Question

Activation energy based concept of enzyme catalysis

Answer 1

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here is your answer...

Let's imagine that you are hiking, and you need to go up a hill to reach the other side. You need to spend some energy going up the hill. The higher the hill, the more energy you need to use to go to the other side.

In biochemical processes, molecules similarly require energy in order to start a reaction. For example, molecules need to have some kinetic energy, or velocity, to collide with other molecules to initiate a reaction. If the collisions don't happen often or don't have enough kinetic energy, no reaction will take place. The energy required to start a reaction is called the activation energy. The lower the activation energy, the faster a reaction happens. The lower the hill you are hiking, the faster you go over to the other side of the hill.  Reactants and products have specific energies. In order to transform the reactants into products, the reactants would have to go through a transition state which is usually higher in energy. To get to this transition state, the system requires the activation energy. Finally, the products reduce their energy to arrive to the final product state.

In this graph we see the plot of energy versus the progress of a reaction. Reactants have higher energy than products. The energy of the reactants increase and then decrease to the final product energy. The highest point in the curve represents the energy of the intermediate state in the reaction. The energy required to achieve the intermediate state is the activation energy of the reaction. Enzymes lower the activation energy of a given reaction, shown by the green curve.

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