The mass deposited at an electrode during electrolysis is directly proportional to which of the following?

Two Faraday of electricity is passed through a solution of $CuSO_4$. The mass of copper deposited at the cathode is ......... $g$. (at. mass of $Cu = 63.5 \ amu$)

For depositing $1 \ g$ of $Cu$ in a copper voltameter by passing $2 \ A$ of current,the time required will be (For copper $Z = 0.00033 \ g/C$)

The density and equivalent weight of a metal are $10.5\, g\, cm^{-3}$ and $100$,respectively. The time required for a current of $3\, A$ to deposit a $0.005\, mm$ thick layer of the same metal on an area of $80\, cm^2$ is closest to $....\, s$

If the total electricity required to deposit $1$ mole of a metal $M$ is equal to that of $10.7$ amperes of current for $10$ hours,the equivalent weight of the metal is (atomic weight $= M \ u$):

When an electric current is passed through a solution of $KCl$,$19.5 \ g$ of potassium (atomic mass $= 39$) is deposited. If the same amount of electric current is passed through a solution of $AlCl_3$,how many grams of aluminum will be liberated?