Question

0.2864g of $Cu$ was deposited on passage of a current of 0.5 ampere for 30 minutes through a solution of copper sulphate. What is the electrochemical equivalent of copper?

Answer 1

Given that,

Weight of copper $=0.2864g$

Current $=0.5ampere$

Time $=30\mathrm{mint}$

Now we get

Quantity of charge passed

$\Rightarrow 0.5\times 30\times 60=900coulomb$

So, $900coulomb$ Deposit copper $=0.2864g$

We know that

$1faraday=96500coulomb$

Thus,

$96500$ coulomb deposit copper$=\frac{0.2864}{900}\times 96500=30.78g$

Hence, Equivalent mass of copper $=30.78g$