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© GCSE Jul-13
PRODUCTION OF AMMONIA NH 3 Millions of tonnes per year
cleaning fluid fertiliser MAKING AMMONIA
RAW MATERIALS N 2 (g) + 3 H 2 (g) 2 NH 3 (g) air methane + steam ammonianitrogenhydrogen © GCSE Jul-13
MAKING AMMONIA N 2 (g) + 3 H 2 (g) 2 NH 3 (g) exothermic endothermic 4 molecules 2 molecules more pressure less pressure © GCSE Jul-13
N 2 (g) + 3 H 2 (g) 2 NH 3 (g) Temperature450ºCLower temperature → more NH 3 Reaction exothermic Higher temperature → faster Compromise between yield & rate Pressure200 atmHigher pressure → more NH 3 4 molecules → 2 molecules Higher pressure → very expensive Compromise between yield & cost CatalystironSpeeds up reaction No effect on yield of NH 3 © GCSE Jul-13
MAKING AMMONIA N 2 (g) + 3 H 2 (g) 2 NH 3 (g) NH 3 is removed by cooling (forms a liquid). Less than 30% yield, so the unreacted H 2 and N 2 are recycled. © GCSE Jul-13
The Haber Process: Making Ammonia L.O: To understand the production of ammonia through the haber process.
Equilibrium &The Haber Process GCSE REVISION. 1. What does Reversible Reaction mean ? A reaction that can proceed in both directions.
Equilibrium &The Haber Process GCSE REVISION. The Haber Process This reaction makes ammonia out of hydrogen and nitrogen. The nitrogen comes from.
AQA Module C2 Reversible Reactions & The Haber Process.
Equilibria in the Real World – The Haber Process Nobel Prize (Chemistry)1918 for the synthesis of ammonia from air. Fritz Haber
Manufacturing ammonia. Fertilisers and much more Global production of ammoniaUses YearTonnes of ammonia
The Haber Process. The Haber process is used to gain ammonia Ammonia is used for: – Plant Fertilliser – Hair Dye.
HABER PROCESS. What is ammonia? It is made industrially by reacting nitrogen with hydrogen in the Haber process. It is a reversible reaction, so it never.
INDUSTRIAL APPLICATIONS Haber process And Contact process.
Version 2.0 Copyright © AQA and its licensors. All rights reserved. C3 3.5 The production of Ammonia.
Unit Industrial Chemistry and Hess’s law. Go to question
Unit 3 Industrial Chemistry and Hess’s law. Go to question In the production of ammonia in the Haber Process, Which is a raw material used.
00:33 Syllabus/Unit: code: C2 Chemical Resources Lesson number: 5 Lesson Title: Manufacturing Chemicals - Ammonia Learning OutcomesHow I didTargets Learning.
Equilibria ⇌. Reversible Reactions In Reversible Reactions the products can react to form the original reactants Equilibrium reactions refer to the forward.
The Haber Process Reversible Reactions and Dynamic Equilibrium.
Write down everything you can think of about this reaction: Nitrogen + Hydrogen ⇌ Ammonia ⇌ reaction is reversible rate of forward reaction = rate of reverse.
Title: Lesson 3 Equilibrium and Industry Learning Objectives: – Review the equilibrium constant experiment from the last lesson – Summarise the impact.
Unit 3 Equilibrium. HIGHER CHEMISTRY REVISION. Unit 3 :- Equilibrium 1. If both potassium iodide solution, KI(aq), and liquid chloroform, CHCl 3 (l),
IC Increasing the yield © Oxford University Press 2011 Increasing the yield.
Making ammonia The Haber process. The Haber process What do we need? Nitrogen – Fractional distillation of air Hydrogen – From natural gas, CH 4 (reforming).
HIGHER CHEMISTRY REVISION. Unit 3 :- Equilibrium 1. If both potassium iodide solution, KI(aq), and liquid chloroform, CHCl 3 (l), are added to a test tube.
Chemistry 1011 Slot 51 Chemistry 1011 TOPIC Gaseous Chemical Equilibrium TEXT REFERENCE Masterton and Hurley Chapter 12.
© Boardworks Ltd of 39. © Boardworks Ltd of 39.
05/05/ Do Chemical Reactions Always Release Energy? Heolddu Comprehensive School.
Manufacturing nitric acid. Mainly fertilisers Global production of nitric acid Around 60,000,000 tonnes of nitric acid are produced annually. However,
Chemical production of ammonia THE HABER PROCESS.
Industrial chemistry Kazem.R.Abdollah (Asiaban) The Haber Process & The Ostwald Process 1.
Chapter 2 Section 3 Go through this power point with your partner, taking notes and discussing the material as you progress through the paper.
Chapter 19 – Production of Ammonia. Properties of Ammonia.
Reversible Reactions and Equilibrium. Mg + 2HCl MgCl 2 + H 2 Irreversible reactions Most Chemical reactions are considered irreversible in that products.
Chapter 16. * Method discovered by German chemist Fritz Haber in * A way to take N 2 from the air and turn it into ammonia. * Previously ammonia.
DYNAMIC EQUILIBRIA. Place 2 cm3 of potassium chromate (VI) solution in a boiling tube and add sodium hydroxide solution until the solution changes colour.
Aim: How is energy related to a phase change? Do Now: 1.Take out your calculator and reference tables. 2.What is the difference between temperature and.
Equilibrium. Non reversible reactions Some chemical and physical reactions occur until one or all the reactants are used up Example 1 Evaporation of water.
16-3: Le Chatelier’s Principle. Le Chatelier’s Principle If a change is made to a system at equilibrium, the rxn will shift in the direction that will.
Liquid nitrogen Group V. Nitrogen and its compounds.
IGCSE CHEMISTRY SECTION 4 LESSON 4. Content The iGCSE Chemistry course Section 1 Principles of Chemistry Section 2 Chemistry of the Elements Section 3.
Le Chatelier’s Principle AP Chemistry. Le Chatelier’s Principle If a stress is applied to a system at equilibrium, the system will change to relieve that.
Factors that Affect Equilibrium Can an equilibrium constant be altered ? What would happen if we changed –The concentration of a reactant or product?concentration.
Temperature and Keq Lesson # 11. How Does Temperature Change the Keq? The Keq is a mathematical constant that does not change for concentration, volume,
Lecture 3411/30/05. Vapor pressure vs. boiling point?
Kinetics Class #4 OB: reactions that are in dynamic equilibrium and how to “push” them forward, or reverse using LeChatelier's Principle.
© Boardworks Ltd 2001 Reversible Reactions and Equilibrium.
IGCSE CHEMISTRY SECTION 5 LESSON 4. Content The iGCSE Chemistry course Section 1 Principles of Chemistry Section 2 Chemistry of the Elements Section 3.
Dynamic Equilibrium. Objectives Describe chemical equilibrium in terms of equilibrium expressions Use equilibrium constants Describe how various factors.
1 of 29© Boardworks Ltd Dynamic Equilibria Learning Objectives: 1.Understand that most reactions are reversible. 2.Understand chemical equilibrium.
The Chemical Industry Fertiliser, Sulphuric Acid, Petrochemical, Pharmaceutical and Chemical Industries The question is how to make a profit from science.
Equilibrium Chemical Equilibrium. General Info on Equilibrium Concerned with how far a reaction goes. Why does it have a low or high % yield? Why do some.
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