Gibbs Free Energy (G) is pivotal in determining the spontaneity of chemical reactions, with its change (ΔG) indicating whether a process is spontaneous, non-spontaneous, or at equilibrium. Chemical equilibrium, described by the equilibrium constant (K), is influenced by pressure and temperature changes, as explained by Le Chatelier's Principle. These concepts are crucial in real-world applications like photosynthesis and the Haber process, where manipulating conditions can optimize yields and efficiency.
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Gibbs Free Energy is a thermodynamic quantity that measures the maximum amount of reversible work that can be performed by a system at constant temperature and pressure
Equation for Change in Gibbs Free Energy
The change in Gibbs Free Energy (ΔG) is defined by the equation ΔG = ΔH - TΔS, where ΔH is the change in enthalpy, T is the absolute temperature, and ΔS is the change in entropy
Significance of ΔG
The sign of ΔG determines the spontaneity of a chemical reaction, with a negative ΔG indicating a spontaneous process, a positive ΔG suggesting a non-spontaneous process, and a ΔG of zero denoting a system in equilibrium
Changes in pressure can affect the Gibbs Free Energy of a system, particularly in reactions involving gases, according to Le Chatelier's Principle
Chemical equilibrium is a condition in which the rate of the forward reaction equals the rate of the reverse reaction, resulting in no net change in the concentrations of reactants and products
Definition of Equilibrium Constant
The equilibrium constant (K) is the ratio of the concentrations of products to reactants, each raised to the power of their stoichiometric coefficients, and is a quantitative measure of the position of equilibrium
Relationship between K and ΔG°
The standard Gibbs Free Energy change (ΔG°) is related to the equilibrium constant (K) by the equation ΔG° = -RT ln(K), with a negative ΔG° corresponding to a larger K value and a greater concentration of products at equilibrium
Le Chatelier's Principle explains how a system at equilibrium responds to changes in conditions, such as pressure, temperature, or concentration, by shifting the equilibrium position to minimize the imposed change
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Definition of Gibbs Free Energy (G)
Thermodynamic quantity measuring max reversible work at constant temperature and pressure.
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Gibbs Free Energy equation components
ΔG = ΔH - TΔS, where ΔH is enthalpy change, T is absolute temperature, ΔS is entropy change.
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ΔG of zero meaning
Indicates a system in equilibrium, no net change in free energy.
