Calculate the electric current required to deposit `0.972 g` of chromium in three hours. ECE of chromium is `0.00018 g C^(-1)`

Calculate the electric current required to deposit 0.972 g of chromium in 3 hours . ECE of chromium is 0.00018 g C^(-1)

Calculate the current ( in Ma) required to deposit 0.195 g of platinum metal in 5.0 hours from a solution of PtCl_(6)^(2-) : ( Atomic weight : pt = 195 )

Calculate the quantity of electricity required to deposit 0.09 g of Aluminium during the following electrode reaction. Al^(3+) + 3e^- rarr Al .

Calculate the current (in mA) required to deposite 0.195g of platinum metal in 5.0 hours from a solution of [PtCl_6^(2-) :(Atomic mass:Pt=195)

Calculate the current (in mA) required to deposite 0.195g of platinum metal in 5.0 hours from a solution of [PtCl_6^(2-) :(Atomic mass:Pt=195)

Calculate the current (in mA) required to deposite 0.195g of platinum metal in 5.0 hours from a solution of [PtCl_6^(2-) :(Atomic mass:Pt=195)

Calculate the strength of the current required to deposit 1.2 g magnesium from molten MgCl_(2) in hour . [1F= 96,500Cmol^(-1), ("atomic mass"): Mg =24.0 u]

Calculate the strength of the current required to deposit 1.2 g magnesium from molten MgCl_(2) in hour . [1F= 96,500Cmol^(-1), ("atomic mass"): Mg =24.0 u]