Question

when one Faraday or 96500 coulombs of electricity is passed through sliver nitrate solution, 108 gms of silver are deposited. calculate the electrochemical equivalent of silver.​

Answer 1

Answer:

According to Faraday's Law of Electrolysis:-

W= nF

I×t×M

W= weight deposited

I= current F= Faraday's constant 96500

t= time M= Molar mass

n= number of electron

Given:-

It=96500 coulomb

Molar mass of Silver, M=108g/mol

n=1

W= 1×96500

96500×108

W=0.0108g

⇒W=10.8mg

Explanation:

According to Faraday's Law of Electrolysis:-

W=

nF

I×t×M

W= weight deposited

I= current F= Faraday's constant 96500

t= time M= Molar mass

n= number of electron

Given:-

It=9.65 coulomb

Molar mass of Silver, M=108g/mol n=1

W=

1×96500

9.65×108

W=0.0108g

⇒W=10.8mg

Answer 2

Given:

no. of coulombs passed = 96500C

mass deposited(silver) = 108 gm

To Find:

calculate the electrochemical equivalent of silver =?

Solution:

we know the expression for electrochemical equivalent,

The electrochemical equivalent of silver

= mass deposited/ no. of coulombs deposited

$=\dfrac{108}{96500}$

= 0.0011 g/C

= 0.111 mg/C

Thus, the electrochemical equivalent of silver is 0.111 mg/C