How many grams of cobalt metal will be deposited when a solution of cobalt $(II)$ chloride is electrolyzed with a current of $10 \ A$ for $109$ minutes? ($1 \ Faraday = 96,500 \ C$; Atomic mass of $Co = 59 \ u$)

The laws of electrolysis were proposed by

Consider the following reaction:
$MnO_4^- + 8H^{+} + 5e^- \rightarrow Mn^{2+} + 4H_2O$,$E^\circ = 1.51 \ V$
The quantity of electricity required in Faraday to reduce five moles of $MnO_4^-$ is ..... .

When a current of $2 \ A$ is passed through a molten salt of a metal for $5 \ hours$,$22.2 \ g$ of the metal (atomic mass $= 177$) is deposited at the cathode. What is the oxidation state of the metal in the molten salt?

How much charge in Coulombs is required for the oxidation of $1 \ mol$ of $H_2O$ to $O_2$?

The same quantity of electricity was passed through solutions of salts of elements $X$,$Y$,and $Z$ with atomic masses $7$,$27$,and $48$ respectively. The masses of $X$,$Y$,and $Z$ deposited were $2.1 \ g$,$2.7 \ g$,and $7.2 \ g$ respectively. The valencies of $X$,$Y$,and $Z$ respectively are: