The amount of copper metal deposited at cathode on passing electric current of $500 \ mA$ for $20 \ min$ in cupric chloride solution is ............ $g$

$A$ dilute solution of sulphuric acid is electrolysed using a current of $0.10 \ A$ for $2 \ hours$ to produce hydrogen and oxygen gas. The total volume of gases produced at $STP$ is $...... \ cm^3$. (Nearest integer) $[$ Given : Faraday constant $F = 96500 \ C \ mol^{-1}$ at $STP$,molar volume of an ideal gas is $22.7 \ L \ mol^{-1} ]$

Calculate the amount of electricity required to convert $1.1 \ mol$ of $Cr_2O_7^{2-}$ to $Cr^{3+}$ in acidic medium.

Two electrolytic cells,one containing acidified ferrous chloride $(FeCl_2)$ and the other containing acidic ferric chloride $(FeCl_3)$,are connected in series. When an electric current is passed through the cells,what is the ratio of iron deposited at the cathodes in the two cells?

How many electrons are involved in the reaction when $0.40 \ F$ of electricity is passed through an electrolytic solution?

If current $(I)$ of an electrolytic cell is doubled and time $(t)$ for electrolysis is halved,then the $\frac{\text{mass}}{\text{eq. wt.}}$ ratio becomes :-