Which of the following represents disproportionation reaction-
(a) 2Cu+ ---> Cu2+ +Cu
(B)3I2 ---> 5I- + I+5
(d) 2HCHO --OH--> HCOO- + CH3OH
(c)H2o + Cl2 + ClO- + 2H+
Dear Student,
Disproportionation reactions are a special type of redox reactions. In a disproportionation reaction an element in one oxidation state is simultaneously oxidised and reduced. One of the reacting substances in a disproportionation reaction always contains an element that can exist in at least three oxidation states. The element in the form of reacting substance is in the intermediate oxidation state; and both higher and lower oxidation states of that element are formed in the reaction.
disproportionation reaction : a, b and d
2 Cu+ (aq) → Cu2+(aq) + Cu(s)
3I2 ---> 5I- + I+5
2HCHO + OH------------>HCOO-+CH3OH
Regards
Disproportionation reactions are a special type of redox reactions. In a disproportionation reaction an element in one oxidation state is simultaneously oxidised and reduced. One of the reacting substances in a disproportionation reaction always contains an element that can exist in at least three oxidation states. The element in the form of reacting substance is in the intermediate oxidation state; and both higher and lower oxidation states of that element are formed in the reaction.
disproportionation reaction : a, b and d
2 Cu+ (aq) → Cu2+(aq) + Cu(s)
3I2 ---> 5I- + I+5
2HCHO + OH------------>HCOO-+CH3OH
Regards