le chateliers principle
- Created by: tia5sos
- Created on: 05-12-20 14:05
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- le chatelier's principle
- whatever you do to a reversible reaction, the equilibrium position will move to try to undo your change
- the equilibrium position moves to minimise any changes you make
- le chatelier's principle states that if there's a change in concerntration, pressure of temperature in a reversible reaction, the equilibrium position will move to help counteract that change
- temperature
- if you decrease the temperature, the equilibrium will move in the exothermic direction to produce more heat
- if you increase the temperature, the equilibrium will move in the endothermic direction to absorb the extra heat
- pressure
- if you increase the pressure, the equilibrium will move towards the side that has fewer moles of gas to reduce pressure
- if you decrease pressure, the equilibrium will move towards the side that has more moles of gas to increase pressure
- concerntration
- if you increase the concerntration of the reactants, the equilibrium will move to the right to use up the reactants (making more products)
- if you increase the concerntration of the products, the equilibrium will move to the left to use up the products (making more reactants)
- decreasing the concerntration will have the opposite effect
- you can predict how the position of equilibrium will change
- you can apply the rules for pressure, concerntration and temperature to any reversible reaction to work out how changing the conditions will effect the equilibrium position
- you can increase yield (how much product is made during a reaction) by changing the conditions to shift the equilibrium to the right (towards the product)
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