Short Answer

Many industrial reactions are carried out under specific pressure and temperature because these conditions help control the reaction rate and the equilibrium position. By choosing suitable pressure and temperature, industries can increase product yield, reduce energy use, and make reactions proceed faster and more safely.

Specific conditions also help shift equilibrium toward the desired products according to Le Chatelier’s principle. This ensures that large-scale production becomes efficient, economical, and practical, allowing industries to produce chemicals in high amounts within a short time.

Detailed Explanation :

Importance of Specific Pressure and Temperature in Industrial Reactions

Industrial chemical reactions often require controlled conditions to produce chemicals quickly, safely, and in large quantities. Two of the most important factors influencing industrial reactions are pressure and temperature. These conditions determine how fast a reaction proceeds, how much product forms, and how much energy is consumed.

Because industries aim for maximum product yield with minimum cost and time, controlling temperature and pressure becomes essential. These conditions affect both the rate of reaction (speed) and the equilibrium position (product amount) in reversible reactions. The use of specific pressure and temperature also ensures consistent quality, safety, and economic feasibility.

1. Effect on Reaction Rate

Temperature and pressure strongly influence how fast reactants convert into products.

1. a) Temperature and Reaction Rate

• Higher temperatures increase particle energy
• Particles move faster and collide more often
• More collisions have sufficient activation energy
• Reaction rate increases

Industries use higher temperatures when faster reactions are needed.

1. b) Pressure and Reaction Rate

Pressure mainly affects gases.
Higher pressure:

• Brings gas molecules closer
• Increases collision frequency
• Speeds up reactions

Therefore, many gas-based industrial reactions require high pressure to achieve desirable reaction rates.

2. Effect on Equilibrium Position

Many industrial reactions are reversible, and their yield depends on equilibrium.
According to Le Chatelier’s principle, changing temperature or pressure shifts the equilibrium to favour either reactants or products.

1. a) Temperature and Equilibrium

• For exothermic reactions: lower temperature favours product formation
• For endothermic reactions: higher temperature favours product formation

Industries choose the optimum temperature that maximizes yield while keeping reaction speed manageable.

1. b) Pressure and Equilibrium

Pressure affects reactions involving gases.

• Increasing pressure favours the side with fewer gas molecules
• Decreasing pressure favours the side with more gas molecules

Industries use this to shift equilibrium toward the desired product.

3. Industrial Examples Showing Importance of Pressure and Temperature
4. a) Haber Process (Ammonia Production)

N₂ + 3H₂ ⇌ 2NH₃ (exothermic)

• High pressure (200 atm) shifts equilibrium toward ammonia
• Moderate temperature (450°C) provides a balance between speed and yield

Specific conditions make large-scale ammonia production possible.

1. b) Contact Process (Sulphuric Acid Production)

2SO₂ + O₂ ⇌ 2SO₃ (exothermic)

• Lower temperature favours product but slows reaction
• A compromise temperature (~450°C) is used for good speed and yield

1. c) Methanol Production

CO + 2H₂ ⇌ CH₃OH

• High pressure increases methanol yield
• Controlled temperature improves reaction rate

These processes show how industries must choose conditions carefully for efficiency.

4. Energy Efficiency and Cost Control

Heating and pressurising reactors require large amounts of energy.

By selecting specific temperature and pressure:

• Energy waste is reduced
• Costs remain manageable
• Production becomes more sustainable

Industries optimize these conditions to minimize operating expenses while maintaining high output.

5. Safety Considerations

Many industrial reactions become:

• Too slow at low temperature
• Too dangerous at extremely high temperature
• Risky at very high pressures

Therefore, specific and carefully monitored conditions:

• Prevent explosions
• Reduce risk of thermal runaway
• Ensure safe operation of reactors

Safety is a major reason for controlling temperature and pressure precisely.

6. Product Quality and Consistency

Specific conditions ensure that:

• Products form correctly
• Impurities are minimized
• Chemical properties stay consistent

This is especially important for:

• Pharmaceuticals
• Fertilizers
• Plastics
• Petrochemicals

Proper temperature and pressure settings guarantee uniformity across batches.

7. Optimization for Catalysts

Many industrial reactions use catalysts.

Catalysts work best at specific:

• Temperatures
• Pressures

Correct conditions ensure:

• Maximum catalyst efficiency
• Longer catalyst life
• Faster reactions

For example, iron catalyst in the Haber process works best at moderate temperatures.

Conclusion

Industrial reactions are carried out under specific pressure and temperature to control reaction rate, shift equilibrium for higher yield, improve energy efficiency, ensure safety, maintain product quality, and optimize catalyst performance. These carefully selected conditions make large-scale chemical production possible, economical, and safe. Without proper control of temperature and pressure, many essential industrial processes would be slow, unproductive, or too dangerous to operate.