If we consider a reaction A + B ⟶ C + D, with $\Delta$S $>0$, then regardless of whether $\Delta$H is positive or negative, increasing the temperature will make $\Delta$H - T$\Delta$S more negative, and the reaction will be more feasible
If we now consider a reaction A + B ⇌ C + D, still with $\Delta$S $>0$ for the forward reaction, if we express $ln(K)= -\frac{\Delta H}{RT}+\frac{\Delta S}{R}$, now increasing temperature only makes $ln(K)$ larger if $\Delta H >0$ and is independent of $\Delta S$
Why has the dependence of the feasibility and equilibrium constant of the reaction switched from entropy to ethalpy. Am I confusing a relationship between the feasibility of a reaction itself and the equilibrium constant, i.e. a higher equilibrium constant does not mean the same thing as the forward reaction being more feasible?
