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In terms of activation energy, why does increasing the temperature of a
reaction make it proceed more quickly?
A. Increasing the temperature reduces the activation energy.
B. Increasing the temperature increases the potential energy of the
reactants.
O C. Increasing the temperature increases how many reactant
molecules reach activation energy.
D. Increasing the temperature makes the molecules move slower.

Respuesta :

Answer:

At higher temperatures, the particles move more quickly and collide more often.

Explanation:

mickymike92

Increasing the temperature increases the potential energy of the reactants, thus making the reaction faster.

What is activation energy?

Activation energy is the minimum energy that reactant molecules must possess in order to collide together to form products.

Increasing the temperature of a reaction helped to make the reaction proceed faster. This is because more reactant particles acquire the energy greater than or equal to the activation energy.

Therefore, increasing the temperature of a reaction makes it proceed more quickly.

Learn more about activation energy at: https://brainly.com/question/26724488

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