Question

A current of 5. 68 a is passed through a Fe(NO3)2 solution. How long, in hours, would this current have to be applied to plate out 7. 20 g of iron?

Answer 1

There are  1.2 hr would this current have to be applied to plate out 7. 20 g of iron .

Calculation ,

Given ; Current ( I ) = 5. 68 A

In $Fe(NO_{3} )_{2}$ , the valancy of Fe is +2 .

2 moles of $e^{-}$ are required for the decomposition of 1 mole of Fe .

7. 20 g  of Fe in moles  = 7. 20 g /55.845 g/mol =0.12 mole

x moles of  $e^{-}$ are required for the decomposition of 0.128 mole of Fe .

moles of   $e^{-}$ are required = 0.256 moles

Charge on 1 mole  of   $e^{-}$ = 96500 C

Charge on 0.256  mole  of   $e^{-}$ = 24704 C

Current ( I )= Q/t  

t =Q / I = 24704 C/5. 68 A = 4349 sec = 1.2 hr

Therefore , there are  1.2 hr would this current have to be applied to plate out 7. 20 g of iron .

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