In which one of the following sets all species show disproportionation reaction?

Question

In which one of the following sets all species show disproportionation reaction? (A) ClO 2-, F 2, MnO 4-and Cr 2 O 72- (B) Cr 2 O 72-, MnO 4-, ClO 2-and Cl 2 (C) MnO 4-, ClO 2-, Cl 2 and Mn 3+ (D) Cr 2 O 72-, MnO 4- ClO 2- text andCl 2

Tardigrade Admin · Accepted Answer

Disproportionation reactions are a special type of redox reactions. One of the reactants in a disproportionation reaction always contains an element that can exist in at least three oxidation states. The element of reacting species is in intermediate oxidation state and simultaneously gets oxidised and reduced MnO 4-do not shows disproportionation reaction.

Q. In which one of the following sets all species show disproportionation reaction?

$Cl O_{2}^{-}, F_{2}, M n O_{4}^{-}$ and $C r_{2} O_{7}^{2 -}$

$C r_{2} O_{7}^{2 -}, M n O_{4}^{-}, Cl O_{2}^{-}$ and $C l_{2}$

$M n O_{4}^{-}, Cl O_{2}^{-}, C l_{2}$ and $M n^{3 +}$

$C r_{2} O_{7}^{2 -}, M n O_{4}^{-} Cl O_{2}^{-} andCl_{2}$

Q. In which one of the following sets all species show disproportionation reaction?

ClO2−​,F2​,MnO4−​and Cr2​O72−​

Cr2​O72−​,MnO4−​,ClO2−​and Cl2​

MnO4−​,ClO2−​,Cl2​ and Mn3+

Cr2​O72−​,MnO4−​ClO2−​andCl 2​

$Cl O_{2}^{-}, F_{2}, M n O_{4}^{-}$ and $C r_{2} O_{7}^{2 -}$

$C r_{2} O_{7}^{2 -}, M n O_{4}^{-}, Cl O_{2}^{-}$ and $C l_{2}$

$M n O_{4}^{-}, Cl O_{2}^{-}, C l_{2}$ and $M n^{3 +}$

$C r_{2} O_{7}^{2 -}, M n O_{4}^{-} Cl O_{2}^{-} andCl_{2}$