What is the difference between an exergonic reaction and an endergonic reaction?

a.) an exergonic reaction results in a decrease in mass, and an endergonic reaction results in an increase in mass.
b.) an exergonic reaction results in an increase in mass, and an endergonic reaction results in a decrease in mass.
c.) an exergonic reaction involves release of energy, and an endergonic reaction involves absorption of energy.
d.) an exergonic reaction involves an absorption of energy, and an endergonic reaction involves release of energy.

The difference between an exergonic reaction and an endergonic reaction is that an exergonic reaction involves release of energy, while an endergonic reaction involves absorption of energy.

In an exergonic reaction, energy is released to the surroundings. The bonds being formed are stronger than the bonds being broken. In an endergonic reaction, energy is absorbed from the surroundings.

The correct answer between all the choices given is the third choice or letter C. I am hoping that this answer has satisfied your query and it will be able to help you in your endeavor, and if you would like, feel free to ask another question.

answer: the enthalpy of the overall chemical reaction is +87.88 kj or +88 kj.

according to hess's law, the overall enthalpy of a reaction is the difference between the sum of enthalpy values of all the products and the sum of enthalpy values of all the reactants.

δh(reaction) = ∑nδh(products) - ∑nδh(reactants)

δh(reaction) = [δh +δh] - [δh]

δh(reaction) = [1(-287.02) + 1(0) ] - [1(-374.9)] kj = +87.88 kj

here, δh (pcl3) = -287.02 kj, δh(cl2) = 0, δh(pcl5) = -374.9 kj

therefore, enthalpy of the overall reaction is +87.88 kj or +88 kj.

b) mutualism

hope this : )