For the following exothermic reaction, a decrease in temperature will shift the equilibrium towards: 2NO(g) + O2 (g) -> 2NO2 (g)
Correct answer: D. Right
- A. Left
- B. The Point of Equilibrium
- C. Both Directions
- D. Right
Explanation
For an exothermic reaction like 2NO (g) + O2 (g) ⇌ 2NO2 (g), a decrease in temperature will shift the equilibrium towards the right. This shift helps to increase the temp as heat is released in exothermic reactions, as the reaction is exothermic in the forward direction. Therefore this option is correct.
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
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:
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:
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)
The value K for H2(g) + CO2(g) <-> H2O(g) + CO(g) is 1.80 at 1000 C. If 1.0 mole of each H2 and CO2 are placed in 1 litre flask, the final equilibrium concentration of CO at 1000 C will be: