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A Which of the following statements is true of an exergonic reaction, but NOT true of an endergonic reaction? View Available Hint(s)A. the potential energy of the products is less than the potential energy of the reactants B. no kinetic energy is released C. activation energy is necessary D. activation energy exceeds net energy release Submit

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Diatonic254

A

The potential energy of the products is less than the potential energy of the reactants is true of an exergonic reaction, but NOT true of an endergonic reaction

Explanation:

In an exergonic reaction, some form of energy is released to the environment during the reaction. Their reaction is thus illustrated with negative free energy in the products side.

The difference in potential energy between the products and the reactants is released into the environment, especially as heat energy, which is why it is an exergonic reaction. Most of the exergonic reactions are spontaneous-which means they do not need activation energy. This is because they favour a decrease in free energy and an increase in entropy according to thermodynamic principles.

Learn More:

For more on exergonic and endergonic reactions check out;

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