The equilibrium constant K c is 10 for N₂O₄ 2 NO₂ .
Initially, 1.00 mole of N₂O₄ is sealed in a 10.0 liter flask. What are the molar concentrations of all species at equilibrium?

Question

The equilibrium constant K c is 10 for N₂O₄ 2 NO₂ . Initially, 1.00 mole of N₂O₄ is sealed in a 10.0 liter flask. What are the molar concentrations of all species at equilibrium?

Quizplus · Accepted Answer

We can start by writing the equilibrium expression for the reaction: N₂O₄ ⇌ 2 NO₂ Kc = [NO₂]²/[N₂O₄] Let's assume that at equilibrium, the concentration of N₂O₄ is x. Then, the concentration of NO₂ will be 2x (because of the stoichiometry of the reaction). Substitute these concentrations into the equilibrium expression: Kc = (2x)²/x = 4x²/x = 4x Solve for x: Kc = 10 = 4x x = 2.5 Now, we can use these values to find the concentrations of NO₂: [NO₂] = 2x = 5.0 And the concentration of N₂O₄: [N₂O₄] = x = 2.5 Finally, we can convert these concentrations into molarities by dividing by the volume of the flask: [NO₂] = 5.0/10.0 = 0.5 M [N₂O₄] = 2.5/10.0 = 0.25 M Therefore, the correct answer is choice B.

The Equilibrium Constant K C Is 10 for N₂O4

The Equilibrium Constant K C Is 10 for N₂O₄