Reaction:
2NH3(g) + 2,5O2(g) = 2NO(g) + 3H2O(g) + heat (exothermic reaction)
Le Chateleier’s principle states: “When an equilibrium system is disturbed, it will adjust to diminish the change that has been made to it”.
There are 4 factors that can influence the equilibrium state: changes of pressure, temperature, concentration and addition of a catalyst.
1. The increasing of pressure causes the shift of equilibrium towards the reaction, where smaller volume of gases is formed. In our case, there are 4.5 moles of gas in the left part of the reaction, and 5 moles in the right part. So, if the pressure decreases, the equilibrium will shift towards the increasing of NO yield.
2. The increasing of temperature promotes the endothermic reaction. There is an exothermic reaction. Therefore, to increase the NO yield, the temperature must be decreased.
3. The increasing of concentration of the reagents leads to a shift in equilibrium toward their use. In our reaction, increasing the concentration of either NH3 or O2 will increase the NO yield. Also, the decreasing of products concentration leads to a shift in equilibrium the right.
4. Addition of a catalyst makes the reaction possible and towards the increasing of NO yield.
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