For the equilibrium 2 NOBr(g)$\leftrightarrows$ 2 NO(g)+ Br₂(g),K_c = 1.56 $\times$10^-3 at 300 K.Suppose 0.400 M NOBr is placed in a reaction vessel at 300 K.At a given point,the concentration of Br₂ is 0.0134 M.Which of the following statements is true?

Question

Quizplus · Accepted Answer

First, we need to calculate Q, the reaction quotient, using the given concentrations:
Q = [NO]²[Br₂]/[NOBr]² = (0.0134)²/(0.400)² = 0.00015536
Since Q < K, the system is not at equilibrium and there is not enough product formed yet. Therefore, the reaction will continue to make more products until Q = K at equilibrium. So, the correct choice is A.

For the Equilibrium 2 NOBr(g) ⇆\leftrightarrows⇆ 2 NO(g)+ Br2(g),Kc = 1 ×\times×

For the Equilibrium 2 NOBr(g) $\leftrightarrows$ 2 NO(g)+ Br₂(g),K_c = 1 $\times$