Given below are two statements: 

Assertion (A):	The decomposition of hydrogen peroxide to form water and oxygen is an example of a disproportionation reaction.
Reason (R):	The oxygen of peroxide is in –1 oxidation state and it is converted to zero oxidation state in O2 and –2 oxidation state in H2O.

1.	Both (A) and (R) are true and (R) is the correct explanation of (A).
2.	Both (A) and (R) are true but (R) is not the correct explanation of (A).
3.	(A) is true but (R) is false.
4.	(A) is false but (R) is true.

Using the standard electrode potentials of the redox couples given below, which of the following is the strongest oxidizing agent?

${\mathrm{E}}^{⊝} \mathrm{values}: {\mathrm{Fe}}^{3+}/{\mathrm{Fe}}^{2+}=+0.\mathrm{77\; V}$ 
${\mathrm{I}}_2\left(\mathrm{s}\right)/{\mathrm{I}}^{-}=+0.54 V$
${\mathrm{Cu}}^{2+}/\mathrm{Cu}=+0.\mathrm{34\; V}$
${\mathrm{Ag}}^{+}/\mathrm{Ag}=0.\mathrm{80\; V}$

1. Fe³⁺
2. I₂(s)
3. Cu²⁺
4. Ag⁺

${\mathrm{E}}^{\Theta }$ values of some redox couples are given below. On the basis of these values choose the correct option.

${\mathrm{E}}^{\mathrm{\Theta }} \mathrm{values}: {\mathrm{Br}}_2/{\mathrm{Br}}^{-}=+1.90$
${\mathrm{Ag}}^{+}/\mathrm{Ag}\left(\mathrm{s}\right)=+0.80$
${\mathrm{Cu}}^{2+}/\mathrm{Cu}\left(\mathrm{s}\right)=+0.34;$
${\mathrm{I}}_2\left(\mathrm{s}\right)/{\mathrm{I}}^{-}=+0.54$

In the reactions given below, thiosulphate reacts differently with iodine than with bromine.

$2{\mathrm{S}}_2{\mathrm{O}}_3^{2-}+{\mathrm{I}}_2\to {\mathrm{S}}_4{\mathrm{O}}_6^{2-}+2{\mathrm{I}}^{-}$

${\mathrm{S}}_2{\mathrm{O}}_3^{2-}+2{\mathrm{Br}}_2+5{\mathrm{H}}_2\mathrm{O}\to 2{\mathrm{SO}}_4^{2-}+2{\mathrm{Br}}^{-}+10{\mathrm{H}}^{+}$

Choose the statements among the following that best describe the above dual behaviour of thiosulphate.

The incorrect statement regarding the rule to find the oxidation number among the following is-

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

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

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: 

Given below are two statements: