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Does AG´° determine whether a reaction is spontaneous? Why?

Does AG´° determine whether a reaction is spontaneous? Why?

Biochemistry
Biochemistry
9th Edition
ISBN:9781319114671
Author:Lubert Stryer, Jeremy M. Berg, John L. Tymoczko, Gregory J. Gatto Jr.
Publisher:Lubert Stryer, Jeremy M. Berg, John L. Tymoczko, Gregory J. Gatto Jr.
Chapter1: Biochemistry: An Evolving Science
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## Does ΔG°' determine whether a reaction is spontaneous? Why? In the context of thermodynamics and chemical reactions, ΔG°' (the standard Gibbs free energy change) is a crucial metric for determining whether a reaction is spontaneous. ### Factors Affecting Spontaneity 1. **Negative ΔG°' Value**: A reaction is considered spontaneous under standard conditions if ΔG°' is negative. This indicates that the process can occur without external input of energy. 2. **Temperature and Pressure**: Although ΔG°' is measured under standard conditions (298 K and 1 atm), the actual conditions in which the reaction occurs may affect the spontaneity. 3. **Concentration of Reactants and Products**: The actual Gibbs free energy change (ΔG) also depends on the ratio of the concentrations of products to reactants, which is not reflected in the standard state. ### Explanation The spontaneity of a reaction is fundamentally tied to the Gibbs free energy change, which combines the system's enthalpy (ΔH) and entropy (ΔS) changes according to the formula: \[ \Delta G = \Delta H - T\Delta S \] Where T represents the temperature in Kelvin. A negative ΔG indicates that the free energy of the system decreases, allowing the reaction to proceed spontaneously. ### Graphical Interpretation *Although there are no graphs or diagrams presented in the text, a typical graphical representation would often show a plot of Gibbs free energy (ΔG) versus reaction coordinate to visualize the energy changes during the reaction pathway.* In summary, ΔG°' is a key determinant of reaction spontaneity, but actual reaction conditions must be considered for a complete understanding.
Transcribed Image Text:## Does ΔG°' determine whether a reaction is spontaneous? Why? In the context of thermodynamics and chemical reactions, ΔG°' (the standard Gibbs free energy change) is a crucial metric for determining whether a reaction is spontaneous. ### Factors Affecting Spontaneity 1. **Negative ΔG°' Value**: A reaction is considered spontaneous under standard conditions if ΔG°' is negative. This indicates that the process can occur without external input of energy. 2. **Temperature and Pressure**: Although ΔG°' is measured under standard conditions (298 K and 1 atm), the actual conditions in which the reaction occurs may affect the spontaneity. 3. **Concentration of Reactants and Products**: The actual Gibbs free energy change (ΔG) also depends on the ratio of the concentrations of products to reactants, which is not reflected in the standard state. ### Explanation The spontaneity of a reaction is fundamentally tied to the Gibbs free energy change, which combines the system's enthalpy (ΔH) and entropy (ΔS) changes according to the formula: \[ \Delta G = \Delta H - T\Delta S \] Where T represents the temperature in Kelvin. A negative ΔG indicates that the free energy of the system decreases, allowing the reaction to proceed spontaneously. ### Graphical Interpretation *Although there are no graphs or diagrams presented in the text, a typical graphical representation would often show a plot of Gibbs free energy (ΔG) versus reaction coordinate to visualize the energy changes during the reaction pathway.* In summary, ΔG°' is a key determinant of reaction spontaneity, but actual reaction conditions must be considered for a complete understanding.
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