How many moles of electrons (how many Faradays of electricity) are required to reduce $1 \ mol$ of $MnO_4^-$ to $MnO_2$?

One gram of metal ion $M^{3+}$ is discharged by the passage of $1.81 \times 10^{23}$ electrons. What is the atomic weight of the metal?

If $5 \ A$ of current is passed for $193 \ s$ through a solution containing $Cu$ salt,$0.32 \ g$ of copper is deposited. What is the oxidation state of the $Cu$ in the salt?

$38.6 \ A$ of current is passed for $100 \ s$ through an aqueous $CuSO_4$ solution using platinum electrodes. The mass of copper deposited from the solution and the volume of gas liberated at $STP$ are respectively (molar mass of $Cu = 63.54 \ g \ mol^{-1}$)

According to Faraday's laws of electrolysis,the amount of decomposition is proportional to

When $1 \ F$ (Faraday) of electricity is passed through an aqueous solution of $CuSO_4$,the amount of $Cu$ deposited is: