Gibbs Free Energy ($G$) predicts the spontaneity of a reaction at a constant temperature and pressure. A negative $\Delta G$ indicates a spontaneous reaction, while a positive $\Delta G$ indicates a non-spontaneous reaction. The equilibrium constant ($K$) relates the concentrations of reactants and products at equilibrium. Gibbs Free Energy and the equilibrium constant are connected by the equation $\Delta G = -RT\ln{K}$, where $R$ is the ideal gas constant and $T$ is the temperature in Kelvin. Understanding this relationship is crucial for predicting reaction outcomes and equilibrium conditions.
Match the terms with their definitions:
| Term | Definition |
|---|---|
| 1. Gibbs Free Energy | a. The state where the rates of forward and reverse reactions are equal. |
| 2. Equilibrium Constant | b. A measure of the relative amount of reactants and products at equilibrium. |
| 3. Spontaneous Reaction | c. A reaction that occurs without the input of external energy. |
| 4. Non-spontaneous Reaction | d. A thermodynamic potential that measures the 'useful' energy of a system. |
| 5. Equilibrium | e. A reaction that requires the input of external energy to occur. |
(Match the numbers to the letters)
Complete the following paragraph using the words: spontaneous, negative, equilibrium, temperature, positive.
A reaction is considered ________ if its Gibbs Free Energy change ($\Delta G$) is ________. The Gibbs Free Energy change is related to the ________ constant ($K$) and ________ ($T$) by the equation $\Delta G = -RT\ln{K}$. A ________ $\Delta G$ value indicates a non-spontaneous reaction.
Explain how changes in temperature can affect the spontaneity of a reaction, considering the Gibbs Free Energy equation.
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