BackGibbs Free Energy and Equilibrium definitions
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1/14BackSkip to main contentBackGibbs Free Energy
A thermodynamic quantity used to predict if a reaction can occur without external input, reflecting both enthalpy and entropy changes. Spontaneous Reaction
A process that proceeds on its own, increasing disorder and requiring no outside energy to occur. Entropy
A measure of disorder or randomness, with higher values indicating more disordered systems. Delta G
A value representing the change in free energy during a reaction, indicating favorability and direction. Standard Free Energy Change
A reference value for spontaneity, calculated under set temperature and pressure, allowing comparison between reactions. Exergonic Reaction
A process that releases energy, resulting in products with lower free energy than reactants and a negative free energy change. Endergonic Reaction
A process that absorbs energy, producing products with higher free energy than reactants and a positive free energy change. Equilibrium
A state where forward and reverse reactions occur at equal rates, causing no net change in reactant or product concentrations. Equilibrium Constant
A ratio reflecting the relative amounts of products and reactants at equilibrium, used to predict reaction direction. Directionality
The tendency of a reaction to proceed toward either products or reactants, influenced by the equilibrium constant. Steady State
A condition where concentrations of reactants and products remain stable over time, despite ongoing input or output. Thermodynamic Favorability
A characteristic of processes that can occur without external energy, often associated with increased disorder and energy release. Reactant
A starting substance in a chemical process, whose transformation leads to product formation. Product
A substance formed as a result of a chemical process, present after the transformation of reactants.
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