How many grams of cobalt metal will be deposited when a solution of cobalt $(II)$ chloride is electrolyzed with a current of $10 \ A$ for $109$ minutes? ($1 \ Faraday = 96,500 \ C$; Atomic mass of $Co = 59 \ u$)

For how much time,$10 \ A$ electric current should be passed through a dilute aqueous $NiSO_4$ solution during electrolysis using inert electrode,in order to get $5.85 \ g$ Nickel (in $s$)?
[At. mass of $Ni = 58.5 \ g/mol$]

When two electrolytic cells containing $NiSO_4$ and $CuSO_4$ solutions are connected in series and an electric current is passed,$1.6 \ g$ of $Cu$ is deposited on the electrode. How much $Ni$ metal is produced? If a cell containing $AgNO_3$ solution is connected instead of $NiSO_4$,how many grams of silver will be obtained? [Atomic mass: $Cu = 63.5 \ g/mol$,$Ni = 58.7 \ g/mol$,$Ag = 108 \ g/mol$]

The mass of copper deposited from a solution of $CuSO_4$ by passage of $5 \ A$ current for $965 \ s$ is ............ $g$ (Mol. wt. of Copper $= 63.5$)

An acidic solution of dichromate is electrolyzed for $8 \ min$ using $2 \ A$ current. As per the following equation: $Cr_{2}O_{7}^{2-} + 14H^{+} + 6e^{-} \rightarrow 2Cr^{3+} + 7H_{2}O$. The amount of $Cr^{3+}$ obtained was $0.104 \ g$. The efficiency of the process (in $\%$) is (Take: $F = 96000 \ C$,At. mass of chromium $= 52$)

The electric charge for electrode deposition of one equivalent of a substance is equal to