Three faradays of electricity was passed through an aqueous solution of iron (II) bromide. The mass of iron metal (at. mass 56) deposited at the cathode is :-

56

No worries! We‘ve got your back. Try BYJU‘S free classes today!

84

Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses

112

No worries! We‘ve got your back. Try BYJU‘S free classes today!

168

No worries! We‘ve got your back. Try BYJU‘S free classes today!

Open in App

Solution

The correct option is B $84$ g
$1 F$ ion discharge $= \frac{56}{2} \times 3$
$3 F ⟶ 84 g$

Suggest Corrections

Similar questions

Q. Three faradays of electricity was passed through an aqueous solution of iron(II) bromide. The mass of iron metal (At. mass

56

) deposited at the cathode is:

3

Faradays of electricity was passed through an aqueous solution of iron

(I I)

bromide. The weight (in g) of iron metal (atomic weight

= 56

amu) deposited at the cathode is:

Three faradays electricity was passed through an aqueous solution of iron (II)

bromide. The weight of iron metal (at. wt. = 56) deposited at the cathode (in

gm) is

[EAMCET 1991]

Q. If

3

faradays of electricity are passed through an iron (II) bromide solution, how many grams of iron metal will be deposited? (At. mass of iron

= 56)

Three Faradays of electricity was passed through an aqueous solution of magnesium bromide. The weight of magnesium metal deposited at the cathode in grams is:

Join BYJU'S Learning Program

Three faradays of electricity was passed through an aqueous solution of iron (II) bromide. The mass of iron metal (at. mass 56) deposited at the cathode is :-

The correct option is B 84 g1F ion discharge =562×33F⟶84g

The correct option is B $84$ g
$1 F$ ion discharge $= \frac{56}{2} \times 3$
$3 F ⟶ 84 g$