Collision Theory

The video explains how chemical reactions occur through particle collisions, emphasizing the need for sufficient energy, known as activation energy, for successful reactions. It discusses four factors affecting reaction rates: temperature, pressure, concentration, and catalysts. Higher temperatures increase particle energy, leading to more successful collisions. Increased pressure and concentration raise collision frequency. Catalysts provide alternative reaction pathways with lower activation energy, speeding up reactions. Understanding these factors allows control over reaction rates, crucial for chemical manufacturing.

What is the minimum amount of energy required for a reaction to occur called?

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What are the four factors that can affect the frequency of particle collisions?

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How does increasing temperature affect the rate of reaction?

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What effect does increasing pressure have on gas reactions?

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Explain how a catalyst speeds up a chemical reaction.

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