Question

Consider the following equilibrium: 4NH3 (g) + 5O2 (g) ↔4NO(g) + 6H2O (g) + 14.4 kJUse Le Chatelier’s principle to describe the all the possible reaction conditions that would favour theproduction of nitrogen monoxide and provide a brief explanation using the collision theory to explainwhy.

Answer 1

Conditions that would favour the production of nitrogen monoxide.

1. Changing of concentration

If you add more concentration of the reactants, the forward reaction will be favoured, the reaction will shift to the right, therefore more NO will be produced, to restore the equilibrium.

2. Changing of temperature

Since this reaction is exothermic (since heat is the product), if the temperature is decreased, the reaction will shift forward, meaning it will shift to the right, this will then produce more NO.

3. Changing the volume/pressure

If we increase the volume, meaning if we decrease the pressure, the reaction will shift towards the side with more particles, the forward reaction has more particles, so the equilibrium will shift to the right and produce more NO.