Question

A solution of cuso4 is electrolysed for 10 minutes with a current of 1.5 ampere what is the mass of copper deposited at cathode

Answer 1

Answer :

• Mass of copper deposited = 0.296 g.

Step-by-step explanation :

Given that,

• Current = 1.5 amperes.
• Time = 10 min = 10 × 60s = 600 seconds.

Also,

• Molar mass of copper = 63.5 g/mol.

$\hrulefill$

The reaction occurring at the cathode is :-

$\rm{Cu^{2+}+2e^-\longrightarrow{}Cu}$

Also, as we know current and time, quantity of electricity passed :-

⇒ Current (amp) × Time (s)

⇒ 1.5 × 600

⇒ 900 C.

Thus, 2 F, i.e., 2 × 96500 C deposited Cu = 1 mol = 63.5 g.

∴ 900 C will deposit Cu :-

$\implies\rm{\dfrac{63.5}{2\times{}96500}\times{}900}$

$\implies\bold{0.296\:g.}$