CH3COO-(aq) + H3O+(aq) → CH3COOH + H2O is spontaneous or non spontaneous rxn?
dGo rxn = (n*dGo products) - (n*dGo reactants)
If dGo rxn is negative the rxn is spontaneous.
To determine whether the given reaction is spontaneous or non-spontaneous, we need to consider the direction in which the reaction proceeds under standard conditions. One way to determine this is by looking at the values of standard Gibbs free energy change (ΔG°) for the reaction.
The standard Gibbs free energy change (ΔG°) can be calculated using the equation:
ΔG° = ΔH° - TΔS°
Where:
ΔG° is the standard Gibbs free energy change
ΔH° is the standard enthalpy change
T is the temperature in Kelvin
ΔS° is the standard entropy change
If ΔG° is negative, the reaction is spontaneous in the forward direction. If ΔG° is positive, the reaction is non-spontaneous in the forward direction.
To determine the values of ΔH° and ΔS°, we need to know the enthalpy change (ΔH°) and entropy change (ΔS°) of the reaction. Unfortunately, the information provided in the question doesn't mention these values. Therefore, we cannot calculate the ΔG° and determine the spontaneity of the reaction without this additional information.
In general, however, the reaction given involves the dissociation of a weak acid (CH3COOH) into its conjugate base (CH3COO-) and hydronium ion (H3O+). The forward reaction is typically favored because the backward reaction involves the recombination of the products, which is less probable. Therefore, it is likely that the reaction is spontaneous in the forward direction under normal conditions. But to confirm this, the specific values of ΔH° and ΔS° need to be known.