Activity $7\mathrm{.}3$

The Haber$-$Bosch Process: Syr

Ammonia, $N{H}_3(g),$ is produced in the millions of tonnes each year. Among other things, it is used to prepare fertilizers and explosives. The procedure uses atmospheric nitrogen and hydrogen to produce ammonia in a process represented by the following equilibrium equation:

$N_2(g)+3H_2(g)2N{H}_3(g),H_r=-92k\frac{J}{m}ol$

Procedure

Look carefully at the equilibrium equation for the preparation of ammonia and at the boiling point data below. In small groups, use Le Ch$$telier$\text{'}$s principle, and other concepts you have learned in this course, to answer the following questions.

Boiling Points of Three Compounds

$\backslash$table$[[$Compound$,$Boiling Point $(C)$

$6.$ Prepare a table to summarize the reaction conditions $($temperature$,$ pressure, use of catalyst, amounts of reactants, and amount of products$)$ required to produce ammonia on an industrial scale. Explain your reasoning in terms of Le Ch$$telier$\text{'}$s principle and other chemistry concepts.