Le Chatalier's Principle Case Study

1) There is a gradual rise in the concentration of the products (NO and Cl2) and a gradually reflecting decrease in the concentration of the reactants (2NOCl). Le Chatalier 's Principle states that if a system at equilibrium is applied with stress, then the system will react to compromise that stress. In terms of temperature, Le Chatalier 's Principle states that if heat is added to the system, the chemical system will react by shifting the reaction to the side that will consume the heat. In this case, an increase in the temperature (heat) added to the left side which caused the reaction to shift to the right (endothermic). By producing more products, the heat added on the reactant is consumed.
2) The concentration of the products and the reactants suddenly spike. After this sudden increase, The concentration of the …show more content…
Le Chatalier 's Principle states that if a system lost or gained heat the reaction will proceed in the direction that counters the stress. In this case, heat was removed and this will result a in reverse reaction where the reaction will shift to the left side to produce more reactant and gain the heat as an endothermic reaction.

iv) in this case, there is no change in shifts of the reaction. the equilibrium would stay the same as catalyst only either speeds up or slows down the rate of reaction but not the equilibrium state.

B) in the summer, the heat in the air and the N2O4 will react to form 2NO2 (brown haze) in a reverse reaction to counter and consume the heat. In the winter the, air would be cold, this would result the in the reaction shifting to the right to replace lost heat by producing heat and N2O4 as products.
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a) By adding more reactants (ammonia or oxygen or both) will shift the reaction to the right to produce more products to reach equilibrium.
b) By removing the water and nitrous oxide from the products by condensation, this will force the reactant to produce and replace more