Electrolysis Questions

The electrochemical equivalent of a metal is $3.3\times 10^{-7}\text{kg}$ per coulomb. The mass of the metal liberated at the cathode when a $3\text{A}$ current is passed for $2\text{seconds}$ will be:

Two voltameters one of copper and another of silver, are joined in parallel. When a total charge $q$ flows through the voltameters, equal amount of metals are deposited. If the electrochemical equivalents of copper and silver are $z_1$ and $z_2$ respectively the charge which flows through the silver voltameter is:

The negative $\text{Zn}$ pole of a Daniell cell, sending a constant current through a circuit, decreases in mass by $0.13\text{g}$ in $30\text{minutes}$. If the electrochemical equivalent of $\text{Zn}$ and $\text{Cu}$ are $32.5$ and $31.5$ (arbitrary units or mass ratio) respectively, the increase in the mass of the positive $\text{Cu}$ pole in this time is: