Answer :
A current of 5.68 a is passed through a Fe(NO3)2 solution. This current has to be applied to the plate for 0.9hr (58mins) out of 7.20 g of iron to be deposited.
Iron has 2 valency in Fe(NO3)2
Hence, we can say that 2 moles of electrons are required for 1 mole of Fe to be deposited
Molar mass of Fe = 55.845 g/mol
5.68 g of Fe in moles = 0.1017 moles
2 mole of electrons are required to deposit 1 mole of Fe
1 mole of electron deposits, 0.5 mol of Fe
Moles of electrons required to deposit 0.1017 moles of Fe = 0.2034
1 mole of electrons carries a charge of 96500C of charge,
The charge carried by 0.2034 moles of electrons is equal to 19281.1C
Now we know, Current = Charge / time
Rearranging the terms, we have,
Time = Charge / Current
Substituting the values, we have
Time = 19281.1/5.68 = 3455.6 or 3456s appx which is equal to 58mins or 0.9Hr
Learn more about the current here
brainly.com/question/2264542
#SPJ4
