Equilbria and Industry QUIZ!! QUESTION one. Write the equation for the reaction for the production of methanol.

Equilbria and Industry QUIZ!! QUESTION two. State 3 uses of ammonia.

Equilbria and Industry QUIZ!! QUESTION three. Give 2 sets of reactants used for making ethanol.

Equilbria and Industry QUIZ!! QUESTION four. Name the 3 different catalysts used in each of the 3 industrial processes you have investigated.

Equilbria and Industry QUIZ!! QUESTION five. All 3 processes are endothermic. True or false.

Equilbria and Industry QUIZ!! QUESTION six. Le Chatelier states that using a low temperature will achieve highest yields in all 3 processes. What happens in reality and why?

Equilbria and Industry QUIZ!! QUESTION seven. What would the ideal pressure be for the production of ethanol? What pressure is actually used?

Equilbria and Industry QUIZ!! QUESTION eight. State 3 uses of methanol and/or ethanol.

Equilbria and Industry QUIZ!! QUESTION nine. Write the equation for the hydration reaction.

Equilbria and Industry QUIZ!! QUESTION ten. In ethanol and ammonia production and how is waste reduced and yield increased?

Equilbria and Industry QUIZ!! QUESTION one. Write the equation for the reaction for the production of methanol. CO(g) + 2H2(g) ⇋ CH3OH(g)

Equilbria and Industry QUIZ!! QUESTION two. State 3 uses of ammonia. Fertiliser, explosives, nylon

Equilbria and Industry QUIZ!! QUESTION three. Give 2 sets of reactants used for making ethanol. 1) glucose (and yeast – technically an enzyme) 2) ethene and water vapour (steam)

Equilbria and Industry QUIZ!! QUESTION four. Name the 3 different catalysts used in each of the 3 industrial processes you have investigated. 1. methanol – copper/zinc oxide/alumina mixture 2. ethanol – phosphoric acid on silica (H3PO4) 3. ammonia – iron (with a potassium hydroxide promoter)

Equilbria and Industry QUIZ!! QUESTION five. All 3 processes are endothermic true or false. FALSE (they are all exothermic)

Equilbria and Industry QUIZ!! QUESTION six. Le Chatelier states that using a low temperature will achieve highest yields in all 3 processes. What happens in reality and why? In reality moderate to high temperatures are used as otherwise the rate of reaction will be too slow and it will take too long to make the products, not economically viable. Methanol: 500K Ethanol: 570K Ammonia: 670K

Equilbria and Industry QUIZ!! QUESTION seven. What would the ideal pressure be for the production of ethanol? What pressure is actually used? Le Chatelier states that high pressure would shift the equilibrium to the right and increase products. Moderately high pressure is used (6500kPa) because it is too expensive to maintain and to produce strong equipment to withstand it. High pressure cause polymerisation and polythene is made which could block equipment.

Equilbria and Industry QUIZ!! QUESTION eight. State 3 uses of methanol and/or ethanol. Methanol: Fuel, feedstock e.g. to make methanal (formaldehyde) that can produce plastic, explosives, glues, paints) Ethanol: Fuel, drinks, solvents in cosmetics e.g. perfume, drug manufacture.

Equilbria and Industry QUIZ!! QUESTION nine. Write the equation for the hydration reaction. C2H4(g) + H2O(g) ⇌ C2H5OH(g)

Equilbria and Industry QUIZ!! QUESTION ten. In ethanol and ammonia production how is waste reduced and yield increased? Reactants are recycled into the system. Ethene gas in ethanol production increases yield from 5% to 95%. Nitrogen and hydrogen gas in the Haber Process.

Fun Facts! In the USA ethanol production has increased by 3700% in the last 30 years. Largely as bioethanol for fuels. As a rule pure methanol must be used to fuel monster trucks and indy cars. Haber was the first to suggest the use of poisonous gases to kill troops during WW1. He was “essentially the Father of Chemical Warfare” and was considered a war criminal by the allies, despite being given a Nobel Prize for production of fertiliser.

