Question

To calculate the free energy (delta G^0,) of a reaction, you can subtract the free energies of formation (G_f^0) of the reactants from those of the products. Given the following data, what will be true of this reaction? C_6H_12O_6 + O_2 rightarrow CO_2 + H_2O G_f^0: -917.30 -394.4 -237.2 The reaction will not require a catalyst to proceed. The reaction is not balanced, so you cannot calculate the change in free energy. The reaction will be endergonic. The reaction will be exergonic.

Answer 1

To calculate the free energy (ΔG0′) of a reaction, you can subtract the free energies offormation (Gf⁰) of the reactants from those of the products. Given the following data,what will be true of this reaction? C₆H₁₂O₆ + O₂→ CO₂ + H₂O Gf⁰ : -917.30 -394.4 -237.2

Ans: The reaction will be exergonic.

Exergonic Reaction:

• An exergonic reaction may be called a spontaneous reaction or a favorable reaction.
• Exergonic reactions release energy to the surroundings.
• The chemical bonds formed from the reaction are stronger than those that were broken in the reactants.
• The free energy of the system decreases. The change in the standard Gibbs Free Energy (G) of an exergonic reaction is negative (less than 0).
• The change in entropy (S) increases. Another way to look at it is that the disorder of the system increases.
• Exergonic reactions occur spontaneously.