Why does increasing the pressure of a gas usually increase reaction rate?
The increased pressure acts as a catalyst on the gas particles in the reaction.
The gas particles are closer, which increases the number of collisions.
The speed of the gas particles increases, which increases the number of collisions.
The surface area of the gas particles increases, which increases the number of collisions.
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Increasing the pressure of a gas usually increases the reaction rate because the gas particles are closer together, which increases the frequency of collisions between particles. This increased frequency of collisions results in a higher likelihood of successful collisions that lead to the formation of products. Additionally, higher pressure also generally results in increased speed of the gas particles, further enhancing the number of collisions and the overall reaction rate.
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