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I’m Lavelle’s lecture today, he said that generally when volume decreases, the equilibrium will shift to the side with less moles of gas. So if volume increases, does equilibrium shift to the side with more moles of gas?
Because K doesn't change when pressure changes, a decreasing volume (or increasing pressure) with more moles of gas on the left will cause the reaction to shift to the right. When the volume is decreased and there are more moles on the right, then the reaction shifts to the left. However, when adding inert gas, there is no change in the reactant or product concentrations and thus no effect on the equilibrium constant.
Yes. If the volume of the container increases then the reaction will favor the side of the reaction with more moles. I think the reason for this is that when you increase the volume, you decrease the concentrations of gases since concentration = moles/volume.
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