Question

How long would it take to deposit 50 g of Al from
an electrolytic cell containing Al,O, using a current
of 105 ampere?
1.32 h
2.15 h
1.42 h
1.54 h​

Answer 1

Answer:

Explanation:

option a. 1.32 h

Answer 2

Answer:

For a electrolytic cell containing Al₂O₃, the time required to deposit 50g of Al is equal to 1.42hr.

Therefore, the option (3) is correct.

Explanation:

The deposition of aluminium in electrolytic cell containing Al₂O₃:-

Al³⁺ (aq)  +   3e⁻ $\longrightarrow$   Al (s)

From the Faraday's law of electrolysis:-

More the charge pass, more the substance will deposit.

W ∝ Q

W = Z × i × t                                                              ..................(1)

Where $i$ is the current passed and t is time and W is weight deposited.

and, Z is electrochemical equivalent

∴   $Z=\frac{Eq. \; mass}{95000}$

Equivalent mass of Aluminium $=\frac{27}{3}=9$

Given, current $i=105A$  and $W= 50g$

Put the value of W, $i$ and Z in eq.(1):

$(50)=\frac{9}{96500}*(105)*t$

$t=\frac{(50)(96500)}{(9)(105)}$

$t=5105.8sec$

$t=1.42hr$

Therefore, the time required to deposit 50g of Al will be 1.42hours.