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Positive ΔG implies
Option: 1
endergonic and spontaneous reaction

Option: 2
exergonic and non-spontaneous reaction

Option: 3
endergonic and non-spontaneous reaction

Option: 4
All of these

Answers (1)

best_answer

Gibbs Free Energy (ΔG):

Gibbs Free Energy (ΔG) is the amount of energy that can be used in a particular reaction.
A chemical reaction is said to be exergonic and spontaneous if the Gibbs Free Energy (ΔG) is negative.
A chemical reaction is said to be endergonic and non-spontaneous if the Gibbs Free Energy (ΔG) is positive.
Gibbs Free Energy (ΔG) of a reaction is negative when Gibbs Free Energy (ΔG) of products is less than that of reactants.
Gibbs Free Energy (ΔG) solely depends on the energy of the reactants and products and is not dependent on the pathway of the reaction.
If Gibbs Free Energy (ΔG) is zero, the reaction has reached equilibrium.
Gibbs Free Energy (ΔG) is not affected by enzymes.

The following graph shows the exergonic and endergonic reactions.

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A chemical reaction is said to be endergonic and non-spontaneous if the Gibbs Free Energy $(\Delta G)$ is positive.

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