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

How many electrons would be required to deposit $6.35 \ g$ of copper at the cathode during the electrolysis of an aqueous solution of copper sulphate? (Atomic mass of copper $= 63.5 \ u$,$N_A =$ Avogadro's constant)

On passing $C$ ampere of electricity through an electrolyte solution for $t$ seconds,$m$ grams of metal are deposited on the cathode. The equivalent weight $E$ of the metal is:

How many atoms of calcium will be deposited at the cathode when a current of $25 \ mA$ is passed through a $CaCl_2$ solution for $60 \ s$?

$9.65 \ C$ of electric current is passed through fused anhydrous $MgCl_2$. The magnesium metal thus obtained is completely converted into a Grignard reagent. The number of moles of Grignard reagent obtained is

When $4.5 \, A$ current is passed through $1 \, L$ of $0.6 \, M$ $CuCl_2$ solution for $1.15 \, hour$,calculate the mass of $Cu$ and the change in concentration of the solution. $[Cu = 63.5 \, u]$