As shown in Table 15.2, the equilibrium constant for the reaction N₂(g) + 3H₂(g) ⇌ 2 NH₃(g) is K_p = 4.34 × 10^-3 at 300°C. Pure NH₃ is placed in a 1.00-L flask and allowed to reach equilibrium at this temperature. There are 1.05 g NH₃ in the equilibrium mixture.

(a) What are the masses of N₂ and H₂ in the equilibrium mixture?

(b) What was the initial mass of ammonia placed in the vessel?

(c) What is the total pressure in the vessel?

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Table 15.2 Variation in K, with Temperature for N2 + 3H2 = 2 NH Temperature (°C) K, 300 4.34 X 10-3 400 1.64 X 104 450 4.51 x 105 500 1.45 X 105 550 5.38 X 106 600 2.25 X 10