The equilibrium constant, K_p, is 2.4 10³ at a certain temperature for the following reaction.

2 NO(g) N₂(g) + O₂(g)

For which of the following sets of conditions is the system at equilibrium? For those that are not at equilibrium, in which direction will the system shift? Give the value of the reaction quotient, Q, to justify your answer.

(a) P_NO = 0.010 atm, P_N2 = 0.11 atm, P_O2 = 2.0 atm

Q < K_p so the reaction shifts right.Q > K_p so the reaction shifts right. Q < K_p so the reaction shifts left.Q > K_p so the reaction shifts left.Q = K_p so the reaction is at equilibrium.

(b) P_NO = 0.0078 atm, P_N2 = 0.36 atm, P_O2 = 0.67 atm

Q < K_p so the reaction shifts right.Q > K_p so the reaction shifts right. Q < K_p so the reaction shifts left.Q > K_p so the reaction shifts left.Q = K_p so the reaction is at equilibrium.

(c) P_NO = 0.0062 atm, P_N2 = 0.51 atm, P_O2 = 0.18 atm

Q < K_p so the reaction shifts right.Q > K_p so the reaction shifts right. Q < K_p so the reaction shifts left.Q > K_p so the reaction shifts left.Q = K_p so the reaction is at equilibrium.