Which of the following is disproportionation reaction?

Question

Which of the following is disproportionation reaction? (A) CH 4+2 O 2 longrightarrow CO 2+2 H 2 O (B) CH 4+4 Cl 2 longrightarrow CCl 4+4 HCl (C) 2 F 2+2 OH - longrightarrow 2 F -+ OF 2+ H 2 O (D) 2 NO 2+2 OH - longrightarrow NO 2-+ NO 3-+ H 2 O

Tardigrade Admin · Accepted Answer

Reactions in which the same substance is oxidised as well as reduced are called disproportionation reaction.

Thus, in the reaction of

N O_{2}

and

O H^{-}, N

is both oxidised as well as reduced. Hence, the oxidation number increases from

+ 4

in

N O_{2}

to

+ 5

in

N O_{3}^{-}

and decreases from

+ 4

in

N O_{2}

to

+ 3

in

N O_{2}^{-}

.

Q. Which of the following is disproportionation reaction?

$C H_{4} + 2 O_{2} ⟶ C O_{2} + 2 H_{2} O$

$C H_{4} + 4 C l_{2} ⟶ CC l_{4} + 4 H Cl$

$2 F_{2} + 2 O H^{-} ⟶ 2 F^{-} + O F_{2} + H_{2} O$

$2 N O_{2} + 2 O H^{-} ⟶ N O_{2}^{-} + N O_{3}^{-} + H_{2} O$

Q. Which of the following is disproportionation reaction?

CH4​+2O2​⟶CO2​+2H2​O

CH4​+4Cl2​⟶CCl4​+4HCl

2F2​+2OH−⟶2F−+OF2​+H2​O

2NO2​+2OH−⟶NO2−​+NO3−​+H2​O

$C H_{4} + 2 O_{2} ⟶ C O_{2} + 2 H_{2} O$

$C H_{4} + 4 C l_{2} ⟶ CC l_{4} + 4 H Cl$

$2 F_{2} + 2 O H^{-} ⟶ 2 F^{-} + O F_{2} + H_{2} O$

$2 N O_{2} + 2 O H^{-} ⟶ N O_{2}^{-} + N O_{3}^{-} + H_{2} O$