For the reaction N₂(g) + 3 H₂(g) ⇌ 2 NH₃(g), the equilibrium constant is K_p = 36.5 at 400 K. Two separate equilibrium mixtures have the following compositions at 400 K and a total pressure of 1.00 bar.

Equilibrium mixture A:

0.0424 mol N₂ 0.136 mol H₂ 0.176 mol NH₃

Equilibrium mixture B:

0.194 mol N₂ 0.0403 mol H₂ 0.0706 mol NH₃

(a) By expressing the partial pressures in the form P_i = x_iP, where x_i is the mole fraction of a particular gas and P is the total pressure, show that the reaction quotient for the reaction can be written as

(b) Calculate Q_p for each equilibrium mixture to verify that Q_p = K_p in each case.

(c) Suppose that 0.100 mol N₂ is added at constant pressure to each mixture. By comparing the values of Q_p and K_p, verify that the addition of N₂ causes a net reaction to the right for mixture Abut a net reaction to the left for mixture B.

Transcribed Image Text:

XNH3 1 2 X p² 3 XN₂XH₂