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

Aluminum oxide is electrolyzed at $1000^\circ C$ to produce aluminum metal. The cathode reaction is $Al^{3+} + 3e^- \rightarrow Al$. What quantity of electricity is required to produce $5.12 \ kg$ of aluminum metal? (Given: $1 \ Faraday = 96500 \ C$)

How many Faraday of electricity is required to deposit $0.8 \ g$ of calcium at cathode by the electrolysis of $CaCl_2$ (in $F$)?

If in a voltaic cell $5 \ g$ of zinc is consumed,then how many ampere-hours are produced? (Given that the $E.C.E.$ of $Zn$ is $3.387 \times 10^{-7} \ kg/C$)

The $SI$ unit of electrochemical equivalent is

When a certain amount of electricity is passed through a solution of $Al^{3+}$,$4.5 \ g$ of aluminum (atomic mass $27 \ amu$) is deposited at the cathode. If the same amount of electricity is passed through $H^{+}$ ions,what volume of hydrogen (in $L$) is produced at $STP$?