Equilibrium Flashcards
Definition of dynamic equilibrium
When the rates of forward and reverse reactions are equal.
COncentration of reactants and products remain constant, but not necessarily equal.
EOE: High temperature in an Endothermic reaction
Equilibrium moves to the right
EOE: Low temperature in a Endothermic reaction
Equilibrium moves to the left
EOE: High temperature in an Exothermic reaction
Equilibrium moves to the right
EOE: High temperature in an Exothermic reaction
Equilibrium moves to the left
EOE: Increased pressure
Equilibrium moves to the side with less gas
EOE: Decreased Pressure
Equilibrium moves to the side with more gas
EOE: Catalysts
A catalysts has the effect of lowering the energy barrier between reactants and products by providing alternative reaction paths.
Endothermic reactions
Release energy
Exothermic reactions
Release energy
Effect of pressure on reactions between gases
Increase in pressure results in the particles being closer together and results in a higher chance of reaction
What does this symbol mean?
⇌
This means that it is a reversible reaction where the reactants form products, which react together to give the reactants back.
Why can equilibrium only be reached in a closed system?
None of the reactants or products are lost.
In an open system, products (or reactants) are lost, therefore equilibrium cannot be established.
Describe the concentrations of reactants and products at equilibrium.
At equilibrium, the concentration of reactant and products remain constant but NOT always equal.
Describe the rates of the forward and reverse reactions at equilibrium.
They take place at equal rates.
Name a reaction condition which will affect the position of equilibrium.
- the addition or removal of reactants or products
- altering temperature
- altering pressure
What way will the equilibrium lie in the following reaction if:
More Fe3+(aq) is added
Fe3+(aq) + CNS-(aq) ⇌ FeCNS2+(aq
Equilibrium will shift to the right and make more products.
What is the Haber Process?
The Haber Process combines nitrogen from the air with hydrogen derived mainly from natural gas (methane) into ammonia. The reaction is reversible and the production of ammonia is exothermic.
What effect would adding a catalyst to a reversible reaction have on the equilibrium?
Adding catalyst has no effect on the position of equilibrium.
Allows equilibrium to be reached more quickly, or established at a lower temperature
