False. Increasing the concentration of a reactant does not lower the activation energy of the reaction. The activation energy is the minimum amount of energy required for a chemical reaction to occur. It is a characteristic of the reaction itself and is determined by the specific reactants and the reaction pathway.
However, increasing the concentration of a reactant can increase the rate of the reaction. This is because a higher concentration means more reactant molecules are present in a given volume, leading to more frequent collisions between reactant molecules. More collisions increase the likelihood of successful collisions that result in the formation of products, thereby speeding up the reaction.
In summary, while increasing the concentration of a reactant can affect the reaction rate, it does not change the activation energy required for the reaction to proceed.