330232 Given that the standard potentials \(\left( {{{\rm{E}}^{\rm{o}}}} \right)\) of \({\rm{C}}{{\rm{u}}^{{\rm{2 + }}}}{\rm{/Cu}}\) and \({\rm{C}}{{\rm{u}}^{\rm{ + }}}{\rm{/Cu}}\) are \({\rm{0}}.{\rm{34}}{\mkern 1mu} {\mkern 1mu} {\rm{V}}\) and \({\rm{0}}.{\rm{522}}{\mkern 1mu} {\mkern 1mu} {\rm{V}}\) respectively, the \({{\rm{E}}^{\rm{o}}}\,\,{\rm{of}}\,\,{\rm{C}}{{\rm{u}}^{{\rm{2 + }}}}{\rm{/C}}{{\rm{u}}^{\rm{ + }}}\) is

330233 A current of 1.40 ampere is passed through \(500 \mathrm{~mL}\) of \(0.180 \mathrm{M}\) solution of zinc sulphate for 200 seconds. What will be the molarity of \(\mathrm{Zn}^{2+}\) ions after deposition of zinc?

330234 \({\rm{4}}{\rm{.5\;g}}\) of aluminium (atomic mass \(27{\rm{u}}\) ) is deposited at cathode from a molten electrolyte containing \({\rm{A}}{{\rm{l}}^{3 + }}\) ions by a certain quantity of electric charge. The volume of hydrogen produced at STP from \({{\rm{H}}^ + }\) ions in a solution by the same quantity of electric charge will be

330235 The number of Faradays(F) required to produce 20 g of calcium from molten
\({\rm{CaC}}{{\rm{l}}_{\rm{2}}}\) (Atomic mass of Ca \({\rm{ = 40g}}\,\,{\rm{mo}}{{\rm{l}}^{{\rm{ - 1}}}}\)) is:

330232 Given that the standard potentials \(\left( {{{\rm{E}}^{\rm{o}}}} \right)\) of \({\rm{C}}{{\rm{u}}^{{\rm{2 + }}}}{\rm{/Cu}}\) and \({\rm{C}}{{\rm{u}}^{\rm{ + }}}{\rm{/Cu}}\) are \({\rm{0}}.{\rm{34}}{\mkern 1mu} {\mkern 1mu} {\rm{V}}\) and \({\rm{0}}.{\rm{522}}{\mkern 1mu} {\mkern 1mu} {\rm{V}}\) respectively, the \({{\rm{E}}^{\rm{o}}}\,\,{\rm{of}}\,\,{\rm{C}}{{\rm{u}}^{{\rm{2 + }}}}{\rm{/C}}{{\rm{u}}^{\rm{ + }}}\) is

330233 A current of 1.40 ampere is passed through \(500 \mathrm{~mL}\) of \(0.180 \mathrm{M}\) solution of zinc sulphate for 200 seconds. What will be the molarity of \(\mathrm{Zn}^{2+}\) ions after deposition of zinc?

330234 \({\rm{4}}{\rm{.5\;g}}\) of aluminium (atomic mass \(27{\rm{u}}\) ) is deposited at cathode from a molten electrolyte containing \({\rm{A}}{{\rm{l}}^{3 + }}\) ions by a certain quantity of electric charge. The volume of hydrogen produced at STP from \({{\rm{H}}^ + }\) ions in a solution by the same quantity of electric charge will be

330235 The number of Faradays(F) required to produce 20 g of calcium from molten
\({\rm{CaC}}{{\rm{l}}_{\rm{2}}}\) (Atomic mass of Ca \({\rm{ = 40g}}\,\,{\rm{mo}}{{\rm{l}}^{{\rm{ - 1}}}}\)) is:

330232 Given that the standard potentials \(\left( {{{\rm{E}}^{\rm{o}}}} \right)\) of \({\rm{C}}{{\rm{u}}^{{\rm{2 + }}}}{\rm{/Cu}}\) and \({\rm{C}}{{\rm{u}}^{\rm{ + }}}{\rm{/Cu}}\) are \({\rm{0}}.{\rm{34}}{\mkern 1mu} {\mkern 1mu} {\rm{V}}\) and \({\rm{0}}.{\rm{522}}{\mkern 1mu} {\mkern 1mu} {\rm{V}}\) respectively, the \({{\rm{E}}^{\rm{o}}}\,\,{\rm{of}}\,\,{\rm{C}}{{\rm{u}}^{{\rm{2 + }}}}{\rm{/C}}{{\rm{u}}^{\rm{ + }}}\) is

330233 A current of 1.40 ampere is passed through \(500 \mathrm{~mL}\) of \(0.180 \mathrm{M}\) solution of zinc sulphate for 200 seconds. What will be the molarity of \(\mathrm{Zn}^{2+}\) ions after deposition of zinc?

330234 \({\rm{4}}{\rm{.5\;g}}\) of aluminium (atomic mass \(27{\rm{u}}\) ) is deposited at cathode from a molten electrolyte containing \({\rm{A}}{{\rm{l}}^{3 + }}\) ions by a certain quantity of electric charge. The volume of hydrogen produced at STP from \({{\rm{H}}^ + }\) ions in a solution by the same quantity of electric charge will be

330235 The number of Faradays(F) required to produce 20 g of calcium from molten
\({\rm{CaC}}{{\rm{l}}_{\rm{2}}}\) (Atomic mass of Ca \({\rm{ = 40g}}\,\,{\rm{mo}}{{\rm{l}}^{{\rm{ - 1}}}}\)) is:

330232 Given that the standard potentials \(\left( {{{\rm{E}}^{\rm{o}}}} \right)\) of \({\rm{C}}{{\rm{u}}^{{\rm{2 + }}}}{\rm{/Cu}}\) and \({\rm{C}}{{\rm{u}}^{\rm{ + }}}{\rm{/Cu}}\) are \({\rm{0}}.{\rm{34}}{\mkern 1mu} {\mkern 1mu} {\rm{V}}\) and \({\rm{0}}.{\rm{522}}{\mkern 1mu} {\mkern 1mu} {\rm{V}}\) respectively, the \({{\rm{E}}^{\rm{o}}}\,\,{\rm{of}}\,\,{\rm{C}}{{\rm{u}}^{{\rm{2 + }}}}{\rm{/C}}{{\rm{u}}^{\rm{ + }}}\) is

330233 A current of 1.40 ampere is passed through \(500 \mathrm{~mL}\) of \(0.180 \mathrm{M}\) solution of zinc sulphate for 200 seconds. What will be the molarity of \(\mathrm{Zn}^{2+}\) ions after deposition of zinc?

330234 \({\rm{4}}{\rm{.5\;g}}\) of aluminium (atomic mass \(27{\rm{u}}\) ) is deposited at cathode from a molten electrolyte containing \({\rm{A}}{{\rm{l}}^{3 + }}\) ions by a certain quantity of electric charge. The volume of hydrogen produced at STP from \({{\rm{H}}^ + }\) ions in a solution by the same quantity of electric charge will be

330235 The number of Faradays(F) required to produce 20 g of calcium from molten
\({\rm{CaC}}{{\rm{l}}_{\rm{2}}}\) (Atomic mass of Ca \({\rm{ = 40g}}\,\,{\rm{mo}}{{\rm{l}}^{{\rm{ - 1}}}}\)) is: