How can the Gibbs energy change of a reaction relate to entropy and enthalpy?
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The Gibbs energy change of a reaction ((\Delta G)) relates to entropy ((\Delta S)) and enthalpy ((\Delta H)) through the Gibbs free energy equation:
[\Delta G = \Delta H - T\Delta S]
Where:
- (\Delta G) is the Gibbs energy change of the reaction.
- (\Delta H) is the enthalpy change of the reaction.
- (T) is the temperature in Kelvin.
- (\Delta S) is the entropy change of the reaction.
This equation demonstrates how the spontaneity of a reaction ((\Delta G < 0) for a spontaneous reaction) is influenced by both the enthalpy and entropy changes. Specifically, if the enthalpy change is negative (exothermic reaction) and the entropy change is positive (increasing disorder), the reaction will be spontaneous at all temperatures. Conversely, if the enthalpy change is positive (endothermic reaction) and the entropy change is negative (decreasing disorder), the reaction will be non-spontaneous at all temperatures. If both the enthalpy and entropy changes have the same sign, the temperature will determine the spontaneity of the reaction.
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When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
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