Final answer:
For a typical reaction, the rate of reaction approximately doubles with every 10 °C rise in temperature, leading to a significant increase in reaction speed with temperature increase.
Step-by-step explanation:
For a typical chemical reaction, the rate of reaction tends to increase as the temperature rises. It is a general rule of thumb that for every 10 °C rise in temperature, the rate of a chemical reaction roughly doubles. This approximate doubling is due to the fact that a higher temperature means molecules have more kinetic energy, thus a greater number of them possess the necessary energy to overcome the activation barrier for the reaction to occur.
This effect can be quite significant, for example, if the temperature of a reaction is raised from 25 °C to 45 °C, the reaction rate would increase by a factor of four, given that it doubles with each 10 °C increase. In cases where the temperature is raised by 20 °C, such as from 25 °C to 45 °C, the reaction would proceed four times faster, as the rate doubles for the first 10 °C increase and then doubles again for the next 10 °C rise.
However, it's important to note that this is a rule of thumb and the actual rate increase can vary based on the specifics of the reaction, including the presence of catalysts, the nature of the reactants, and the reaction conditions.