Among the following hydrohalic compounds, the best reductant is -

$1. \mathrm{HCl}$
$2. \mathrm{HBr}$
$3. \mathrm{HI}$
$4. \mathrm{HF}$

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.

1. Mg²⁺+ 2e^–$\to$Mg_(s)
2. Fe²⁺ + 2e^–$\to$ Fe_(s)
3. Au³⁺+ 3e^–$\to$Au_(s)
4. K⁺+ le ^–$\to$K_(s)

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.

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: 

Given below are two statements: 

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

The largest oxidation number exhibited by an element depends on its electronic configuration. With which of the following electronic configurations will the element exhibit the largest oxidation number?

1. 3d¹4s²

2. 3d³4s²

3. 3d⁵4s¹

4. 3d⁵4s²

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