To minimise pressure surges and maintain a constant mass flow in the cabin

Equi. Homogeneous reactants and products in the same physical state. Equi different heterogeneous. Kc: The law of mass action tells us the equilibrium constant q is the product of the high concentration of the products to their stoichiometric coefficients, divided by the product of the concentrations of the reactants raised to their respective stoichiometric coefficients. The value of Kc is specific for each reaction qiomica and independent of initial concentrations of reactants and products. It just depends on the temperature. T = KC = Degree of dissociation: indicates the amount to as x q open one of reagent reacted. Is the ratio between the amount, expressed in mol, q reagent has reacted and the amount of initial reagent: a = Qc reaction quotient: q has the same form of expression and the equilibrium constant is the mathematical ratio of the initial concentrations of reactants and products. If Qc = 0 à DERCHO. Qc = infinity izkierd. Comparing balance Kc Qc = Qc <Kc right Qc> Kc Kp IZKI it is independent of the initial concentrations of reactants and products and only depends on temperature. Le Chatelier's principle: when a system undergoes a change in equilibrium concentration of the reacting species, pressure or temperature the system responds reaching a new equilibrium that partially counteract the effect of the modification.

Modification of the concentration: a) increasing the concentration of reactants or the product Diminish Qc <Kc is shifted to the right. B) if we decrease the concentrcion of reagents or increase the product Qc> Kc is shifted to the izkierda.

Modification of pressure or volume: at T = constant) pressure: adding or removing a species in gaseous concentration and modifying the reaction goes as above. - Adding an inert gas to maintain constant volume. No effect on balance pro xq no partial pressure increases. If pressure is maintained cntante increase the total volume of the mixture and apply displacement criterion studied. - Changing the system volume ddel. Implies decrease in pressure and vice versa. B) changing the volume: volume-increasing pressure and Diminish concentreacion, so ke be moved to where greater number of moles of gas - lower concentrations duress and the volume increases and moves to where there are no moles Mnor gases. C) amend temperature: a temperature increase favors the sense that the reaction is endothermic and decreased the sense ke is exothermic. Increm H