For a reaction in a sealed, rigid container, $\Delta$H is always greater than $\Delta$E.

Question

Quizplus · Accepted Answer

The given reaction is F1F1F1S1F1F1F10H <=> F1F1F1S1F1F1F10E. The equilibrium constant for this reaction depends on the difference in Gibbs free energy between the products and the reactants, given by the equation ΔG = ΔH - TΔS, where ΔH is the enthalpy change, ΔS is the entropy change, and T is the temperature. 
If ΔH is larger than TΔS, then ΔG will be negative, and the reaction will favor the products. Conversely, if ΔH is smaller than TΔS, then ΔG will be positive, and the reaction will favor the reactants. 
The question states that the container is sealed and rigid, which means that the volume and pressure of the system are constant. If one product (H) is more volatile than the other (E), then the system will favor the less volatile product (E), resulting in a lower value of ΔG for the reaction that produces E. Therefore, F1F1F1S1F1F1F10E should have a larger equilibrium constant (and a more negative ΔG) than F1F1F1S1F1F1F10H.

For a Reaction in a Sealed, Rigid Container Δ\DeltaΔ H Is Always Greater Than

For a Reaction in a Sealed, Rigid Container $\Delta$ H Is Always Greater Than