Identify the disproportionation reaction among the following:

1. ${\mathrm{CH}}_4+2{\mathrm{O}}_{\mathrm{2 }}\to {\mathrm{CO}}_2+2{\mathrm{H}}_2\mathrm{O}$

2. ${\mathrm{CH}}_4+4{\mathrm{Cl}}_{\mathrm{2 }}\to {\mathrm{CCl}}_4+4\mathrm{HCl}$

3. $2{\mathrm{F}}_2+2{\mathrm{OH}}^{- }\to 2{\mathrm{F}}^{-}+{\mathrm{OF}}_2+{\mathrm{H}}_2\mathrm{O}$

4. $2{\mathrm{NO}}_2+2{\mathrm{OH}}^{- }\to {\mathrm{NO}}_2^{-}+{\mathrm{NO}}_3^{-}+{\mathrm{H}}_2\mathrm{O}$

Given below are two statements: 

The oxidising agent and reducing agent in the given reaction are

$5{\mathrm{P}}_{4\left(\mathrm{s}\right)}+12{\mathrm{H}}_2{\mathrm{O}}_{\left(\mathrm{l}\right)}+12{{\mathrm{HO}}^{-}}_{\left(\mathrm{aq}\right)}\to$
$8{\mathrm{PH}}_{3\left(\mathrm{g}\right)}+12{{\mathrm{HPO}}_2^{-}}_{\left(\mathrm{aq}\right)}$

1. Oxidising agent = ${\mathrm{P}}_4$; Reducing agent = ${\mathrm{P}}_4$

2. Oxidising agent = ${\mathrm{P}}_4$; Reducing agent = ${\mathrm{H}}_2\mathrm{O}$

3. Oxidising agent = ${\mathrm{H}}_2\mathrm{O}$; Reducing agent = ${\mathrm{P}}_4$

4. None of the above

Given below are two statements: 

The set of metals that can show disproportionation reaction is -

The number of moles of MnO^-₄ required to oxidise one mole of ferrous oxalate completely in an acidic medium is-

1. 0.6 mole

2. 0.4 mole

3. 7.5 moles

4. 0.2 mole