Final answer:
To calculate the standard Gibbs energy change (ΔG°) and the equilibrium constant (K) for the given reaction, use the equations ΔG° = -RT ln(K) and K = e^(-ΔG°/RT). If ΔG° is negative, the reaction is exergonic (spontaneous), and if it is positive, the reaction is endergonic (non-spontaneous).
Step-by-step explanation:
To calculate the standard Gibbs energy change (ΔG°) and the equilibrium constant (K) for the given reaction, we need to use the equation: ΔG° = -RT ln(K), where R is the ideal gas constant and T is the temperature in Kelvin.
We can use the given values of ΔH° and ΔS° to calculate ΔG°. ΔG° = ΔH° - TΔS°. Then we can rearrange the equation to solve for K: K = e^(-ΔG°/RT).
Based on the calculated value of ΔG°, if it is negative, the reaction is exergonic (spontaneous). If it is positive, the reaction is endergonic (non-spontaneous).