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What is the effect of an increase in pressure, and an increase in expansion on an equilibrium equation with more moles of reactant on the left side of the equation as compared to moles of product? Why is this the case?
Increase in pressure equals to a decrease in volume; what an increase in pressure does is that it increases all the molar concentrations within the system. What Le Chatelier's principle tells us is that in order to minimize this sudden increase in molar concentration, the equilibrium shifts to the side in which there are fewer moles because naturally, fewer moles increase less than that of the side with more moles.
An increase in expansion is increasing the volume, so the reverse action will occur (concentration moves from lower moles equation -> higher moles side of equation)
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