Title : Lesson 3 Equilibrium and Industry Learning Objectives: – Review the equilibrium constant experiment from the last lesson – Summarise the impact of equilibrium effects on the Haber Process and the Contact Process – Practise equilibrium exam questions
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Title: Lesson 3 Equilibrium and Industry Learning Objectives: – Review the equilibrium constant experiment from the last lesson – Summarise the impact.
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Title: Lesson 3 Equilibrium and Industry
Learning Objectives:– Review the equilibrium constant experiment from the last
lesson
– Summarise the impact of equilibrium effects on the Haber Process and the Contact Process
– Practise equilibrium exam questions
Main Menu
Recap The diagrams below represent equilibrium
mixtures for the reaction Y + X2 XY + X at 350 K and 550 K respectively. Deduce and explain whether the reaction is exothermic or endothermic.
Y =
5 5 0 K3 5 0 KX = 350K 550K
Main Menu
Recap Dynamic Equilibrium and Le Chatelier’s Principle before you move on…
This lesson…You will be covering Equilibrium and Industry…Industrial processes you have come across before in
IGCSE The Haber Process Sulphuric Acid and The Contact Process
Task for this lesson Read through the slides and watch the videos for ‘The
Haber Process’ and ‘The Contact Process’ Fill out the summary sheet for both reactions Read through the slides on ‘Making Methanol’ Answer the questions on the sheet on Equilibrium and
Industry Complete the SL Equilibrium exam questions
Haber Process
N2(g) + 3H2(g) ⇌ 2NH3(g) ; H = -93 kJ mole-1
= manufacture of ammonia by direct synthesis from nitrogen and hydrogen
N2(g) obtained from atmosphere
H2(g) obtained by thermal cracking of hydrocarbons
In practice, the process carried out at 450C and 20000kPa in the presence of an iron catalyst
Le Chatelier’s Principle suggests NH3(g) production is
favoured by :(1) HIGH pressure since 4 mols 2 mols
(2) LOW temperature since forward reaction exothermic
(3) Removal of NH3 to pull equilibrium to the right and increase the yield