Initially one mole each N2 and O2 were made to react as,If at equilibrium 0 ∙ 25 moles of O2 is present the equilibrium concentration of NO will be:
Correct answer: C. 1.50 moles
- A. 0.50 moles
- B. 0.125 moles
- C. 1.50 moles
- D. 1.75 moles
Explanation
N2(g) + O2(g) 2NO(g) As from the balance chemical equation it is clear that 1 mole O2 gives 2 mole NO so as 0.25 mole O2 left so 0.75 mole consumed so it will give 1.50 mole NO.2x0.75-1=1.50
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 the reaction,CO(g) + (1/2)O2(g) ⟶ CO2(g)
Students were heating CaCO3 in an open container to produce CO2 gas,CaCO3(s) ⟶ CaO(s) + CO2(g)If we increase pressure on this system the:
Value of Kspfor PbSO4 systems at 25 °C is equal to:
For exothermic reversible reaction, the activation energy for forward direction depends upon:
The pH of an acidic buffer depends upon the concentration of acid, concentration of salt and:
For a particular reversible reaction If [Products]/[Reactants]>Kc It means that: