b. Which gas sample has the largest average kinetic energy? c. Which gas sample

Question

b. Which gas sample has the largest average kinetic energy? c. Which gas sample has the fastest average velocity? d. The molecules A are larger than B and thus hit the walls with more force, so how can the pressure in the two containers be equal to each other? 16. Nitrogen gas (N,) reacts with hydrogen gas (H) to form ammonia gas (NH,). You have nitrogen and hydrogen gases in a 18.0 L container fitted with a movable piston (the piston moves so as to keep the pressure inside the container constant). Initially the partial pressure of each reactant gas is 1.0 atm. Assume the temperature is constant and that the reaction goes to completion. a. Calculate the partial pressure of ammonia in the container after the reaction has gone to completion b. Calculate the volume of the container after the reaction has gone to completion. Homework Sets

Explanation / Answer

16.

a. N2 + 3H2 --> 2NH3     Kp = 0.018 [from literature]

Kp = [NH3]^2/[N2][H2]^3

initial [N2] = [H2] = 1.0 atm

let x be the change at equilibrium,

0.018 = (2x)^2/(1-x)(1-3x)^3

0.018 - 0.162x + 0.486x^2 - 0.486x^3 = 4x^2

x = 0.05 atm

so at equilibrium partial pressures of,

p[N2] = 1 - 0.05 = 0.95 atm

p[H2] = 1 - 3 x 0.05 = 0.85 atm

p[NH3] = 2 x 0.05 = 0.10 atm

b. total final pressure = 0.95 + 0.85 + 0.10 = 1.9 atm

total initial Pressure = 2.0 atm

initial volume = 18 L

final volume = 2 x 18/1.9 = 18.95 L

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