276030 How long a current of 3 amperes has to be passed through a solution of $\mathrm{AgNO}_{3}$ to coat a metal surface of $80 \mathrm{~cm}^{2}$ and $0.005 \mathrm{~mm}$ thick layer. Density of $\mathrm{Ag}$ is $10.5 \mathrm{~g} \mathrm{~cm}^{-3}$

276031 The number of coulombs required for the
deposition of 108 g of silver is

276032 A current of 2.0 A passed 5 hours through a molten metal salt deposits $22.2 \mathrm{~g}$ of metal (At wt. = 177). The oxidation state of the metal in the metal salt is

276034 On passing a current of 1.0 ampere for $16 \mathrm{~min}$ and $5 \mathrm{sec}$ through one litre solution of $\mathrm{CuCl}_{2}$, all copper of the solution was deposited at cathode. The strength of $\mathbf{C u C l}_{2}$ solution was (Molar mass of $\mathrm{Cu}=63.5$; Faraday constant $=96,500 \mathrm{Cmol}^{-1}$ )

276030 How long a current of 3 amperes has to be passed through a solution of $\mathrm{AgNO}_{3}$ to coat a metal surface of $80 \mathrm{~cm}^{2}$ and $0.005 \mathrm{~mm}$ thick layer. Density of $\mathrm{Ag}$ is $10.5 \mathrm{~g} \mathrm{~cm}^{-3}$

276031 The number of coulombs required for the
deposition of 108 g of silver is

276032 A current of 2.0 A passed 5 hours through a molten metal salt deposits $22.2 \mathrm{~g}$ of metal (At wt. = 177). The oxidation state of the metal in the metal salt is

276034 On passing a current of 1.0 ampere for $16 \mathrm{~min}$ and $5 \mathrm{sec}$ through one litre solution of $\mathrm{CuCl}_{2}$, all copper of the solution was deposited at cathode. The strength of $\mathbf{C u C l}_{2}$ solution was (Molar mass of $\mathrm{Cu}=63.5$; Faraday constant $=96,500 \mathrm{Cmol}^{-1}$ )

276030 How long a current of 3 amperes has to be passed through a solution of $\mathrm{AgNO}_{3}$ to coat a metal surface of $80 \mathrm{~cm}^{2}$ and $0.005 \mathrm{~mm}$ thick layer. Density of $\mathrm{Ag}$ is $10.5 \mathrm{~g} \mathrm{~cm}^{-3}$

276031 The number of coulombs required for the
deposition of 108 g of silver is

276032 A current of 2.0 A passed 5 hours through a molten metal salt deposits $22.2 \mathrm{~g}$ of metal (At wt. = 177). The oxidation state of the metal in the metal salt is

276034 On passing a current of 1.0 ampere for $16 \mathrm{~min}$ and $5 \mathrm{sec}$ through one litre solution of $\mathrm{CuCl}_{2}$, all copper of the solution was deposited at cathode. The strength of $\mathbf{C u C l}_{2}$ solution was (Molar mass of $\mathrm{Cu}=63.5$; Faraday constant $=96,500 \mathrm{Cmol}^{-1}$ )

276030 How long a current of 3 amperes has to be passed through a solution of $\mathrm{AgNO}_{3}$ to coat a metal surface of $80 \mathrm{~cm}^{2}$ and $0.005 \mathrm{~mm}$ thick layer. Density of $\mathrm{Ag}$ is $10.5 \mathrm{~g} \mathrm{~cm}^{-3}$

276031 The number of coulombs required for the
deposition of 108 g of silver is

276032 A current of 2.0 A passed 5 hours through a molten metal salt deposits $22.2 \mathrm{~g}$ of metal (At wt. = 177). The oxidation state of the metal in the metal salt is

276034 On passing a current of 1.0 ampere for $16 \mathrm{~min}$ and $5 \mathrm{sec}$ through one litre solution of $\mathrm{CuCl}_{2}$, all copper of the solution was deposited at cathode. The strength of $\mathbf{C u C l}_{2}$ solution was (Molar mass of $\mathrm{Cu}=63.5$; Faraday constant $=96,500 \mathrm{Cmol}^{-1}$ )