Which of the following is disproportionation reaction?
Which of the following is disproportionation reaction?
The correct option is C
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 a t least three oxidation states. The element in the reacting substance is in an intermediate oxidation state, and both lower and higher oxidation states of that element are formed among the products.
Now let us look at the decomposition of H2O2 (Hydrogen peroxide) to H2O and O2. In H2O2 oxidation state of O is -1. Now let us assess the oxidation state of Oxygen atoms in the products. For the dioxygen O2 molecule, since the product is in the elemental state, the oxidation state is 0. For H2O, Oxygen atom has a -2 oxidation state.
Let us depict the reaction with the relevant oxidation numbers:
2+1H2−1O2(aq)⟶2+1H2−2O(l)+0O2(g)
As you can see, the same element is both oxidized and reduced into at least two components such that the oxidation state of the element in the reactant is intermediate to that of the oxidation states of the same element among the products.
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 a t least three oxidation states. The element in the reacting substance is in an intermediate oxidation state, and both lower and higher oxidation states of that element are formed among the products.
Now let us look at the decomposition of H2O2 (Hydrogen peroxide) to H2O and O2. In H2O2 oxidation state of O is -1. Now let us assess the oxidation state of Oxygen atoms in the products. For the dioxygen O2 molecule, since the product is in the elemental state, the oxidation state is 0. For H2O, Oxygen atom has a -2 oxidation state.
Let us depict the reaction with the relevant oxidation numbers:
2+1H2−1O2(aq)⟶2+1H2−2O(l)+0O2(g)
As you can see, the same element is both oxidized and reduced into at least two components such that the oxidation state of the element in the reactant is intermediate to that of the oxidation states of the same element among the products.
