The thermodynamic equilibrium constant for the following reaction is 0.15 at 1227°C.
2 SO2(g) + O2(g) 2 SO3(g)
Which is true? Can be more than one answer.
a. The reaction is product-favored.
b. The reaction is reactant-favored.
c. G°is less than zero.
d. G° is greater than zero.
e. G° is equal to zero.
THANKS!
To determine the answer, we need to compare the value of the thermodynamic equilibrium constant (K) to determine if the reaction is product-favored or reactant-favored. The equilibrium constant is defined as the ratio of the concentration of products to the concentration of reactants, each raised to their respective stoichiometric coefficients.
In this case, the given equilibrium constant (K) is 0.15. Since the equilibrium constant is less than 1, it indicates that the concentration of products is lower than the concentration of reactants at equilibrium.
Based on this information, the correct answer is as follows:
b. The reaction is reactant-favored.
Additionally, we can also make inferences about the value of Gibbs free energy change (ΔG°) for this reaction.
Gibbs free energy change is related to the equilibrium constant by the equation:
ΔG° = -RTln(K)
By combining this equation with the given value of K, we can conclude:
c. G° is less than zero
Therefore, both options b and c are true for this question.