Describe how collision theory explains an increase in the rate of a reaction at higher temperatures.

When temp increases, kinetic energy of molecules increases. Higher kinetic energy means molecules move around more and increased movement leads to more collisions. Collision theory states that the rate of reaction is proportional to the number of collision so therefore rate of reaction increases. (It is assumed that these collisions will meet the activation energy for the reaction)

Answered by Charlie M. Chemistry tutor

1642 Views

See similar Chemistry A Level tutors

Related Chemistry A Level answers

All answers ▸

4.00 g metal carbonate, MCO3 reacts with acid to liberate a gas that occupies 0.5878 dm3 at 25˚C and 2.0 x 105 Pa. Identify the group 2 metal, M. Info: R = 8.314 J K-1 mol-1


Explain trend in why the ionisation energies increase across the period


(i) What property does Magnesium Oxide have that makes it useful to create heat-resistant bricks to line furnaces? (ii) Explain why H2S exists as a gas and H2O exists as a liquid (at r.t.p).


State the reagents and conditions for the formation of an aldehyde, starting from a primary-alcohol.


We're here to help

contact us iconContact usWhatsapp logoMessage us on Whatsapptelephone icon+44 (0) 203 773 6020
Facebook logoInstagram logoLinkedIn logo

© MyTutorWeb Ltd 2013–2024

Terms & Conditions|Privacy Policy
Cookie Preferences