In a reaction (at equilibrium) that makes more moles of gas than it consumes, what is the effect of increasing the pressure?
Well, if you make more mols of gas...
#aA(g) -> bB(g)#
#b > a#and these are stoichiometric coefficients.
Write the equilibrium constant.
#K_P = P_B^b/(P_A^a)#
#K_P = P_B^(a+c)/(P_A^a)#
#= (P_B/P_A)^a P_B^c#
If you increase the total pressure, you must increase the partial pressures.
Even if the mols of
Therefore, the equilibrium is skewed towards the products, and by Le Chatelier's principle, it wishes to undo the imbalance and shift towards the reactants.