Catalysts

Catalysts

Definition:

• A catalyst is a substance that alters the rate of a chemical reaction without being consumed in the process.

Importance:

• Catalysts play a crucial role in making chemical reactions more efficient and economical.

Lower Temperature Reactions:

• Catalysts enable reactions to occur at lower temperatures than they would without a catalyst.
• This is particularly significant in industry, where energy costs and safety are essential considerations.

Examples of Industrial Catalysts:

• Iron: Used in the Haber Process to manufacture ammonia.
• Platinum: Employed in the Ostwald Process for nitric acid production.
• Rhodium and Platinum: Found in catalytic converters in vehicles to reduce harmful emissions.
• Nickel: Used to harden vegetable oil and make margarine.
• Vanadium (V) Oxide: Applied in the contact process to produce sulfuric acid.

Activation Energy Reduction:

• Adding a catalyst lowers the activation energy required for a reaction.
• This change increases the number of molecules with the minimum kinetic energy necessary for a successful collision.
• As a result, the rate of reaction is enhanced due to a higher number of successful collisions.

Summary:

• Catalysts are substances that accelerate chemical reactions without being consumed. They enable reactions to occur at lower temperatures, making them essential in various industrial processes. Catalysts achieve this by lowering the activation energy barrier, increasing the number of successful

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Catalysts

Summary:

• Catalysts are substances that accelerate chemical reactions without being consumed. They enable reactions to occur at lower temperatures, making them essential in various industrial processes. Catalysts achieve this by lowering the activation energy barrier, increasing the number of successful collisions, and enhancing the rate of reaction.