Question

A current of 9.65 ampere is drawn from a daniell cell for exactly one hour its molar masses of copper and zinc for 63.5 gram per mole and 65.4 gram per mole respectively the loss in mass at anode and weight and mass at cathode respectively are

Answer 1

Answer : 11.77g,11.43g
11.77
g
,
11.43
g
The reaction occurring in Daniell cell is Zn+Cu2+→Zn2++Cu
Z
n
+
C
u
2
+
→
Z
n
2
+
+
C
u
Zinc is lost at anode and Cu is deposited at cathode.
Amount of current withdrawn is (9.65A)(60×60s)/(96500Cmol−1)
(
9.65
A
)
(
60
×
60
s
)
/
(
96500
C
m
o
l
−
1
)
,which is 0.36mol.Since two electrons are involved in the reduction and oxidation reactions,0.18mol of zn is lost at anode and 0.18mol of Cu is deposited at cathode.The masses are 11.77g and 11.43g for Zn and Cu,respectively.

Answer 2

Answer:

The answer would be 11.77g and 11.43

Explanation:

We will split the redox reaction into its half cell reactions ...Then with Faradays law we will solve it...m=ZIT,