The weight of silver $(at. \ wt. = 108)$ displaced by a quantity of electricity which displaces $5600 \ mL$ of $O_2$ at $STP$ will be ............ $g.$

For the given reaction how much quantity of electricity in Coulomb is required? $\frac{2}{3} Al_2O_3 \rightarrow \frac{4}{3} Al + O_2$

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: $1 \ Faraday = 96500 \ C$)

In the electrolysis of an aqueous $NiI_2$ solution using $Ni$ electrodes,what happens to the mass of the cathode upon passing $1$ equivalent of charge? (Given: atomic mass of $Ni = 59$)

Consider the reaction: $Cr_{2}O_{7}^{2-} + 14H^{+} + 6e^{-} \rightarrow 2Cr^{3+} + 7H_{2}O$. What is the quantity of electricity in coulombs needed to reduce $1 \ mol$ of $Cr_{2}O_{7}^{2-}$?

$96500 \ C$ of electric charge liberates how many grams of $Cu$ from $CuSO_4$ solution?