Which of the following would differ if you compared the same reaction taking place with and without an enzyme
A - the chemical energy of the rectants
B- the chemical energy of the products
C- the energy is required to start the reaction
D- the overall energy reaction
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Yes it is C I agree with @action.jackson11
A catalyst reduces the activation energy of both the forward and reverse reactions by offering an alternative pathway for the reactants. this makes the reaction go faster, i.e. increasing the rate. Because the catalyst reduces the energy for the forward and reverse reactions, it does not change the position of the equilibrium. The catalyst doesn't change anything else other than this so immediately A, and B are wrong. however when considering an un-catalyzed reaction, the activation energy, or energy required to start the reaction will be higher and it will take longer. Remember, energy is needed to make our reaction go, but reactant molecules need to be orinented properly, in addition to having the required kinetic energy average or temperature. The catalyst lowers the energy required to start the reaction C is the best answer. D the overall energy of reaction, is false because you can clearly look at the graph and see that the energy of the reactants and products for the catalyzed vs the uncatalyzed reaction is the same.
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Enzymes are biological catalysts. In the presence of a catalyst, a reaction proceeds via a different route/mechanism that is one of lower activation energy. The activation energy is the minimum energy that molecules have to collide with for there to be a chance for a reaction. Lowering the activation energy means that there will be a greater proportion of molecules with sufficient energy to react and so increasing the rate of reaction. After this boost there is enough energy produced to keep the reaction going (it is self sustained).