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 ) ?

Options

A. 0.054 A
B. 0.214 A
C. 0.428 A
D. 0.027 A

Answer

A

Explanation

`[PtCl_(6)]^(2-) ` or `Pt^(4+)+4e^(-) rarr Pt`
`4xx96500` C of electricity will deposit Pt `=195g`
195 g of Pt will be deposited by `96500xx4C`
0.195 g of Pt will be deposited by
`(9500xx4xx0.195)/(195)`
Current, `I=(4xx96500xx0.195)/(195xx2xx60xx60)=0.054 V`