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 current ( in ma ) required to deposit 0.195 gr of platinum metal in 5.0 hours from a solution of PtCl_6^(-2) ( Atomic weight : 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 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)

How much current is required to deposit 0.195 g of elemental Pt from a solution containing (PtCl_(6)]^(2-) ion with a time period of 2 hrs ( Atomic mass of Pt = 195 ) ?

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 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 three hours. ECE of chromium is 0.00018 g C^(-1)