Question

The second reaction in the formation of sulfuric acid occurs slowly. 2 upper S upper O subscript 2 (g) plus upper O subscript 2 (g) right arrow 2 upper S upper O subscript 3 (g). NO2 is added to the reaction to speed it up. In which form would this substance be a homogeneous catalyst for this reaction?

Answer 1

Answer:

Overall, the formation of sulfuric acid occurs as further:

1. $S + O_{2}$ ⇒ $SO_{2}$ - sulfur containing compound gets oxidized

2. $2SO_{2} + O_{2}$ ⇒ $2SO_{3}$ - sulfur dioxide oxidizing to sulfur trioxide

3. $SO_{3} + H_{2}O$ ⇒ $H_{2}SO_{4}$ - sulfur trioxide further reacts with water

$NO_{2}$ enters the cycle after the first step as a gas. It oxidises the sulfur dioxide, resulting in sulfur trioxide, and itself becomes nitrogen monoxide. However, due to the oxygen in the air. it gets oxidised again and becomes readily available to oxidise another molecule of sulfur dioxide. This process repeats and repeats until all are converted.

All reagents in equations 1 and 2 are in gaseous state!

In the 3rd equation, the water is liquid and sulfuric acid itself is aqueous.

Answer 2

Answer:NO2 is added in the reaction in the form of a gas.

Explanation:

Homogenous catalysts are catalysts which exists in the same form as the reactants and since the reactants are gaseous in nature i.e SO2 and O2, so the catalyst that is used is in gaseous form too.