Respuesta :
Answer:
C) at equilibrium, the concentration of C will be much greater than the concentration of A or B.
Explanation:
A + B ⇌ C; ΔG° = -20 kJ·mol⁻¹
If ΔG is negative, the reaction is spontaneous and position of equilibrium lies to the right, so the equilibrium concentration of C is much greater than that of A or B.
A) is wrong. The molar ratio of A:B is 1:1. If their initial concentrations are 1 mol·L⁻¹, their final concentrations will be equal.
B) is wrong. The position of equilibrium lies to the right, so the concentration of C will be much greater than that of A.
D) and E) are wrong. ΔG says nothing about the rate of a reaction. It deals with the spontaneity and position of equilibrium not the speed at which equilibrium is achieved.
The value of [tex]\Delta[/tex]G has been negative, thus the concentration of C has been much higher than the concentration of A or B at equilibrium has been correct. Thus, option C is correct.
Gibb's free energy has been defined as the rate of the reversible reaction. The negative value of Gibbs free energy results in the reaction being spontaneous, and the rate of formation of the product has been higher than the rate of dissociation.
The given reaction has a value of [tex]\Delta[/tex]G been -20 kJ/mol. The negative sign indicates that the rate of the formation of C has been greater than the rate of dissociation of C.
Thus, statement C stating that the concentration of C has been much higher than the concentration of A or B at equilibrium has been correct. Thus, option C is correct.
For more information about Gibbs free energy, refer to the link:
https://brainly.com/question/9552459
