Increasing the concentration of a substance increases the kinetic energy of the particles that make up the substance.

Catalyst describes the idea that atoms, ions, and molecules must collide in order to react.

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Decreasing the concentration of reactants increases the collision frequency between reacting particles.

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• FALSE

Catalysts increase the rates of chemical reactions by raising the activation energy of the reactions.

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• FALSE

A chemical reaction may be energetically favorable (i.e. exothermic), and so if the activation barrier is high (i.e. the activation energy is high), the reaction rate may be extremely slow.

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Smaller particle size allows for a larger surface area to be exposed for the reaction.

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Raising the temperature of a reaction increases the rate of the reaction by increasing the energy of the collisions between reacting particles.

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Lowering the surface area of a reactant increases the rate of the reaction.

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Collisions only result in a reaction if the particles collide with a certain maximum energy called the activation energy of the reaction.

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Catalysts permit reactions to proceed along a higher energy path.

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• FALSE