For a chemical reaction, it is usually found that the reaction rate is faster at higher temperatures. The rate increases because:
(a) The concentrations of reactants increase.
(b) More reactants collide with energy equal to or greater than the activation energy.
(c) The concentrations of products increase.
(d) The volume expands and there is more room for new compounds (products) to form.
Answer (3)
*the correct option here is **B) more reactants collide with energy equal to or greater than the activation energy... ** ** when the molecules collide with each other due to high temperature they gain kinetic energy and the energy required to start the reaction decreases and reaction starts at lower energy at high rate ... ** *
For a chemical reaction, it is usually found that the reaction rate is faster at higher temperature. The rate increases predominantly because more reactants collide with energy equal to or greater than the activation energy. This is due to an increase in the kinetic energy of reactant molecules when temperatures are raised, leading to a higher frequency of collisions and a greater proportion of those collisions that are successful in surmounting the energy barrier to reaction. Thus, the correct answer to the question is:
(b) more reactants collide with energy equal to or greater than the activation energy
Raising the temperature also increases the energy (RT) of molecules, allowing a greater fraction to overcome the activation barrier (Eā), leading to an increased rate constant and thus a faster reaction rate.
The correct answer is (b) "More reactants collide with energy equal to or greater than the activation energy," because higher temperatures lead to greater kinetic energy and more effective collisions in a reaction.
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