Haber process

The Haber process is a process used to produce the useful substance ammonia from nitrogen and hydrogen.

Sources of gases

Hydrogen

Hydrogen is only found in the air in the form of water vapour, as if there was more hydorgen gas, it would react with the oxygen, forming water. However, the reverse reaction can be used to form hydrogen: the electrolysis of water. Also, a fuel processor can be used to extract the hydrogen from methane (natural gas).

Electrolysis of water

Pure water is a poor conductor of electricity, so often a soluble ionic compound is added, such as an acid, base or salt. Sulphuric acid (H₂SO₄) is often used because it is fully dissociated when dissolved in water, and is difficult to oxidise, so oxygen gas will form at the anode..

Only some water molecules form an oxide and a hydroxide ion, meaning that water is only partially ionised and hence a poor conductor of electricity.

H₂O _(l) → H⁺ + OH^-

Sulphuric acid, on the other hand, is fully ionised when dissolved in water:

H₂SO_{4 (aq)} → 2H⁺ + SO₄^2-

Once electrolysis has begun, the hydrogen ions move towards the cathose where they are reduced to form hydrogen gas:

2H⁺ + 2e^- → H_{2 (g)}

At the anode, each water splits into an oxygen ion and 2 hydrogen ions. Every pair of oxygen ions forms a covalent bond, forming a molecule of oxygen gas, which bubbles off.

H₂O → O^2- + 2H⁺ + 2e^-

2O^2- → O_{2 (g)}

For every two electrons passed, 2 hydrogen ions form a molecule of hydrogen gas at the cathode, but another 2 hydrogen ions are formed at the anode. The sulphate ions stay in solution throughout the reaction, meaning that overall, the amount of sulphuric acid remains constant, and it is the water that is electrolysed:

4H⁺ + 2H₂O _(l) → 2H_{2 (g)} + O_{2 (g)} + 4H⁺

Or, more simply:

2H₂O _(l) → 2H_{2 (g)} + O_{2 (g)}

Fuel processor

Also known as a fuel reformer, a fuel processor extracts hydrogen from hydrocarbons, such as methanol and methane (natural gas).

Reforming methanol

The reforming of methanol involves mixing liquid methanol with water, and then using a catalyst to help break down the methanol molecules into carbon monoxide and hydrogen. The water than reacts with the carbon monoxide to produce carbon dioxide and more hydrogen:

CH₃OH _(l) → CO _(g) + 2H_{2 (g)}

CO _(g) + H₂O _(g) → CO_{2 (g)} + H_{2 (g)}

So, overall:

CH₃OH _(l) + H₂O _(l) → CO_{2 (g)} + 3H₂

Reforming methane

Methane is reacted with water to form carbon dioxide and hydrogen:

CH_{4 (g)} + H₂O _(l) → CO + H_{2 (g)} + H_{2 (g)}

Just as with reforming methanol, the carbon monoxide produced reacts with water to form carbon monoxide and more hydrogen:

CO _(g) + H₂O → CO_{2 (g)} + H₂O _(l)

So, overall:

CH_{4 (g)} + 2H₂O _(l) → CO_{2 (g)} + 4H₂O _(l)

Nitrogen

Nitrogen is by far the most abundant gas in the Earth's atmosphere, making up 78.084% of the air we breathe. It is from the air that nitrogen is normally collected.

Reaction

The reaction between nitrogen and hydgrogen gases is reversible , meaning that some ammonium will be formed, but not all with react. The yield of ammonia depends upon the conditions: temperature, pressure and the presence of a catalyst.

N_{2 (g)} + 3H_{2 (g)} ↔ 2NH_{3 (g)}

Le Chatelier's principle explains the effects of changing the temperature and pressure on a reversible reaction, as well as showing the effects of a catalyst.

Temperature

Increasing the temperature breaks bonds apart, so increasing the temperature will force the equilibrium to the side with more molecules, thus decreasing the yield of ammonia. Furthermore, the higher the temperature, the higher the cost and also the higher the danger, so factory owners may not wish to make the temperature too high for economic and safety considerations. However, increasing the temperature will mean that the particles have more energy, so the rate of reaction will increase, so the ammonia will be made more quickly. In industry, the Haber process is usually carried out at a "compromise temperature" of between 400°C and 450°C.

Pressure

Increasing the pressure will cause the particles to be compressed together more. This means that the equilibrium will be forced to the side with fewer molecules, so the yield will increase. Higher pressures will also increase the rate of reaction, so the ammonia will be produced quicker. However, creating and maintaining a high pressure is very expensive, thus factory owners must find a "compromise pressure". In industry, this is about 200 atmospheres.

Catalyst

A catalyst is a substance that lowers the activation energy required for a reaction to take place. In a reversible reaction, a catalyst will have no effect on the direction of the reaction, but instead makes it reach equilibrium more quickly. Catalysts are used as they do not get used up, thus they only need to be bought once, and allow more ammonia to be produced in a fixed period of time, increasing the efficiency of the factory.

Industry

The Haber process is still used today to make ammonia. In 2000, production of ammonia was at record levels of 130 million tonnes . 22% was made in China and 15% was from North America . Prices are expected to increase due to the rising prices of methane, which is used to produce the hydrogen used in the process .

Uses of ammonia

• Manufacture of nitric acid
• Manufacture of ammonium nitrate, a fertilizer
• Explosives

See also

• Ammonia
• Ammonium
• Hydrogen
• Le Chatelier
• Nitric acid
• Nitrogen
• Reversible reaction