3.1.6 Chemical Equilibria

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dynamic equilibrium
rate of forwards and backwards reaction equal
concentration of reactants and products constant
only occurs in closed system
Temperature increased
shift in ENDOthermic direction
to reduce temp by absorbing heat
Temperature decreased
shift in EXOthermic direction
increase temp by giving out heat
equilibrium shift to OPPOSE change
Pressure increase
shift to side with fewer gas molecules
to reduce pressure
Pressure decrease
shift to side with more gas molecules
to increase pressure
lower temps may give
higher yield of product
BUT
slow rates of reaction
high pressure may give
higher yield of product
faster rate of reaction
BUT
too high energy costs for pumps
too high equipment costs (has to withstand high pressures)

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3.1.6 Chemical Equilibria

Cards (8)

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3.1.6.2 Equilibrium constant Kc

3.1.6 Chemical equilibria, Le Chatelier's principle and Kc

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3.1.6 - Chemical equilibria, Le Chatelier’s principle and Kc

3.1.6: Chemical Equilibria, Le Chatelier's Principle and Kc

3.1.6 Chemical equilibria, Le Chatelier’s principle and Kc

3.1.6.1 Chemical equilibria and Le Chatelier's principle

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3.1.6 chemical equilibria, le Chatelier's principles and Kc

3.1.6.1 Chemical equilibria and Le Chatelier's principle

3.1.6.2 Equilibrium constant Kc for homogeneous systems

2.3 Chemical Equilibrium