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Describe the differences between the enthalpy and entropy of a chemical reaction.

Enthalpy is the heat energy released or absorbed during a chemical reaction, while entropy is the measure of disorder or randomness.

Enthalpy is a thermodynamic property that measures the heat energy released or absorbed during a chemical reaction. It is represented by the symbol ΔH and is usually measured in kilojoules per mole (kJ/mol). If ΔH is negative, it means that the reaction releases heat energy and is exothermic, while if it is positive, the reaction absorbs heat energy and is endothermic.

Entropy, on the other hand, is a measure of disorder or randomness in a system. It is represented by the symbol ΔS and is usually measured in joules per mole per Kelvin (J/mol.K). If ΔS is positive, it means that the system becomes more disordered, while if it is negative, the system becomes more ordered.

The relationship between enthalpy and entropy is described by the Gibbs free energy equation, which states that the change in free energy (ΔG) is equal to the change in enthalpy (ΔH) minus the temperature (T) multiplied by the change in entropy (ΔS). If ΔG is negative, the reaction is spontaneous and will occur without any external input of energy.

In summary, enthalpy measures the heat energy released or absorbed during a chemical reaction, while entropy measures the disorder or randomness in a system. The relationship between enthalpy and entropy is described by the Gibbs free energy equation, which determines whether a reaction is spontaneous or not.

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