10507067
Descripción
Mapa Mental por Chloe Drewery, actualizado hace más de 1 año
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Creado por Chloe Drewery
hace alrededor de 7 años
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Equilibrium Revision Mindmap
- Kp
- It is the same as Kc, except Kp is for gases and involves partial
pressures instead of concentrations.
- Partial Pressure (p) = mole fraction x total pressure.
- It is the same as Kc, except Kp is for gases and involves partial
pressures instead of concentrations.
- Kc
- This is the equilibrium constant = [products] / [reactants]
- Greater than 1, equilibrium lies to the right.
- Less than 1, equilibrium lies to the left.
- =0, equilibrium lies directly in the middle.
- This is the equilibrium constant = [products] / [reactants]
- Effect of Temperature
- Changing the temperature causes the value
of Kc/Kp to change as temperature is a
condition.
- For an exothermic reaction: increasing temperature causes K to decrease.
Decreasing temperature causes K to increase.
- For an endothermic reaction: increasing temperature
causes K to increase. Decreasing temperature causes K to
decrease.
- Changing the temperature causes the value
of Kc/Kp to change as temperature is a
condition.
- Effect of Concentration
- Changing concentration doesn't affect the value of Kc.
- Changing concentration doesn't affect the value of Kc.
- Effect of Pressure
- Changing pressure doesn't affect the value of Kc.
- Changing pressure doesn't affect the value of Kc.
- Effect of Catalyst
- Adding a catalyst doesn't affect the value of Kc.
- Adding a catalyst doesn't affect the value of Kc.
- Equilibrium
- Homogeneous: all species are in the same state.
- Heterogeneous: species which make up the reactants
and products are in different physical states.
- An equilibrium is where the rate of the
forwards reaction is equal to the reverse.
- Requires: A closed system and a reversible reaction.
- Le Chatelier's Principle: When a system at equilibrium is
disturbed, equilibrium shifts to oppose this change.
- Homogeneous: all species are in the same state.
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