current of 1.5 amperes was passed through them until 1.45 g of silver deposited at the cathode of cell B. What mass of zinc was deposited? (At. Mass of Ag = 108 amu, At. Mass of Zn = 65.3 amu)

330213 When 0.1 mol \({\rm{MnO}}_{\rm{4}}^{{\rm{2 - }}}\) is oxidised the quantity of electricity required to completely oxidise \({\rm{MnO}}_{\rm{4}}^{{\rm{2 - }}}\,\,{\rm{to}}\,\,{\rm{MnO}}_{\rm{4}}^{\rm{ - }}\) is

330214 The number of moles of electrons passed when currect of 2 A is passed through a solution of electrolyte for 20 minutes is