In the reaction, 2SO2 (g) + O2 ⇌ 2SO3 (g) ∆H= -X cal most favorable conditions of temperature and pressure for a greater yield of SO3 are:
Correct answer: D. Low temperature and high pressure
- A. Low temperature and low pressure
- B. High temperature and low pressure
- C. High temperature and high pressure
- D. Low temperature and high pressure
Explanation
The correct answer is Option D: Low temperature and high pressure. According to Le Chatelier's principle, increasing the pressure will shift the equilibrium towards the side with fewer gas moles, which is the product side (2SO3), resulting in a higher yield of SO3. Additionally, since the reaction is exothermic (∆H = -X cal), lowering the temperature will also favor the forward reaction, further increasing the yield of SO3. The combination of low temperature and high pressure is thus the most favorable for maximizing the production of SO3. Other options either incorrectly prioritize temperature and pressure conditions that do not favor the formation of SO3 or apply an incorrect understanding of Le Chatelier's principle.
Report an error
The more specific you are, the faster it gets fixed. A source beats an opinion.
Prefer email? [email protected]
About Chemical Equilibrium
Reversible reactions reach dynamic equilibrium when forward and reverse rates become equal, and Le Chatelier's principle predicts the effect of changing concentration, pressure or temperature. The chapter also covers solubility product, the common ion effect, buffer action and the conditions used in Haber's process, with equilibrium shifts distinguished from changes in the equilibrium constant.
Practise Chemical Equilibrium
625 free Chemical Equilibrium MCQs from Chemistry, each with the correct answer and an explanation. Unlimited attempts, no account needed.
Discussion
Stuck on an option, or know a faster way to get there? Ask or explain it here.
No comments yet. Be the first to explain this one.
Exams that ask Chemistry questions like this
Chemistry is on 14 papers prepared for on TestUstad, and all of them draw the same bank, so this question is worth knowing for every one of them.
More Chemical Equilibrium questions
For which one of the following gaseous equilibrium will an increase in pressure increase the yield of the product:
A system at equilibrium can be disturbed by:
Nitrogen dioxide decomposes on heating according to the following equation: 2NO2 (g) ⇌ 2NO (g)+ O2 (g) When 4 moles of nitrogen dioxide were put into a 1 dm3 container and heated to a constant temperature, the equilibrium mixture contained 0.8 moles of oxygen. What is the numerical value of the equilibrium constant, Kc, at the temperature of the experiment?
For the following exothermic reaction, a decrease in temperature will shift the equilibrium towards: 2NO(g) + O2 (g) -> 2NO2 (g)
Which of the following reaction has greater Kp than Kc?
How will the equilibrium of the following reaction be affected if additional nitrogen is added?N2(g) + 3H2(g) ⇌ 2NH3(g)