Le Chatelier's Principle

This chemistry video tutorial provides a basic introduction into Le Chatelier's Principle of chemical equilibrium. It explains how to determine which direction the reaction will shift if the concentrations of the reactants or the products increase in value. It discusses the effect of adding a catalyst or an inert gas on the position of equilibrium. It also discusses the effect of changing the volume and pressure on equilibrium.
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17:09 Sir, adding an inert gas could increase the pressure so the position of equilibrium will shift to the right since products have less molecules, therefore CO decreases.

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7:05 Just a small note, this would only be true if the volume for the amount of A being added is negligible, as if it wasn't negligible, b would have higher concentration.

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I'm confused about 9:45 ,when the reactant goes up and product goes down it should shift to the left. why shift to the right?

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​@@ayushnaprasad5068 bro to increase the concentration of nh3 the equi will shift towards product

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Please can you make a video on the effect of changes in temperature on Le Chetalier’s principle

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Great job as always bro! But what if we add inert gases at constant pressure and at constant volume? coz they do affect the equilibria

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this response might be a little late but inert gases don’t have any effect on the reaction because it is not a part of the reaction.

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under KTG assumptions no change but real gases do not behave ideally. thus the volume occupied by the inert gas is not negligible and causes the reaction to be shifted to the side with less moles.

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