Redox Reactions And Electrochemistry Question 494
Question: On passing a current of 1.0 ampere for 16 min and 5 sec through one litre solution of $ CuCl_2 $ , all copper of the solution was deposited at cathode. The strength of $ CuCl_2 $ solution was (Molar mass of Cu= 63.5; Faraday constant $ =96500Cmo{l^{-1}} $ )
Options:
A) 0.01 N
B) 0.01 M
C) 0.02 M
D) 0.2 N
Show Answer
Answer:
Correct Answer: A
Solution:
[a] By Faraday’s Ist law of electrolysis, $ \frac{W}{E}=\frac{Q}{96500} $ (where Q= it = charge of ion)
We know that no. of gram equivalent $ =\frac{W}{E}=\frac{it}{96500}=\frac{1\times 965}{96500}=\frac{1}{100} $ (where i = 1 A, $ t=16\times 60+5=965sec. $ )
Since, we know that Normality $ =\frac{No.of,gram,equivalent}{Volume( inlitre )}=\frac{\frac{1}{100}}{1}=0.01N $
BETA
