How does a 10°C increase in temperature typically affect the rate of a chemical reaction?

A 10°C increase in temperature typically leads to an increase in the rate of a chemical reaction, and it is generally observed that for many reactions, the rate can approximately double with every 10°C rise in temperature. This relationship exists because higher temperatures provide more energy to the reactant molecules, leading to more frequent and more energetic collisions. As more molecules reach the activation energy needed for a reaction to occur, the overall reaction rate increases.

It's important to note that this doubling effect is a general rule of thumb and can vary between different reactions. However, this principle underlies many biochemical and chemical processes, which is why an increase in temperature often results in a significant increase in reaction rates. In contrast, other options imply decreases or neutral effects on reaction rates, which do not align with the established understanding of the relationship between temperature and reaction kinetics.