(a(i))[1]
Name the component X.
(a(ii))[1]
Suggest a suitable electrolyte for Y.
(b)[3]
During an experiment, a current of $0.200\,\text{A}$ flowed through the cell for $40.0\,\text{minutes}$. The mass of the silver cathode rose by $0.500\,\text{g}$. The electron has a charge of $-1.60 \times 10^{-19}\,\text{C}$. Calculate: • number of moles of silver deposited on the cathode • number of coulombs of charge passed • number of electrons passed • number of electrons needed to deposit $1\,\text{mol}$ of silver at the cathode.