Use the graph below to answer the following questions: Free Energy A+B a. I 1 b. Progress of the Reaction The Ea (Energy of activation) without the enzyme The net exergonic release of free energy The Ea (Energy of activation) with the enzyme I C. d. e. C+D C B A
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The lowest amount of energy needed to activate atoms or molecules so they can undergo chemical transformation or physical transport is known as the activation energy.
IMPORTANCE- Chemical reactions have a strong correlation between their activation energy and pace. More specifically, the slower the chemical reaction is, the larger the activation energy is. This is so because molecules cannot start a reaction until they have surpassed the activation energy barrier.
FACTORS AFFECTING- Molecules gather energy and accelerate as the temperature rises. Because of this, it is more likely that molecules will be travelling with the required activation energy for a reaction to occur upon impact at a higher temperature.
An enzyme will bind to a reactant during an enzyme-catalyzed reaction, assisting in the process of turning it into a product. Through a reduction in the activation energy needed, enzymes break down the barriers that ordinarily prohibit chemical reactions from occurring.
MECHANISM OF ACTION-
The reactants must collide with sufficient kinetic energy and in a particular orientation for a chemical reaction to occur. In order to disrupt existing bonds, the reactants must collide with sufficient force. This is the activation energy needed to start the reaction. If the reactants meet at the proper angle, though, less energy is needed.
By giving the reactants better orientation, an enzyme lowers the activation energy required for a reaction to happen, hence speeding up the rate of reaction and increasing the frequency of successful collisions.
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