How much electricity in terms of Faraday is required to produce $20.0 g$ of $C a$ from molten $C a C l_{2}$ .

1 F

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

2 F

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

20 F

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

0.1 F

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

Open in App

Solution

The correct option is A $1 F$
The corresponding reaction is,
$C a^{2 +} + 2 e^{-} ⟶ C a$
So, $2 F$ electricity is required to produce $1 m o l$ of $C a$
The molar mass of $C a$ is $40 g$
$∴$ To produce $20 g$ of $C a$ $1 F$ is required

Suggest Corrections

Similar questions

100

C a C l_{2}

(i) How much electricity in terms of Faraday required to produce.

20.0 g of Ca from molten $C a C l_{2} P$

(ii) How much electricity in terms of Faraday required to produce.

How much electricity in terms of Faraday is required to produce

(i) 20.0 g of Ca from molten CaCl₂.

(ii) 40.0 g of Al from molten Al₂O₃.

20.0 g

C a

C a C l_{2}

20.0 g

C a

C a C l_{2}

40.0 g

A l

A l_{2} O_{3}

Join BYJU'S Learning Program