During the electrolysis of aqueous $NaCl$ solution, the product formed at the cathode is?

Which of the following reactions occurs at the anode when the electrolysis of an aqueous $CuSO_4$ solution is carried out using copper electrodes?

When electric current is passed through a cell having an electrolyte,the positive ions move towards the cathode and the negative ions towards the anode. If the cathode is pulled out of the solution,what happens to the ions?

The number of electrons involved in the reaction when $1 \ Faraday$ of electricity is passed through an electrolytic solution is?

When an aqueous solution of $CuCl_2$ is electrolysed using $Pt$ inert electrodes,the reactions at the cathode and anode respectively are:

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.