Question

A solution of cuso4 is electrolysed for 10 minutes with a current of 3 amperes. What is the mass of copper deposited at the anode? (atomic mass of cu = 63 g)

Answer 1

Answer:

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Answer 2

0.59 g of copper is deposited at the cathode

Explanation:

According to mole concept:

1 mole of an atom contains $6.022\times 10^{23}$ number of particles.

We know that:

Charge on 1 electron = $1.6\times 10^{-19}C$

Charge on 1 mole of electrons = $1.6\times 10^{-19}\times 6.022\times 10^{23}=96500C$

I = current passed = 3 A

q = total charge =?

t = time required = 10 min = 600 sec    (1 min= 60 sec)

Putting values in above equation, we get:

$3A=\frac{q}{600s}\\\\q=1800C$

$CuSO_4\rightarrow Cu^{2+}+SO_4^{2-}$

At cathode : $Cu^{2+}+2e^-\rightarrow Cu$

$2\times 96500=193000C$ is required to deposit = 63 g of copper

1800C is required to deposit = $\frac{63}{193000}\times 1800=0.59g$ g of copper

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