330194 What is the charge required for the reduction of two moles of \(\mathrm{Cu}^{2+}\) to \(\mathrm{Cu}\) ?

330195 Three faradays of electricity are passed through molten \({\rm{A}}{{\rm{l}}_{\rm{2}}}{{\rm{O}}_{\rm{3}}}\), aqueous solution of \({\rm{CuS}}{{\rm{O}}_{\rm{4}}}\) and molten NaCl taken in different electrolytic cells. The amount of Al, Cu and Na deposited at the cathodes will be in the ratio of

330196 Faraday’s law of electrolysis are related to the

330216 What is the weight of \(\mathrm{Al}\) deposited at cathode when 1 ampere current is passed through molten \(\mathrm{AlCl}_{3}\) for 9650 seconds? (At. mass of \(\mathrm{Al}=27\) )

330197 When \({\text{0}}{\text{.1mol MnO}}_{\text{4}}^{{\text{2 - }}}\) is oxidised, the quantity of electricity required to completely oxidise \(\mathrm{MnO}_{4}^{2-}\) to \(\mathrm{MnO}_{4}^{-}\) is:

330194 What is the charge required for the reduction of two moles of \(\mathrm{Cu}^{2+}\) to \(\mathrm{Cu}\) ?

330195 Three faradays of electricity are passed through molten \({\rm{A}}{{\rm{l}}_{\rm{2}}}{{\rm{O}}_{\rm{3}}}\), aqueous solution of \({\rm{CuS}}{{\rm{O}}_{\rm{4}}}\) and molten NaCl taken in different electrolytic cells. The amount of Al, Cu and Na deposited at the cathodes will be in the ratio of

330196 Faraday’s law of electrolysis are related to the

330216 What is the weight of \(\mathrm{Al}\) deposited at cathode when 1 ampere current is passed through molten \(\mathrm{AlCl}_{3}\) for 9650 seconds? (At. mass of \(\mathrm{Al}=27\) )

330197 When \({\text{0}}{\text{.1mol MnO}}_{\text{4}}^{{\text{2 - }}}\) is oxidised, the quantity of electricity required to completely oxidise \(\mathrm{MnO}_{4}^{2-}\) to \(\mathrm{MnO}_{4}^{-}\) is:

330194 What is the charge required for the reduction of two moles of \(\mathrm{Cu}^{2+}\) to \(\mathrm{Cu}\) ?

330195 Three faradays of electricity are passed through molten \({\rm{A}}{{\rm{l}}_{\rm{2}}}{{\rm{O}}_{\rm{3}}}\), aqueous solution of \({\rm{CuS}}{{\rm{O}}_{\rm{4}}}\) and molten NaCl taken in different electrolytic cells. The amount of Al, Cu and Na deposited at the cathodes will be in the ratio of

330196 Faraday’s law of electrolysis are related to the

330216 What is the weight of \(\mathrm{Al}\) deposited at cathode when 1 ampere current is passed through molten \(\mathrm{AlCl}_{3}\) for 9650 seconds? (At. mass of \(\mathrm{Al}=27\) )

330197 When \({\text{0}}{\text{.1mol MnO}}_{\text{4}}^{{\text{2 - }}}\) is oxidised, the quantity of electricity required to completely oxidise \(\mathrm{MnO}_{4}^{2-}\) to \(\mathrm{MnO}_{4}^{-}\) is:

330194 What is the charge required for the reduction of two moles of \(\mathrm{Cu}^{2+}\) to \(\mathrm{Cu}\) ?

330195 Three faradays of electricity are passed through molten \({\rm{A}}{{\rm{l}}_{\rm{2}}}{{\rm{O}}_{\rm{3}}}\), aqueous solution of \({\rm{CuS}}{{\rm{O}}_{\rm{4}}}\) and molten NaCl taken in different electrolytic cells. The amount of Al, Cu and Na deposited at the cathodes will be in the ratio of

330196 Faraday’s law of electrolysis are related to the

330216 What is the weight of \(\mathrm{Al}\) deposited at cathode when 1 ampere current is passed through molten \(\mathrm{AlCl}_{3}\) for 9650 seconds? (At. mass of \(\mathrm{Al}=27\) )

330197 When \({\text{0}}{\text{.1mol MnO}}_{\text{4}}^{{\text{2 - }}}\) is oxidised, the quantity of electricity required to completely oxidise \(\mathrm{MnO}_{4}^{2-}\) to \(\mathrm{MnO}_{4}^{-}\) is:

330194 What is the charge required for the reduction of two moles of \(\mathrm{Cu}^{2+}\) to \(\mathrm{Cu}\) ?

330195 Three faradays of electricity are passed through molten \({\rm{A}}{{\rm{l}}_{\rm{2}}}{{\rm{O}}_{\rm{3}}}\), aqueous solution of \({\rm{CuS}}{{\rm{O}}_{\rm{4}}}\) and molten NaCl taken in different electrolytic cells. The amount of Al, Cu and Na deposited at the cathodes will be in the ratio of

330196 Faraday’s law of electrolysis are related to the

330216 What is the weight of \(\mathrm{Al}\) deposited at cathode when 1 ampere current is passed through molten \(\mathrm{AlCl}_{3}\) for 9650 seconds? (At. mass of \(\mathrm{Al}=27\) )

330197 When \({\text{0}}{\text{.1mol MnO}}_{\text{4}}^{{\text{2 - }}}\) is oxidised, the quantity of electricity required to completely oxidise \(\mathrm{MnO}_{4}^{2-}\) to \(\mathrm{MnO}_{4}^{-}\) is: