The criterion for whether a reaction proceeds spontaneously is ΔG not ΔG^∘, because ΔG takes int

step 1 Here we're looking at the difference between delta G and delta G with a little degree symbol. I

The criterion for whether a reaction proceeds spontaneously...

Key Concepts

Gibbs Free Energy (?G)

Gibbs free energy is a thermodynamic function that determines the spontaneity of a chemical reaction under non-standard conditions. It combines enthalpy and entropy changes and accounts for the actual concentrations or pressures of reactants and products, allowing one to predict if a reaction will proceed spontaneously in a particular environment.

Standard Gibbs Free Energy (?G°)

Standard Gibbs free energy refers to the change in free energy when a reaction occurs under standard conditions, typically 1 bar pressure and 1 M concentration for all species. It provides a reference point for the energetic favorability of a reaction, but does not account for deviations in reactant or product concentrations that occur in real systems.

Reaction Spontaneity

Reaction spontaneity is determined by the sign and magnitude of the Gibbs free energy change (?G). A negative ?G indicates that a reaction is thermodynamically favorable and will proceed without the need for additional energy input, while a positive ?G signals that the reaction is non-spontaneous under the given conditions.

Effect of Concentration on Reaction Free Energy

The actual Gibbs free energy change (?G) depends on the concentrations of reactants and products as described by the reaction quotient (Q). By incorporating concentration effects through the relationship ?G = ?G° + RT ln Q, this concept explains why a reaction may be spontaneous under non-standard conditions even if the standard free energy change (?G°) suggests otherwise.

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