GENERAL KNOWLEDGE

Detailed explanation-1: -An increase in temperature typically increases the rate of reaction. An increase in temperature will raise the average kinetic energy of the reactant molecules. Therefore, a greater proportion of molecules will have the minimum energy necessary for an effective collision (Figure.

Detailed explanation-2: -The activation energy of a chemical reaction is closely related to its rate. Specifically, the higher the activation energy, the slower the chemical reaction will be. This is because molecules can only complete the reaction once they have reached the top of the activation energy barrier.

Detailed explanation-3: -No it doesn’t. This is a huge misconception that High Schoolers have. The temperature increase increases the number of collisions in the container, which makes the reaction faster. The only way to lower down the activation energy is by using catalysts which lower down the Activation energy of the reaction.

Detailed explanation-4: -When temperature increases, the kinetic energy of molecules increases. The molecules move around faster and collide with each other more often, thus increasing the probability of the reaction occurring. This increases the reaction rate.