For the Equilibrium 2 NOBr(g) ⇄ 2 NO(g) + Br₂ $\lt$

question 30

Multiple Choice

For the equilibrium 2 NOBr(g) ⇄ 2 NO(g) + Br₂ (g) , K_c = 1.56 * 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 statement below is true?

• A)Q \(\lt\)K, so the reaction will continue to make more products.
• B)Q \(\gt\) K, so the reaction will consume products to make more reactants.
• C)Q = K, so the system is at equilibrium.
• D)The value of K will decrease until it is equal to Q.
• E)The value of K will increase until it is equal to Q.

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