How many electrons would be required to deposit 6.35 gm of copper at the cathode during the electrolysis of an aqueous solution of copper sulphate?

According to the reaction: Cu2+(aq) + 2e- → Cu(s)
We require 2 moles of electrons or 2NA electrons to deposit 1 mol or 63.5 g of Cu.
For 6.35 g, we require (2NA/63.5) * 6.35 = 2NA/10 = NA/5 electrons.
Hence, the number of electrons required to deposit 6.35 gm of copper = NA/5 electrons.