Question

For the reaction N2O4(g) m 2 NO2(g), a reaction mixture at a certain temperature initially contains both N2O4 and NO2 in their standard states (see the defi nition of standard state in Section 6.9 ) . If Kp = 0.15, which statement is true of the reaction mixture before any reaction occurs? (a) Q = K; the reaction is at equilibrium. (b) Q 6 K; the reaction will proceed to the right. (c) Q 7 K; the reaction will proceed to the left.

Answer 1

The reaction mixture is at equilibrium because Q = K.

Step-by-step explanation:

In the given question, we are told that the reaction N2O4(g) m 2 NO2(g) has an equilibrium constant (Kp) of 0.15. We are asked to determine the state of the reaction mixture before any reaction occurs. To do this, we can compare the reaction quotient (Q) to the equilibrium constant (K). If Q = K, the reaction is at equilibrium. If Q < K, the reaction will proceed to the right. And if Q > K, the reaction will proceed to the left. Since the given Kp value is 0.15 and there is no information about the initial concentrations of N2O4 and NO2, we cannot determine the exact value of Q. Therefore, the correct answer is (a) Q = K; the reaction is at equilibrium.