How does a catalyst speed a reaction at low temperatures? It raises the amount of energy required to break chemical bonds. It lowers the amount of energy required to break chemical bonds. It increases the concentration of the reactant particles.

When solids and liquids react, increasing the surface area of the solid will increase the reaction rate. The reaction rate decreases with a decrease in temperature. Catalysts can lower the activation energy and increase the reaction rate without being consumed in the reaction.

The temperature changes the amount of energy the particles have. Increasing the temperature will mean there are more particles with high energy, greater than the activation energy, so a higher chance of a successful reaction. This means that an increase in temperature will increase the rate.

A catalyst is a substance that can be added to a reaction to increase the reaction rate without getting consumed in the process. Catalysts typically speed up a reaction by reducing the activation energy or changing the reaction mechanism.

A Catalyst is a substance which changes the reaction rate without affecting the overall energetics of the reaction or undergoing any chemical reaction. The Catalyst is used to change the reaction rates (kinetics) without changing the reaction products. Therefore, the catalyst does not alter the Gibbs free energy.

Because the purpose of a catalyst is to speed up the same slower reaction without changing what products are made. Otherwise it is a different reaction altogether. At that point it becomes a entirely different reaction, which is not the goal of using a catalyst.