Question

In an electroplating process, copper (ionic charge +2e, atomic weight 63.6 g/mol) is deposited using a current of 10.0 A. What mass of copper is deposited in 10.0 minutes? Avogadro's number is 6.022 × 1023 molecules/mol and e = 1.60 × 10-19 C.

Answer 1

Answer : The mass of copper deposit is, 1.98 grams

Explanation :

First we have to calculate the charge.

Formula used :
`Q=I* t`

where,

Q = charge = ?

I = current = 10 A

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

Now put all the given values in this formula, we get

`Q=10A* 600s=6000C`

Now we have to calculate the number of atoms deposited.

As, 1 atom require charge to deposited =
`2* (1.6* 10^(-19))`

Number of atoms deposited =
`((6000))/(2*(1.6* 10^(-19)))=1.875* 10^(22)` atoms

Now we have to calculate the number of moles deposited.

Number of moles deposited =
`((1.875* 10^(22)))/((6.022* 10^(23)))=0.03113` moles

Now we have to calculate the mass of copper deposited.

1 mole of Copper has mass = 63.5 g

Mass of Copper Deposited =
`63.5* 0.03113 =1.98g`

Therefore, the mass of copper deposit is, 1.98 grams