On electrolysis of dilute sulphuric acid using Platinum $(Pt)$ electrodes,the product obtained at the anode will be:

On electrolysis,$1 \ mole$ of aluminium will be deposited from its molten salt by

If a current of $0.5 \ A$ flows through a metallic wire for $2 \ hours$,then how many electrons would flow through the wire?

Given below are two statements $:$
$1 \ M$ aqueous solution of each of $Cu(NO_3)_2, AgNO_3, Hg_2(NO_3)_2$ and $Mg(NO_3)_2$ are electrolysed using inert electrodes.
Given $: E_{Ag^{+}/Ag}^{\theta} = 0.80 \ V, E_{Hg_2^{2+}/Hg}^{\theta} = 0.79 \ V, E_{Cu^{2+}/Cu}^{\theta} = 0.24 \ V$ and $E_{Mg^{2+}/Mg}^{\theta} = -2.37 \ V$.
Statement $(I) :$ With increasing voltage,the sequence of deposition of metals on the cathode will be $Ag, Hg$ and $Cu$.
Statement $(II) :$ Magnesium will not be deposited at cathode instead oxygen gas will be evolved at the cathode.
In the light of the above statement,choose the most appropriate answer from the options given below.

Which of the following compounds is formed when electrolysis of brine solution takes place?

Products of electrolysis depend upon which factors? Justify with suitable examples.