Solution Found!
The oxidation of SO2 is the key step in H2SO4 production:
Chapter 17, Problem 62P(choose chapter or problem)
The oxidation of \(\mathrm{SO}_{2}\) is the key step in H2SO4 production:
a) What qualitative combination of 𝑇 and 𝑃 maximizes \(\mathrm{SO}_{3}\) yield?
(b) How does addition of \(\mathrm{O}_{2}\) affect 𝑄? 𝐾?
(c) Why is catalysis used for this reaction?
Equation Transcription:
SO2
H2SO4
SO3
O2
Text Transcription:
SO_2
H_2SO_4
SO_3
O_2
Questions & Answers
QUESTION:
The oxidation of \(\mathrm{SO}_{2}\) is the key step in H2SO4 production:
a) What qualitative combination of 𝑇 and 𝑃 maximizes \(\mathrm{SO}_{3}\) yield?
(b) How does addition of \(\mathrm{O}_{2}\) affect 𝑄? 𝐾?
(c) Why is catalysis used for this reaction?
Equation Transcription:
SO2
H2SO4
SO3
O2
Text Transcription:
SO_2
H_2SO_4
SO_3
O_2
ANSWER:
Solution 62P:
Step 1:
According to Le Chatelier's principle “only temperature changes alter the equilibrium constant.”
- A temperature rise will increase the equilibrium constant for a system with a positive H°rxn.
- A temperature rise will decrease the equilibrium constant for a system with a negative H°rxn.
The change in the pressure of the container changes the concentration of the gaseous reactants and products which result in shift in equilibrium depending upon the number of moles of gaseous reactants and gaseous products.
- If the number of moles of gaseous reactants and gaseous products is same, the change in pressure has no effect.
- If the pressure decreases, the reaction shifts that side which has more number of moles.
- If the pressure increases, the reaction shifts that side which has less number of moles formation.