How much volume of oxygen at $STP$ will be liberated by $2$ $ampere$ flowing for $3$ $minutes$ and $13$ $seconds$ through acidified water? (in $cc$)

Potassium chlorate is prepared by the electrolysis of $KCl$ in basic solution:
$6 OH^{-} + Cl^{-} \rightarrow ClO_{3}^{-} + 3 H_{2}O + 6 e^{-}$
If only $60\%$ of the current is utilized in the reaction,the time (rounded to the nearest hour) required to produce $10 \ g$ of $KClO_{3}$ using a current of $2 \ A$ is:
(Given: $F = 96,500 \ C \ mol^{-1}$,molar mass of $KClO_{3} = 122 \ g \ mol^{-1}$)

Electrolysis of $600 \ mL$ aqueous solution of $NaCl$ for $5 \ min$ changes the $pH$ of the solution to $12$. The current in Amperes used for the given electrolysis is $...........$. $(Nearest \ integer)$.

$A$ 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 $22.7 \ L \ mol^{-1} ]$

$10 \, A$ current is passed through $CuSO_4$ solution for $193 \, \text{minutes}$ at $1 \, \text{bar}$ pressure and $300 \, K$ temperature. If the cell has $80 \%$ efficiency,find the weight of $Cu$ deposited and the volume of $O_2$ evolved. $[Cu = 63.5 \, u, R = 0.08314 \, \text{L bar K}^{-1} \text{mol}^{-1}]$

For electroplating,$1.5 \ A$ current is passed for $250 \ s$ through $250 \ mL$ of $0.15 \ M$ solution of $MSO_4$. Only $85 \ \%$ of the current was utilised for electrolysis. The molarity of $MSO_4$ solution after electrolysis is closest to $.......$ [Assume that the volume of the solution remained constant] (in $M$)