Easy Tips/Tricks about Effect of change in concentration, pressure/volume on chemical Equilibrium

Le Chatelier's Principle: If a system at equilibrium is subjected to a change in concentration, pressure, or temperature, the system will adjust itself to counteract that change and establish a new equilibrium state.
1. Effect of Change in Concentration
Changing the concentration of a reactant or product disturbs the equilibrium, forcing it to shift to consume the added substance or replace the removed substance.
Increase concentration of Reactants: Equilibrium shifts to the right (towards products).
Decrease concentration of Reactants: Equilibrium shifts to the left (towards reactants).
Increase concentration of Products: Equilibrium shifts to the left (towards reactants).
Decrease concentration of Products: Equilibrium shifts to the right (towards products).
2. Effect of Change in Pressure/Volume (Gaseous Systems) Pressure and volume are inversely related (\(P\propto 1/V\)). Changes only affect reactions involving gases where the total moles of gas differ on either side of the equation (\(\Delta n_{g}\ne 0\)). A. Increasing Pressure (Decreasing Volume) Action: The system reduces volume, increasing pressure.Shift: To reduce pressure, the system shifts to the side with fewer moles of gas.

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