How does increasing temperature cause an increase in rate of reaction?

As you increase the temperature of the reaction, the particles gain kinetic energy. This causes them to move faster and as a result, the frequency of collisions increases. This means there is an increased proportion of collisions with energy greater than or equal to the activation energy, so it is easier for the reaction to occur, which increases the rate. The activation energy is the minimum energy required by the collision between two particles for them to react. An opposite effect is seen with lowering the temperature, which lowers the rate of reaction.

AB
Answered by Aryan B. Chemistry tutor

2570 Views

See similar Chemistry GCSE tutors

Related Chemistry GCSE answers

All answers ▸

Can you explain the properties of a giant covalent lattice?


What is an ionic bond?


Explain how electrons are arranged.


A colourless liquid is tested with silver nitrate solution and produces a white precipitate and produces a brick red flame test result. Name the compound found in the colourless liquid


We're here to help

contact us iconContact ustelephone icon+44 (0) 203 773 6020
Facebook logoInstagram logoLinkedIn logo

© MyTutorWeb Ltd 2013–2025

Terms & Conditions|Privacy Policy
Cookie Preferences