Why can an increase in temperature lead to more effective collisions between reactant particles and an increase in the rate of a
chemical reaction? (1) The activation energy of the reaction increases.
(2) The activation energy of the reaction decreases.
(3) The number of molecules with sufficient energy to react increases.
(4) The number of molecules with sufficient energy to react decreases.
Activation energy is the minimum amount of energy required by the reactant molecules to undergo a chemical reaction.
Therefore, when temperature is increased then there will be increase in number of collisions between the reactant molecules. Hence, molecules with lesser energy than the activation energy will also gain energy and thus, they will effectively participate in the chemical reaction.
Hence, we can conclude that an increase in temperature lead to more effective collisions between reactant particles and an increase in the rate of a chemical reaction because the number of molecules with sufficient energy to react increases.
An an increase in
temperature lead to more effective collisions between reactant particles and an
increase in the rate of a chemical reaction because the number of
molecules with sufficient energy to react increases. The answer is number 3.
