Reverse Reactions: Standard Enthalpy & Thermodynamics

[dissolver]

If it is thermodynamically favored for a reaction to occur forward and reverse, does that mean that the standard enthalpy of the reaction is close to 0?

 

[Gokul43201]

If it is thermodynamically favored for a reaction to occur forward and reverse, does that mean that the standard enthalpy of the reaction is close to 0?

If the forward and reverse reaction rates are comparable, you will find the the standard Gibbs Free Energy change for the reaction is close to 0.

 

[Blueshift5]

Not necessarily. The thermodynamic favorability of a reaction is determined by the difference in free energy between the reactants and products, not the standard enthalpy. While a reaction with a standard enthalpy close to 0 may be more likely to occur in both directions, it is not a determining factor. Other factors, such as entropy and temperature, also play a role in the thermodynamic favorability of a reaction. Additionally, the standard enthalpy does not take into account the activation energy required for a reaction to occur, which can also affect the direction of the reaction. Therefore, the standard enthalpy alone cannot be used to predict the thermodynamic favorability of a reaction.