wiz-icon
MyQuestionIcon
MyQuestionIcon
1
You visited us 1 times! Enjoying our articles? Unlock Full Access!
Question

During the electrolysis of molten sodium chloride, the time required to produce 0.10 mol of chlorine gas using a current of 3 amperes is approximately:

A
220 minutes
No worries! We‘ve got your back. Try BYJU‘S free classes today!
B
330 minutes
No worries! We‘ve got your back. Try BYJU‘S free classes today!
C
55 minutes
No worries! We‘ve got your back. Try BYJU‘S free classes today!
D
110 minutes
Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses
Open in App
Solution

Given

Equivalent weight of chlorine = Molecularweightofchlorinenfactor=35.51=35.5g

Electric current passed = 3 amperes

Number of moles = 0.10 mole

Weight of 2 chlorine ions = Numberofmoles×Molecularmass

Step 1:

At Cathode: 2H2O+2eH2+2OH

At Anode: 2ClCl2+2e

Step 2:

Applying Faraday's Law

W=E×It96500

W is the weight of substance deposited

E is the equivalent weight of the substance

I is the electric current passed

t is the time in sec

0.1×71=35.5×t(sec)×396500

t=6433sec=107.2min110min
Hence, option (D) is correct.


flag
Suggest Corrections
thumbs-up
146
Join BYJU'S Learning Program
similar_icon
Related Videos
thumbnail
lock
Faraday's Laws
CHEMISTRY
Watch in App
Join BYJU'S Learning Program
CrossIcon