Question

All the three oxygen atoms of ozone are utilized in the oxidation of:
A.${K_2}Mn{O_4}$ solution
B.Moist ${I_2}$
C.Acidified $FeS{O_4}$ solution
D.Acidified $SnC{l_2}$ solution

Answer 1

Oxidation can be most simply said as the process of addition of oxygen to any compound. In other terms, it involves the removal of electrons from the atom, molecule or ion being oxidized. As a result, there is an increase in the oxidation number taking place. Ozone will react completely with a compound which is a very good reducing agent.

Complete step by step answer:
Ozone is a good oxidizing agent with the chemical formula ${O_3}$. It breaks into nascent oxygen and dioxygen molecules and thus oxidizes a variety of compounds.
When potassium manganate, ${K_2}Mn{O_4}$, is reacted with ozone, it is oxidized to potassium permanganate, $KMn{O_4}$, using up one oxygen atom from ozone and oxygen gas is obtained as a byproduct.
When moist iodine is reacted with ozone, iodic acid is formed. 5 moles of ozone are used up and one oxygen atom is used from each ozone atom.
Ozone in reaction with acidified ferrous sulphate oxidizes the latter to ferric sulphate and one oxygen atom is used up and oxygen gas is released as a byproduct.
$SnC{l_2}$ is a good reducing agent and on reaction with ozone uses up all three oxygen atoms and forms stannic chloride, $SnC{l_4}$. ${O_2}$ is not evolved in this reaction.

Hence, the correct answer is D.

Note:
Ozone is a triatomic allotropic form of oxygen. It has the chemical formula ${O_3}$. It is formed when the ultra violet rays of sunlight come in contact with Dioxygen molecules. The ultra violet rays split the oxygen molecule into two oxygen free radicals. These free radicals further react with the dioxygen molecules resulting in the formation of ozone. Ozone is produced naturally by this reaction in the stratosphere and the troposphere which are the upper and lower atmospheres respectively.