Which of the following is not an example of disproportionation reaction?

4 C l O_{3}^{-} \to C l^{-} + 3 C l O_{4}^{-}

No worries! We‘ve got your back. Try BYJU‘S free classes today!

2 H_{2} O_{2} \to 2 H_{2} O + O_{2}

No worries! We‘ve got your back. Try BYJU‘S free classes today!

2 N O_{2} + 2 O H^{-} \to N O_{2}^{-} + N O_{3}^{-} + H_{2} O

No worries! We‘ve got your back. Try BYJU‘S free classes today!

T i C l_{4} + 2 M g \to T i + 2 M g C l_{2}

Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses

Open in App

Solution

The correct option is D $T i C l_{4} + 2 M g \to T i + 2 M g C l_{2}$
Disproportionation, sometimes called dismutation, is a redox reaction in which a compound of intermediate oxidation state converts to two different compounds, one of higher and one of lower oxidation states. Thus calculating the oxidation number of each central atom by using $H = + 1, O = - 2, C l = - 1$
A. $4 + 5 C l O_{3}^{-} \to - 1 C l^{-} + 3 + 7 C l O_{4}^{-}$
Its a disproportionation reaction
B. $2 H_{2}_{2} \to 2 H_{2} - 2 O +_{2}$
Its a disproportionation reaction
C. $2 + 4 N O_{2} + 2 O H^{-} \to + 3 N O_{2}^{-} + + 5 N O_{3}^{-} + H_{2} O$
Its a disproportionation reaction
D. $+ 4 T i C l_{4} + 2 0 M g \to 0 T i + 2 + 2 M g C l_{2}$
Its not a disproportionation reaction but its a displacement reaction.

Suggest Corrections

Similar questions

T i C l_{4} + 2 M g \to T i + 2 M g C l_{2}

2 H_{2} O_{2} \to 2 H_{2} O + O_{2}

Metals as reducing agents

(a)Krolls process for titanium
$T i {C l}_{4} + 2 M g ⟶ 2 M g {C l}_{2} + T i$

(b)Gold Schmidt alumino thermite process?

2 N_{2} O_{5} (g) \to 4 N O_{2} (g) + O_{2} (g)

N_{2} O_{5}_{a} N O_{2} + N O_{3}

N O_{3} + N O_{2}_{- a} N_{2} O_{5}

N O_{2} + N O_{3}_{b} N O_{2} + O_{2} + N O

N O + N O_{3}_{c} 2 N O_{2}

2 N_{2} O_{5} ⟶ 4 N O_{2} + O_{2}

N_{2} O_{5} ⇌ N O_{2} + N O_{3}

N O_{2} + N O_{3} ⟶ N O + N O_{2} + O_{2}

N O + N O_{3} ⟶ 2 N O_{2}

Join BYJU'S Learning Program