A reaction has an equilibrium constant very much less than 1. Will the reaction proceed spontaneously?
A. Yes, because products are favored and deltaG° < 0.
B. Yes, because reactants are favored and deltaG° > 0.
C. No, because reactants are favored and deltaG° > 0.
D. No, because products are favored and deltaG° < 0.
To determine whether a reaction will proceed spontaneously, we need to consider the value of the equilibrium constant (K) and the sign of the standard Gibbs free energy change (ΔG°).
In this case, the equilibrium constant (K) is very much less than 1, which means that the concentration of the reactants is much higher than that of the products at equilibrium.
When K is small, it indicates that the reaction is reactant-favored, meaning that the reactants are favored at equilibrium.
The sign of the standard Gibbs free energy change (ΔG°) can be used to determine whether a reaction is spontaneous or not. If ΔG° is negative, it means that the reaction is spontaneous and will proceed in the forward direction. If ΔG° is positive, it means that the reaction is non-spontaneous and will not proceed in the forward direction.
Since the question states that the equilibrium constant (K) is very much less than 1, it implies that the reaction is reactant-favored. Therefore, the answer is C. No, because reactants are favored and ΔG° > 0.