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

4168 Views

See similar Chemistry A Level tutors

Related Chemistry A Level answers

All answers ▸

What is the difference in kinetics between a 0th, 1st and 2nd order reaction?


Describe the arrangement of protons, neutrons and electrons in an atom of Neon (Atomic No. 10, Atomic Weight 20.18). You may use diagrams to aid you.


In terms of Electrostatic Forces, Suggest why the ‘Electron Affinity’ of Fluorine has a Negative value.


If we burn 3 moles of carbon in air (as per the equation), what mass (in grams) of carbon dioxide will be produced? What volume will this gas occupy at standard temperature and pressure?


We're here to help

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

MyTutor is part of the IXL family of brands:

© 2025 by IXL Learning