WenonaMajkowski188
Answered

Welcome to Westonci.ca, the ultimate question and answer platform. Get expert answers to your questions quickly and accurately. Discover comprehensive solutions to your questions from a wide network of experts on our user-friendly platform. Get detailed and accurate answers to your questions from a dedicated community of experts on our Q&A platform.

As the temperature of a chemical reaction in the gas phase is increased, the rate of the reaction increases because
(1) fewer particle collisions occur
(2) more effective particle collisions occur
(3) the required activation energy increases
(4) the concentration of the reactants increases

Sagot :

Edufirst
Answer: option (2) more effective particle collisions occur.


Justification:


Always keep in mind that the temperature is a measure of the average kinetic energy of the particles.


The higher the temperarute the hiigher the kinetic energy.


Also, remeber that the kinetic energy is the energy of motion: the higher the kinetic energy the hgher the speed of the particles and the more energetic the collisions.


Therefore, those more energetic collisions will increase the number of collisions that overcome the activiation energy leading to higher rate of conversion (reaction), whic is what a more effective particle collisions occur mean.
We hope this was helpful. Please come back whenever you need more information or answers to your queries. Your visit means a lot to us. Don't hesitate to return for more reliable answers to any questions you may have. Westonci.ca is here to provide the answers you seek. Return often for more expert solutions.