The compound AgF₂ (unstable) acts as a/ an:

1. Oxidising agent.

2. Reducing agent.

3. Both oxidising and reducing agent.

4. Neither oxidising and reducing agent.

Which of the following hydrohalic acids acts as the best reducing agent?

$1.<mspace\; width="1em"></mspace>\mathrm{HCl}$
$2.<mspace\; width="1em"></mspace>\mathrm{HBr}$
$3.<mspace\; width="1em"></mspace>\mathrm{HI}$
$4.<mspace\; width="1em"></mspace>\mathrm{HF}$

From the following, identify the reaction having the top position in the EMF series (standard reduction potential) according to their electrode potential at 298 K.

Standard reduction potentials of the half-reactions are given below: 

$F_{2\left(g\right)}$ $+$ $2e^{-}\to 2{F^{-}}_{\left(aq\right)}$ $;$ $E°$ $=+2.85$ $V$ $$

$C{l}_{2\left(g\right)}$ $+$ $2e^{-}\to 2{C{l}^{-}}_{\left(aq\right)}$ $;$ $E°$ $=+1.36$ $V$ $$

$B{r}_{2\left(g\right)}$ $+$ $2e^{-}\to 2{B{r}^{-}}_{\left(aq\right)}$ $;$ $E°$ $=+1.06$ $V$ $$

$I_{2\left(g\right)}$ $+$ $e^{-}\to 2{I^{-}}_{\left(aq\right)}$ $;$ $E°$ $=+0.53$ $V$ $$

The strongest oxidizing and reducing agents, respectively, are: 

1. $B{r}_2$ and $C{l}^{-}$

2. $C{l}_2$ and $B{r}^{-}$

3. $C{l}_2$ and $I_2$

4. $F_2$ and $l^{-}$

A solution contains Fe²⁺, Fe³⁺ and I^– ions. This solution was treated with iodine at 35^°C. E° for Fe³⁺/Fe²⁺ is +0.77 V and E° for I₂/2I^– = 0.536 V.
The favourable redox reaction is:

1. Fe²⁺ will be oxidized to Fe³⁺.

2. I₂ will be reduced to I^–.

3. There will be no redox reaction.

4. I^– will be oxidized to I₂.

Given below are two statements: 

Identify the disproportionation reaction among the following:

1. ${\mathrm{CH}}_4+2{\mathrm{O}}_{\mathrm{2<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>}}\to \hspace{0.17em}{\mathrm{CO}}_2+2{\mathrm{H}}_2\mathrm{O}$

2. ${\mathrm{CH}}_4+4{\mathrm{Cl}}_{\mathrm{2<mspace\; width="1em"></mspace>}}\to \hspace{0.17em}{\mathrm{CCl}}_4+4\mathrm{HCl}$

3. $2{\mathrm{F}}_2+2{\mathrm{OH}}^{-\hspace{0.17em}}\to \hspace{0.17em}2{\mathrm{F}}^{-}+{\mathrm{OF}}_2+{\mathrm{H}}_2\mathrm{O}$

4. $2{\mathrm{NO}}_2+2{\mathrm{OH}}^{-\hspace{0.17em}}\to \hspace{0.17em}{\mathrm{NO}}_2^{-}+{\mathrm{NO}}_3^{-}+{\mathrm{H}}_2\mathrm{O}$

Which of the following arrangements represents the increasing oxidation number of the central atom?

1. ${\mathrm{CrO}}_2^{-},$ ${\mathrm{ClO}}_3^{-},$ ${\mathrm{CrO}}_4^{2-},$ ${\mathrm{MnO}}_4^{-}$

2. ${\mathrm{ClO}}_3^{-},$ ${\mathrm{CrO}}_4^{2-},$ ${\mathrm{MnO}}_4^{-},$ ${\mathrm{CrO}}_2^{-}$

3. ${\mathrm{CrO}}_2^{-},$ ${\mathrm{ClO}}_3^{-},$ ${\mathrm{MnO}}_4^{-},$ ${\mathrm{CrO}}_4^{2-}$

4. ${\mathrm{CrO}}_4^{2-},$ ${\mathrm{MnO}}_4^{-},$ ${\mathrm{CrO}}_2^{-},$ ${\mathrm{ClO}}_3^{-}$

Which of the following statement regarding the rules to calculate the oxidation number is incorrect?