As shown in Table 15.2, the equilibrium constant for the reaction
N₂(g) + 3 H₂(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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The equilibrium constant for the reaction N2 (g) + 3H2 (g)----><----2NH3 (g) is Kp = 4.34 x 10^{ - 3} at 300 degrees C.Pure NH3 is placed in a 1.00L flask and allowed to reachequilibrium at this temperature. There are 1.05 g NH3 in theequilibrium mixture.

A)What is the mass of N2 in the equilibrium mixture?

B)What is the mass of H2 in the equilibrium mixture?

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

D)What is the total pressure in the vessel?

peachdinosaur663

Question #4. Nitrogen gas and hydrogen gas are combined and allowed to react at a certain temperature according to the following reaction: N2(g) + 3H2(g) double arrow 2 NH3(g)

At equilibrium the total pressure in the vessel is 50.0 atm. The mixture contains the following mole fractions: 0.890 NH3, 0.228 N2, and 0.683 H2. Determine Kp at the temperature of this experiment.

As shown in Table 15.2, K_p for the equilibrium

N₂(g) + 3 H₂(g) 2 NH₃(g)

is 4.51 × 10^-5 at 450 °C. For each of the mixtures listed here, indicate whether the mixture is at equilibrium at 450 °C. If it is not at equilibrium, indicate the direction (toward product or toward reactants) in which the mixture must shift to achieve equilibrium.

(a) 98 atm NH₃, 45 atm N₂, 55 atm H₂
(b) 57 atm NH₃, 143 atm N₂, no H₂
(c) 13 atm NH₃, 27 atm N₂, 82 atm H₂