Problem: Nitrogen and hydrogen react to form ammonia according to the following equation:N2(g) + 3 H2(g) → 2 NH3(g)Consider the following representations of the initial mixture of reactants and the resulting mixture after the reaction has been allowed to react for some time:If the volume is kept constant, and nothing is added to the reaction mixture, what happens to the total pressure during the course of the reaction?

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The given reaction is a gas-evolution reaction. If the reaction is allowed to proceed with the volume of the container is kept constant,

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Nitrogen and hydrogen react to form ammonia according to the following equation:
N2(g) + 3 H2(g) → 2 NH3(g)
Consider the following representations of the initial mixture of reactants and the resulting mixture after the reaction has been allowed to react for some time:

Two containers, the container on the left contains the initial amounts of reactants and has three molecules composed two blue spheres combined and eight molecules composed of two smaller white spheres combined. The container on the right is the mixture after it has been allowed to react for some time. It has one molecule of two blue spheres combined, two molecules of two white spheres combined, and four molecules composed of a central blue sphere surrounded by three white spheres in a trigonal pyramidal geometry.


If the volume is kept constant, and nothing is added to the reaction mixture, what happens to the total pressure during the course of the reaction?

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