Negative Enthalpy
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Re: Negative Enthalpy
Spontaneous reactions depend on whether or not the delta G is negative; since the equation for delta G is
deltaH-T(deltaS), then if the enthalpy is positive you can still have a negative delta G (and a spontaneous reaction) if the absolute value of T(deltaS) is greater than the enthalpy change
deltaH-T(deltaS), then if the enthalpy is positive you can still have a negative delta G (and a spontaneous reaction) if the absolute value of T(deltaS) is greater than the enthalpy change
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Re: Negative Enthalpy
They do not necessarily happen by themselves since enthalpy is a state function. It depends on the intermediate energy when going from the initial enthalpy to the final enthalpy.
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