Question

Calculate the standard Gibbs energy of the reaction CO(g) +CH3OH(l)→CH3COOH(l) at 298 K, from the standard entropies and enthalpies of formation given in the Data section.

Answer 1

To calculate the standard Gibbs energy (ΔG°) of a reaction, subtract the product of temperature and the standard entropy change (ΔS°) from the standard enthalpy change (ΔH°). If ΔG° is negative, the reaction is spontaneous; if ΔG° is positive, the reaction is nonspontaneous.

Step-by-step explanation:

To calculate the standard Gibbs energy (ΔG°) of the reaction CO(g) + CH3OH(l) → CH3COOH(l) at 298 K, you can use the equation ΔG° = ΔH° - TΔS°.

First, find the ΔH° and ΔS° values of the reaction from the standard enthalpies and entropies of formation given in the Data section. Then, plug those values into the equation and calculate ΔG°.

Finally, determine the spontaneity of the reaction based on the sign of ΔG°. If ΔG° is negative, the reaction is spontaneous; if ΔG° is positive, the reaction is nonspontaneous.