Why is the Haber Process run at 450 °C instead of room temperature?

the forward reaction of the harbour process is exothermic, it gives out heat. so increasing temperature  will shift the equilibrium and decrease the yeild, however increasing the temperature also increases the rate of reaction.

All chemical processes have to compromise between  high rate and high yeild to give the most economical conditions. in this case the high rate turns out to be more economical so a high temerature is used. 

TF
Answered by Tom F. Chemistry tutor

11379 Views

See similar Chemistry GCSE tutors

Related Chemistry GCSE answers

All answers ▸

how is steel stronger than iron?


Describe the effects of increasing the 1)Pressure 2) Temperature of the following system and what effect this will have on the equilibrium position of this reversible reaction given the forward reaction is exothermic 3H2 + N2 <--> 2NH3


What effect will increased temperature have on an equilibrium with a forward reaction which is exothermic?


Explain why chlorine is more reactive than iodine.


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