Question

A catalyst increases the rate of a reaction because,

A. the added catalyst finds a new lower energy pathway to form products
B. the catalyst increases the collisions between the reactant particles the catalyst provides a new and lower energy pathway to products
C. the catalyst increases the concentration of the reactants
D. the catalyst increases the collisions between the reactant particles
E. the catalyst increases the volume of the reagents

Answer 1

A catalyst increases the rate of a chemical reaction by providing a new and lower energy pathway, lowering the activation energy, and enabling more effective collisions between reactant molecules.

Step-by-step explanation:

A catalyst increases the rate of a reaction by providing a new and lower energy pathway to products. This is achieved by lowering the overall activation energy of the reaction, enabling a greater percentage of reactant molecules to have effective collisions. As a result, the reaction rate increases because there is a higher likelihood of these collisions leading to successful chemical changes. Catalysts do not alter the concentrations of reactants, affect the volume of reagents, or get consumed in the reaction.

In essence, catalysts work by offering an alternative mechanism for the reaction to proceed, which requires less energy than the path the reaction would take in the absence of the catalyst. By doing so, they significantly accelerate the reaction without being altered themselves, which is a crucial aspect of their function in chemical reactions.