Question

3.1 Why does the rate of most reactions increase with increasing temperature?

​

Answer 1

Answer:

Increasing the temperature a reaction takes place at increases the rate of reaction. At higher temperatures, particles can collide more often and with more energy, which makes the reaction take place more quickly.

Answer 2

Answer:

As on increasing temperature, the energy of gases increases, so a larger fraction of colliding particles can cross the energy barrier (i.e., the activation energy ), which leads to an increase in rate.

Step-by-step explanation:

For a collision to be effective, the colloiding molecules must have energy more than a particular value known as threshold energy. At room temperature most of the reactant molecules have energy less than the threshold value. When temperature is increased, the reactant molecules absorb this energy and their energy becomes equal to or greater than threshold value. This extra amount of energy absorbed by the reacting molecules is known as activation energy.

Activation energy Threshold energy Average kinetic energy of the reactants.

Evidently, the rate of reaction increases on rise in temperature, because average kinetic energy of the reactants increases and activation energy decreases. Also, on rise in temperature, the number of molecules having kinetic energy greater than threshold value increases. Thus, the increase in the rate of reaction with increase in temperature in mainly due to increase in number of effective collisions.

Please Mark Me as Brainliest!!!