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9 Cards in this Set
- Front
- Back
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Define the term 'activation energy' |
The minimum amount of energy required for successful collisions between particles and a reaction to occur |
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Explain why an increase in pressure, at a constant temperature, increases the rate of a reaction |
Particles are closer together and therefore collide more often |
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Define the term 'catalyst' |
a substance used to speed up a reaction but remains chemically unchanged at the end |
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Explain, in general terms, how a catalyst works |
Provides an alternate route/pathway Lowers the activation energy |
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In order for 2 particles to react, they must collide. Explain why most collisions do not result in a reaction. |
They do not have the activation energy |
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State one way in which the collision frequency between particles in a gas can be increased without changing the temperature. |
Increase pressure |
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Suggest why a small increase in temperature can lead to a large increase in reaction rate between colliding particles. |
Because even a small increase means that many more particles have the activation energy or higher |
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State Le Chatelier's Principle |
if any factor is changed that affects an equilibrium, the position of equilibrium will shift to oppose that change |
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state the effect, if any, of a catalyst on the position of an equilibrium |
none |
