How are reaction rates typically affected by catalysts?

Catalysts are substances that accelerate chemical reactions without being consumed in the process. They achieve this by providing an alternative reaction pathway with a lower activation energy barrier. This means that more molecules have sufficient energy to undergo the reaction, which effectively increases the overall reaction rate.

The presence of a catalyst allows for a greater number of effective collisions between reactant molecules, leading to a higher frequency of successful interactions that result in product formation. As a result, reactions that might otherwise proceed slowly can occur at a significantly faster rate when a catalyst is introduced.

While catalysts do demonstrate varying effectiveness depending on the conditions, they've been shown to enhance reaction rates regardless of temperature, contradicting the notion that they only work at high temperatures. This fundamental understanding is crucial for applications in various fields, such as industrial chemistry, where catalysts are essential for efficient production processes.