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  • If Gibbs Free Energy (ΔG) is zero thenOption: 1 the reaction has reached non-equilibriumOption: 2

If Gibbs Free Energy (ΔG) is zero then

Option: 1

the reaction has reached non-equilibrium


Option: 2

the reaction has reached equilibrium


Option: 3

the reaction has started


Option: 4

the reaction has stopped


Answers (1)

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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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If Gibbs Free Energy(\Delta G) is zero, the reaction has reached equilibrium.

Posted by

Devendra Khairwa

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