The Haber-Bosch process is used in industry to produce ammonia. Explain how the use of high temperature and pressure affects the rate of reaction.

According to collision theory: Increasing the temperature increases the average energy of the system. This means more molecules have enough energy to overcome the activation enthalpy when they collide, causing more collisions to be successful and hence leading to a faster reaction. Increasing the pressure increases the number of collisions between the molecules, meaning a higher likelihood for a successful collision.

AW
Answered by Adam W. Chemistry tutor

3869 Views

See similar Chemistry A Level tutors

Related Chemistry A Level answers

All answers ▸

What's the difference between Sn1 and Sn2 reactions?


How can you tell if a reaction is endothermic or exothermic? Describe a way of determining if a reaction is exothermic or endothermic using simple laboratory equipment.


Giving the electronic configurations for each element, predict the trend in 1st ionisation energies going across period 2 from Lithium to Neon.


Why is 2-trichloroethanoic acid such a strong acid?


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 2013–2025

Terms & Conditions|Privacy Policy
Cookie Preferences