Which reaction is more energetically favored, one with ΔG^∘=-44 kJ / mol or one with ΔG^∘=+44

step 1 So in this question, we're asked to determine which reaction would be more energetically favored

Which reaction is more energetically favored, one with...

Labs

Want to see this concept in action?

NEW

Explore this concept interactively to see how it behaves as you change inputs.

View Labs

Key Concepts

Gibbs Free Energy

Gibbs free energy is a thermodynamic function that indicates the amount of useful work obtainable from a chemical reaction at constant temperature and pressure. It integrates enthalpy and entropy changes, effectively predicting whether a process will occur spontaneously. A negative ?G indicates that the process can occur without external input, while a positive ?G suggests that the process is non-spontaneous under standard conditions.

Reaction Spontaneity

Reaction spontaneity refers to the tendency of a chemical process to occur on its own without continual energy input. In thermodynamic terms, a reaction is spontaneous if the change in Gibbs free energy (?G) is negative, meaning the reaction is energetically favored and can proceed naturally. Conversely, a positive ?G reflects a non-spontaneous reaction that requires additional energy to drive it forward.

Exergonic and Endergonic Reactions

Exergonic reactions are those that release energy and have a negative ?G, indicating that they are thermodynamically favorable. Endergonic reactions, by contrast, absorb energy and are characterized by a positive ?G, meaning that energy must be invested for the reaction to occur. This distinction is essential for understanding the energy profile and feasibility of chemical reactions.

Transcript

Please give Ace some feedback