Why does increasing temperature generally increase the rate of a chemical reaction? A. It increases the amount of reactant. B. It decreases the size of the reactant particles. C. It causes the particles of the reactants to move faster and collide more often. D. It increases the space between reactant particles, so they have more room to move apart.
Question
Why does increasing temperature generally increase the rate of a chemical reaction? A. It increases the amount of reactant. B. It decreases the size of the reactant particles. C. It causes the particles of the reactants to move faster and collide more often. D. It increases the space between reactant particles, so they have more room to move apart.
Solution
The correct answer is C. "It causes the particles of the reactants to move faster and collide more often."
Here's why:
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Increasing temperature provides the particles with more kinetic energy. This kinetic energy is the energy that particles have due to their motion.
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With more kinetic energy, the particles move faster.
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The faster movement of particles leads to more frequent collisions between the reactant particles.
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Not only are there more collisions, but the collisions are also more energetic. This means that a greater proportion of the collisions have enough energy to overcome the activation energy of the reaction (the minimum energy required for a reaction to occur).
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Therefore, the rate of reaction increases because more of the collisions result in a reaction.
Options A, B, and D are not correct because temperature does not directly affect the amount or size of reactant particles, nor does it increase the space between them.
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