If the activation energy required for a chemical reaction were reduced, what would happen to the rate of the reaction? a. the rate would increase. b. the rate would decrease. c. the rate would remain the same. d. the rate would go up and down.

The correct answer would be A.The rate would increase.

Activation energy is the minimum or threshold energy required by the particles in order in to start a specific reaction.

If activation energy required for a chemical reaction is reduced then more number of particles can attain that energy easily and thus more number or particles can undergo collisions for a chemical reaction.

Thus, rate of chemical reaction would increase if activation energy is reduced.

If the activation energy required for a chemical reaction were reduced,  the rate of the reaction would increase.

Activation energy in chemistry is the minimum amount of energy that is required to activate atoms or molecules to a condition in which they can undergo chemical transformation or physical transport. The Activation Energy (Ea) also is the energy level that the reactant molecules must overcome before a reaction can occur. The definition of activation energy  given by Svante Arrhenius is the minimum amount of energy that is needed for the chemical reaction to proceed. The source of activation energy is heat with reactant molecules absorbing thermal energy from their surroundings.

The reaction rate decreases with a decrease in temperature. Catalysts can lower the activation energy and increase the reaction rate without being consumed in the reaction. If the amount of the activation energy is decreased then, the reaction would be completed faster.  Factors influenced the reaction rates of chemical reactions are the concentration of reactants, temperature, the physical state of reactants and their dispersion, the solvent, and the presence of a catalyst

Grade:  9

Subject:  biology

Chapter:  activation energy

Keywords:  activation energy