Question

How does Ozone react with the following?
i) \[PbS\]
ii) ${C_2}{H_4}$
iii) $Ag$
iv) $Hg$

Answer 1

Hint: Ozone is one of the strongest oxidizing agents known, much stronger than ${O_2}$ . So when ozone reacts with any of the given compounds, it gives an oxidized product. Hence, calculate the oxidation states of the given compounds and accordingly the oxidized products.

Complete step-by-step answer:i) Firstly, let us find the oxidation state of Lead in $PbS$
We know that Sulfur’s oxidation state is $ - 2$ so the oxidation state of Lead would be $ + 2$
When Ozone reacts with Lead sulphide, it oxidizes it to lead sulphate. We can write this reaction as follows.
$PbS + 4{O_3} \to PbS{O_4} + 4{O_2}$
ii) Similarly, we can find the oxidation state of Carbon in ${C_2}{H_4}$ and the oxidation state is $ - 2$
When ozone reacts with ${C_2}{H_4}$ , it breaks the $C = C$ bond to form two moles of Formaldehyde. We write this reaction as follows.
${C_2}{H_4} + 2{O_3} \to 2HCHO + 2{O_2}$
iii) We do the same for $Ag$ and since Silver is not bonded to any other atoms and has zero charge on it, its oxidation state would be zero.
Ozone reacts with Silver to form Silver oxide. We can write this reaction as follows.
$2Ag + {O_3} \to A{g_2}O + {O_2}$
iv) Similarly, since $Hg$ is not bonded and has no charge on it, oxidation state will be zero.
When Ozone reacts with Mercury, it oxidizes it to Mercurous oxide. We can write this reaction as follows.
 $2Hg + {O_3} \to H{g_2}O + {O_2}$

Note: The given compound Ozone is a strong oxidizing agent. It oxidizes Lead sulphide to Lead sulphate. It breaks the bonds between ethane to form two moles of Formaldehyde. It oxidizes Silver and Mercury to Silver oxide and Mercurous oxide respectively.