Haber process - ammonia production, manufacturing process
Ammonia is a leading chemical industry in the world. Because ammonia is used to prepare other chemicals and has its uses. In this
tutorial we are going to cover followings.
- Explanation of ammonia
- Manufacturing process of ammonia starting from raw materials
- Uses of ammonia in industry
Explanation of ammonia
Ammonia is compound which has molecular formula of NH3. It is a gas in room temperature. In laboratories, ammonia is as
aqueous ammonium hydroxide (NH4OH) solution. Ammonia is a very toxic compound and have to use it very carefully.
Chemistry of ammonia
Ammonia is a very toxic, sharp suffocating odor, colourless gas. Ammonia is basic gas and it is found as aqueous ammonium hydroxide solution in the laboratory. Ammonia dissolve very well in water.
Manufacturing process of ammonia, Haber process
In this section, we discuss how raw materials are converted to ammonia and what conditions (optimum conditions) should be maintained
to get desired product. Reactions involving in ammonia production is explained with each step.
Raw Materials in Haber process
- Nitrogen Gas - N2(g)
- Hydrogen Gas H2(g)
Extracting raw materials from other sources
- N2(g) is derived from air.
- H2(g) is derived from natural gas
Obtaining nitrogen gas from air
Pressure of air is increased and temperature is increased. Then air can be converted to liquid phase. That liquid air is done fractional
distillation. From this method N2 is separated.
Obtain hydrogen gas from natural gas
- Natural gas is a hydrocarbon mainly containing methane(CH4).
- In our case methane gas is reacted with steam.
- Reaction is done in between 700-1000 0C with help of catalyst.
- This complete reaction is endothermic.
CH4(g) + H2O(g) →
CO(g) + 3H2(g)
CO + H2O(g) →
H2(g) + CO2(g)
Hydrogen and nitrogen reaction
Hydrogen and nitrogen react and give ammonia. But this reaction is a reversible one. After starting the rection, it will start the
backward reaction to give hydrogen and nitrogen. Forward reaction is a exothermic.
- Reversible Reaction
- Needs Catalyst (contain iron in the catalyst)
Catalysts used in haber process
- Iron Oxide. K2O(s) , Al2O3(s) are used as catalyst developers.
- Iron dust. K2O(s) , Mo or Ca are used as catalyst developers.
Forward reaction is a exothermic one. Therefore using low temperature will increase the forward reaction and give higher percentage of
ammonia. But having low temperature will reduce the reaction rate. So, have to wait much time to take the product. By considering both
product amount and production rate, temperature is decided.
4000C - 4500C temperature is applied.
In forward reaction, two molecules are given by reaction four molecules. ( one N2 molecule + three H2 molecules).
Therefore pressure is decreased, volume is decreased. So increasing pressure will bring the reaction more forward (more NH3).
But Equipments which are affordable to high pressure are expensive. Also to generate high pressure, cost is high.
Around 200 atm pressure should be given.
Ammonia preparing reaction
1:3 N2 : H2 volume ratio
Reaction does not come to completeness. Hence there are remaining N2(g) &
H2(g) with NH3(g) in the product. Product is cooled
here. When product is being cooled ammonia becomes to liquid
state from gaseous state. But N2(g) &
H2(g) are in gaseous state.
As the final product liquid ammonia is separated.
Unreacted nitrogen and ammonia is resent to the react.
Equilibrium of hydrogen and nitrogen reaction
Can obtain more ammonia, increasing reactants?
- Excess reactants will bring equilibrium constant to the right. Hence more N2(g) &
H2(g) will give more NH3(g).
- But more reactants will increase the pressure in the reactor.
Therefore affordable devices have to be applied for high pressure. This results high cost.
- And also adding more reactants will cost more money.
Can obtain more ammonia, decreasing temperature?
- Decreasing Temperature means of decrease of Heat in the reactor
- Forward reaction of NH3 production is exothermic reaction.
- Therefore removing heat from the reactor will bring equlibrium constant to the right giving large
- Decrease of heat results decrease of energy in reactants.
- To Happen a reaction, moleculers should have
activaton energy. Otherwise, molecules which have
activation energy will only react.
- Decrease of energy causes decrease of number of molecules which have activation energy.
- Therefore, the reaction rate will fall. It means ammonia product in a unit time (per day ,
per month )will be decreased.
- Manufactures can't wait long time.
- Then very low temperature can't be applied.
Uses of Ammonia
Environmental pollution of Ammonia Industry
- Adding NH3(g) gas into atmosphere will pollute air.
- Ammonia dissolves in water and water become basic.
- Dissolving ammonia in water, water is polluted.
- Due to high temperatures, heat is added to the environment. Temperature of environment will be increased.
- Carbon dust is released to the environment due to obtaining H2 from petroleum.
- If H2 is obtained from NaCl(aq) electrolysis, atmosphere can be polluted by releasing Cl2.
Related tutorials to ammonia production
For urea production
For nitric acid production
Identify ammonia and ammonium salts
Testing ammonia gas