Manufacturing chemicals: making ammonia - C2e

Created by: iram_f
Created on: 25-11-14 20:09

What are the optimum conditions for creating ammonia in the Haber process?

An iron catalyst is needed to speed up the rate of the reaction (it does not affect the yield), a temperature of 450° is required to make the reaction go faster (though this decreases % yield) and pressure of 200 atmospheres increases % yield.

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What is the balanced equation for ammonia?

N2 + 3H2 = 2NH3

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What is ammonia used for?

Ammonia used to be used to make explosives, though is not used so frequently nowadays. 80% of ammonia produced is used for fertilisers, as well as nitric acid or household cleaners.

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What affects the cost of ammonia production?

The cost of the reactants, energy costs (for the temperature and pressure) and pollution-control costs. They must also account for the maintenance of machinery needed for high pressures and ensuring the reaction goes as fast as possible.

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How does the Haber process work?

N2 and H2 are pressurised in the compresser, leading to the reaction vessel where the iron catalyst is. At a temperature of 450° gaseous ammonia is produced and sent to the liquefier. Unreacted N2 and H2 are recycled and sent to the compressor.

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What is a reversible reaction?

A reversible reaction goes in both directions at the same time (in the state of equilibrium).

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Other cards in this set

Card 2

Front

What is the balanced equation for ammonia?

Back

N2 + 3H2 = 2NH3

Card 3

Front

What is ammonia used for?

Back

Card 4

Front

What affects the cost of ammonia production?

Back

Card 5

Front

How does the Haber process work?

Back

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Manufacturing chemicals: making ammonia - C2e