g The free energy change of the reaction A (g) ---> B(g) is zero under certain conditions. The STANDARD Free energy change of the reaction is -42.5 kJ. Which of the following statements must be true about the reaction described here? A) The concentration of the product is greater than the concentration of the reactant. B) The reaction is at equilibrium. C) The concentration of the reactant is greater than the concentration of the product.

In thermodynamics, the Gibbs free energy is a term used traditionally to refer to the available or useful work that can be obtained from a thermodynamic system.

Gibbs free energy is a measure of the chemical potential that a reaction has left to do work. Hence, if the free energy is zero, then the reaction has attained equilibrium, and there is no more work to be done

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andromache andromache · Answer 2 · 2022-04-07T13:48:05+02:00

The statement that should be true related to the reaction should be that it should be at equilibrium.

What is Gibbs free energy?

In terms of thermodynamics, this energy should be applied for the availability or the useful work that should be obtained via the system of thermodynamics.

Also, it determined the chemical potential where the reaction has left for doing the work. Also in the case when the free energy should be zero so here the reaction should be attained the equilibrium.

hence, the option b is correct.

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