Equilibria and Industry To answer these given questions: What are the reagents? What are the products? Draw up the equation for the reaction. What are the conditions used for the reaction? Is there any compromise from the Principle rules? What are the main uses of the product? Fun facts!? :)

Methanol Production What are the reagents? Carbon monoxide gas and hydrogen gas What are the products? Methanol gas Draw up the equation for the reaction. CO(g) + 2H2(g) <> CH3OH(g) ∆H= -90kJmol-1 What are the conditions used for the reaction? T: 500K P: 5-10 x 103 kPa catalyst: combination of copper, zinc oxide and alumina (Al2O3) What are the main uses of the product? Fuel mixtures, a feedstock:oxidised to methanal (formaldehyde) which can to make glues. paints, plastics and explosives. Fun fact: Pure methanol is required by rule to be used in Champcars, Monster Trucks, USAC sprint cars... any methanol fire can be put out with water.

Methanol Production CO(g) + 2H2(g) <> CH3OH(g) ∆H= -90kJmol-1 Is there any compromise from the Principle rules? Le Chatelier states: PRESSURE: If we have high pressure the reaction will shift to the right and favour products. In reality pressures are fairly high but very high pressures are expensive. TEMPERATURE: If we have low temperatures the reaction will shift to the right and favour products. In reality higher temperature and a catalyst are used to increase the rate and make the production more efficient and economically viable. Yield: 5-10%

Ethanol Production What are the reagents? 2 methods: a) fermentation: glucose solution b) hydration: ethene and water vapour What are the products? a) ethanol solution and carbon dioxide b) ethanol gas Draw up the equation for the reaction. a) C6H12O6 (aq) >yeast> 2C2H5OH (aq) + 2CO2 (g) this is not a reversible reaction b) C2H4(g) + H2O(g) <> C2H5OH(g) ∆H = -46kJmol-1 What are the conditions used for the reaction? (b only) T:570K P: 6500kPa catalyst: H3PO4 (phosphoric acid) absorbed on silica What are the main uses of the product? Solvent in cosmetics, fuel, alcohol we drink, drugs and detergents. Fun facts!? :) In the USA ethanol production has increased by 3700% in the last 30 years. This is largely due to bioethanol production and used in fuel.

Ethanol Production Is there any compromise from the Principle rules? Le Chatelier states: PRESSURE: If we have high pressure the equilibrium will shift to the right and favour products. In reality the pressure isn't that high, this is because it is expensive to produce the pressure and to produce the factory equipment strong enough to withstand it. If pressure is too high polymerisation occurs and polythene is made which could clog up the plant. TEMPERATURE: If we have low temperature the equilibrium will shift to the right and favour products. In reality moderate temperatures are used as otherwise the rate of the reaction will be too slow and therefore not economical. Yield: 5% (but the recycling of ethene means that actually 95% conversion is achieved)

Ethanol Production PROPORTIONS OF REACTANTS: If we add more water vapour (cheap) the equilibrium will shift to the right and favour the product. In reality this dilutes the catalyst and prevents it from working, more ethene is actually used even though this is more expensive, actually the unreacted ethene is recycled round the system and is not wasted.

The Haber Process What are the reagents? Nitrogen gas and hydrogen gas What are the products? Ammonia gas Draw up the equation for the reaction. N2(g) + 3H2(g) <> 2NH3(g) ∆H = -92kJmol-1 What are the conditions used for the reaction? T: 670K P: 20,000kPa catalyst: iron What are the main uses of the product? 80% of the ammonia manufactured is used as a fertiliser. Explosives, drugs, dyes and nylon. Fun (?) facts!? :) Haber was the first to suggest the use of poisonous gases to kill troops during WW1. He was “essentially the Father of Chemical Warfare” and was considered a war criminal by the allies, despite being given a Nobel Prize for production of fertiliser.

The Haber Process Is there any compromise from the Principle rules? Le Chatelier states: PRESSURE: If we have high pressure the equilibrium will shift to the right and favour the product. In reality the pressure is high but not as high as it could be to produce more product. This is because it is expensive to produce the pressure and to produce the factory equipment strong enough to withstand it. TEMPERATURE: If we have low temperature the equilibrium will shift to the right and favour the product. In reality the temperature used is high, this is because a lower temperature would reduce the rate and therefore not produce the ammonia efficiently. Yield: 15% To make the reaction more cost effective the nitrogen and hydrogen gases are recycled.