Oxidation number

Given below are two statements.

Statement I: Iron (III) catalyst, acidified $\mathrm{K_2Cr_2O_7}$ and neutral $\mathrm{KMnO_4}$ have the ability to oxidise $\mathrm{I^-}$ to $\mathrm{I_2}$ independently.

Statement II: Manganate ion is paramagnetic in nature and involves $p\pi-p\pi$ bonding.

In the light of the above statements, choose the correct answer from the options given below.

In the titration of $\mathrm{KMnO_4}$ and oxalic acid in acidic medium, the change in oxidation number of carbon at the end point is ______

On reaction with stronger oxidizing agent like $\mathrm{KIO_4}$, hydrogen peroxide oxidizes with the evolution of $\mathrm{O_2}$. The oxidation number of I in $\mathrm{KIO_4}$ changes to ______.

In neutral or faintly alkaline medium, $\mathrm{KMnO_4}$ being a powerful oxidant can oxidize, thiosulphate almost quantitatively, to sulphate. In this reaction overall change in oxidation state of manganese will be :

The correct statement(s) related to oxoacids of phosphorous is(are)

Ozonolysis of $\ce{ClO2}$ produces an oxide of chlorine. The average oxidation state of chlorine in this oxide is ____.

(A) $\mathrm{HOCl+H_2O_2\to H_3O^++Cl^-+O_2}$

(B) $\mathrm{I_2+H_2O_2+2OH^-\to2I^-+2H_2O+O_2}$

Choose the correct option.

Choose the correct statement(s) among the following.

With reference to aqua regia, choose the correct option(s)

The order of the oxidation state of the phosphorus atom in $\ce{H3PO2}$, $\ce{H3PO4}$, $\ce{H3PO3}$, and $\ce{H4P2O6}$ is

Which of the following reactions is an example of a redox reaction ?

The pair of compounds having metals in their highest oxidation state is :

In which of the following reactions, hydrogen peroxide acts as an oxidizing agent ?

The number of P−OH bonds and the oxidation state of phosphorus atom in pyrophosphoric acid ($\ce{H4P2O7}$) respectively are :

The pair in which phosphorous atoms have a formal oxidation state of +3 is :

The non-metal that does not exhibit positive oxidation state is :

Choose the incorrect formula out of the four compounds for an element X below :

For the reaction:
$$\ce{I- + ClO3- + H2SO4 -> Cl- + HSO4- + I2}$$
The correct statement(s) in the balanced equation is/are:

Consider the following list of reagents:

Acidified $\ce{K2Cr2O7}$, alkaline $\ce{KMnO4}$, $\ce{CuSO4}$, $\ce{H2O2}$, $\ce{Cl2}$, $\ce{O3}$, $\ce{FeCl3}$, $\ce{HNO3}$ and $\ce{Na2S2O3}$.

The total number of reagents that can oxidise aqueous iodide to iodine is

Hydrogen peroxide in its reaction with $\ce{KIO4}$ and $\ce{NH2OH}$ respectively, is acting as a