Rates of Reaction and Equilibria Key Definitions

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Rate of Reaction
The rate at which reactants are being converted into products
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Collision Theory
Particles must collide to react. A minimum amount of energy is needed for a reaction to occur. They must also collide in the correct orientation
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Concentration
The amount of solute in a given volume of solvent
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Kinetic Energy
The energy possessed by a body because of its motion
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Activation Energy
The minimum amount of energy that the colliding particles must possess for a collision to result in a reaction
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Catalyst
A substance that increases reaction rate without being consumed by the overall reaction
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Homogeneous Catalyst
Reactants and catalyst are in the same state
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Heterogeneous Catalyst
Reactants and catalyst are in different states
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Static Equilibrium
A system in equilibrium that is in balance and not changing (there is no movement)
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Dynamic Equilibrium
A system in equilibrium with continuous movement- forward and reverse rates are the same
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Closed System
Nothing is added or taken away e.g. pressure, concentration and temperature
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Le Chatelier's Principle
When a change is made to a system in equilibrium, the position of equilibrium moves to oppose the change made
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Reversible Reaction
Reactions that take place in both forward and reverse directions
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Other cards in this set

Card 2

Front

Particles must collide to react. A minimum amount of energy is needed for a reaction to occur. They must also collide in the correct orientation

Back

Collision Theory

Card 3

Front

The amount of solute in a given volume of solvent

Back

Preview of the back of card 3

Card 4

Front

The energy possessed by a body because of its motion

Back

Preview of the back of card 4

Card 5

Front

The minimum amount of energy that the colliding particles must possess for a collision to result in a reaction

Back

Preview of the back of card 5
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