Chapter 14, Problem 14.132QP

Consider the production of ammonia from its elements:

${\text{N}}_2(g)+3{\text{H}}_2(g)\stackrel{}{\rightleftharpoons }2{\text{NH}}_3(g)$

In a pilot experiment, a mixture of 1.00 part nitrogen gas and 3.00 parts hydrogen gas at a total pressure of 10.00 atm was passed through a hot tube over a catalyst at 450.0°C. What are the total moles of gas in a 1.000-L volume of this equilibrium mixture? If the equilibrium mixture contains a partial pressure of 0.204 atm of ammonia, how many moles of ammonia are in this 1.000-L volume? How many moles of N₂ are in this same volume? What is the partial pressure of N₂ in this equilibrium mixture? What is the equilibrium constant K_p for this reaction?