Question

How long it will take for the deposition of 0.2g of copper when silver nitrate solution is electrolysed using 0.5 ampere of current (Mol mass of Cu =63u)​

Answer 1

Given:

Mass of copper deposited = 0.2 g

Current passed = 0.5 Ampere

Molar mass of Cu = 63 u

To find:

Time taken for copper deposition

Solution:

According to Faraday's law of electrolysis we can calculate the time taken for deposition. Formula used is as follows,

              $w = Zit$

or,          $w = \frac{E}{F} it$

here, w = weight of copper which gets deposited

        E = equivalent weight

        F = Faraday's constant

        i = current passed

         t = time taken

It is given,  w = 0.2 g

                  E = 63 u

                  F = 96500 Cmol⁻¹

                  i = 0.5 Ampere

by substituting all the values, we get

              $0.2 = \frac{63}{96500} \times 0.5 \times t$

               $t = \frac{0.2 \times 96500 }{63 \times 0.5}$

               t = 612.69 s

Therefore, time taken for copper to get deposited is 612.69 s.