The diagram below represents a spontaneous reaction (deltaG degree

Question

The diagram below represents a spontaneous reaction (ΔG° < 0). Drag the labels to the correct bins.

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Gibbs Free Energy Change Gibbs Free Energy change represents the highest amount of reversible work that can be derived in a reversible system of reaction with constant pressure and temperature. It is directly influenced by the enthalpy, entropy, and temperature changes that occur in the reaction system. The reaction that is spontaneous under the conditions set will exhibit negativity Gibbs Free Energy change.

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Lauren Walsh · Accepted Answer

Concepts and Reason

If the products and reactants have lower energy than the reactants, the reaction is not spontaneous. The reaction can also be spontaneous if the energy of the reactants and products is higher than the energy of the products. The energy of the transition state is greater than that of reactants or products.

Fundamentals

The energy profile diagram shows the energy distribution of the system during reaction.

If the reaction produces less energy than the reactants, then the free energy of the reaction is less that zero [katex]\left( {\Delta {{\rm{G}}^o} < 0} \right)[/katex]

If the reaction occurs in an endothermic state, the reactants will have less energy than their products. In this case, the free energy of the reaction is greater that zero [katex]\left( {\Delta {{\rm{G}}^o} > 0} \right)[/katex]

The energy of reactants is represented by the horizontal portion of the curve on the left, and the energy for products by the horizontal portion of the curve on the right.

The activation energy is the energy difference between transition states and reactants.

The energy difference between products and reactants is called "change in free energy of reaction", which is represented as [katex]\Delta {{\rm{G}}^o}[/katex]

The uncatalyzed reactions are represented by the blue curve, while the catalyzed reactions are represented by the green curve.

Drag the labels as shown in the diagram:

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