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Description
Flashcards by Clare Noone, updated more than 1 year ago
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Created by Clare Noone
about 5 years ago
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| Question | Answer |
| What is the word equation for the haber process? | nitrogen(N2)+Hydrogen (3H2)<->ammonia (2NH3) +heat |
| Why is the reaction well suited for an industrial scale? | hydrogen are easy to obtain from air, hydrogen can be obtained from reacting methane with steam to form hydrogen and carbon dioxide, reaction is reversable (eventually reaches dynamic equalibrium) |
| What are the conditions? | pressure=200 atmospheres, temp=450, catalyst= iron |
| What occurs to the ammonia, hydrogen and hitrogen after the haber process? | Ammonia cools in condenser, it turns into a liquid and is removed. Ammonia is used to make ammonium nitrate(nitrogen rich fertiliser). Unused hydrogen and nitrogen are recycled so nothing is wasted. |
| How does temperature affect the rate of the Haber reaction? | forward reaction= exothermic meaning that equilibrium will move towards nitrogen and hydrogen. However lower temps=slower rate. 450C= compromise between max yeild and speed of reaction |
| How does pressure affect the rate of reaction? How can you traditionally speed up the reaction without affecting results. | High pressure= position of equilibrium towards products (4 molecules to two). this maximizes percentage yield and rate of reaction. It is kept at 200 to keep inexpensive and not dangerous. Iron catalyst speeds up without affecting yield. |
| What are the advantages of formulated fertilisers and what three essential elements do they contain? what are they? Clue-never pet Pete | replace missing elements or provide more of them to increase yield and produce bigger and faster. Three main elements they use: nitrogen, phosphorus, potassium |
| What are NPK fertilisers? | formulations containing right percentages of salts of nitrogen, phosphorus, and potassium |
| name two reaction that ammonia is used for to make nitrogen containing compounds: | ammonia can be reacted with oxygen and water to make nitric acid. ammonia can react with acids to form ammonium salts. for example, Ammonia(NH3)+ Nitric acid(HNO3)->Ammonium nitrate (NH4NO3) |
| How is ammonium nitrate used in industry? | carried out in giant vats, high concentrations resulting in very exothermic reaction, heat released is used to evaporate water to make concentrated product of ammonium nitrate |
| How is ammonium nitrate used in the lab? | reaction carried out by titration and crystallization. reactants at low concentrations (less heat produced). After titration it is crystallized slowly(this is why it isn't used in industry) to form ammonium nitrate crystals. |
| What are potassium chloride and potassium sulphate sources of? | potassium- they are mined |
| Why is phosphate rock not useful? How do we make it useful? | phosphate salts are insoluble within the rock so plants cannot directly absorb them as nutrients- they have to be reacted with acids to produce soluble phosphates |
| Give examples of producing soluble phosphate: | react with nitric acid to form phosphoric acid and calcium nitrate, with sulfuric acid to get calcium sulfate and calcium phosphate, with phosphoric acid to produce calcium phosphate |
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