Question

how much time will it require to deposit 4g of Ca during electrolysis of molten CaCl2 with a current of 2A?​

Answer 1

Answer:

0.8 current then 1hour

Explanation:

Answer 2

Answer:

The time requires to deposit $4g$ of $Ca^{2+}$ is 160.8min during the electrolysis.

Explanation:

The chemical reaction of electrolysis of CaCl₂:

                 $Ca^{2+}+2e^{-}$  →   $Ca(s)$

Given, mass of calcium $=4g$

Number of moles of $Ca^{2+}=\frac{4}{40}=0.1moles$

1 mole of $Ca^{2+}$ requires $= 2 moles$ of electrons  

$0.1moles$ of $Ca^{2+}$ requires $=2*0.1=0.2moles$ of electrons

$1 mole$ of electrons $=96500Coulombs$

$0.2moles$ of electrons has charge, $q=(0.2)(96500)=19300C$

Given, current $I=2A$

We know, $I=\frac{q}{t}$

Here, time $t=\frac{q}{I}$

⇒  $t=\frac{19300C}{2A}=9650sec$ or $160.8min$