This question is about the industrial production of sulfur trioxide.
In the Contact process, sulfur trioxide (
SO3 SO_3 SO3) is produced from sulfur dioxide (
SO2 SO_2 SO2) and oxygen (
O2 O_2 O2).
During the process, unreacted sulfur dioxide and oxygen gases are recycled back into the reactor. Explain why these unreacted gases are recycled.
Which catalyst is used in this industrial reaction?
Describe the chemical test for oxygen gas. Give the result if oxygen gas is present.
- Test:
- Result:
The reaction of sulfur dioxide with oxygen is exothermic:
2SO2(g)+O2(g)→2SO3(g) 2\text{SO}_2(\text{g}) + \text{O}_2(\text{g}) \rightarrow 2\text{SO}_3(\text{g}) 2SO2(g)+O2(g)→2SO3(g)The reaction profile below represents this reaction when it is uncatalysed:
How would the reaction profile be different if a catalyst was used? Select one option:
- The final energy level of the products would be lower.
- The starting energy level of the reactants would be higher.
- The curve would reach a lower peak.
- The activation energy would be greater.
Sulfur trioxide is reacted with concentrated sulfuric acid and then diluted with water to produce more sulfuric acid. Suggest one major industrial use of sulfuric acid.