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 o

Question

1 year ago

6

ut 7. 20 g of iron?

1 answer:

daser333 [38] · Answer 1 · 2024-02-08T01:09:58+03:00

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 .

To learn more about iron

#SPJ4