Enthalpy

... rather than exergonic/endergonic. I am afraid there is no simple way to show exergonic/endergonic reactions since deltaG is a quantitative sum of enthalpy and entropy. Maybe an explosion would be the best example of an exergonic reaction because it releases heat and increases entropy. Lighting ...

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fyi, the standard enthalpy for creation of element is 0.

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Consider the thermochemical equations given below. C2H4(g) + 3 O2(g) → 2 CO2(g) + 2 H2O(l) ΔH° = −1411 kJ (per mol C2H4) C(s) + 3 H2 (g) + ½ O2(g) → C2H5OH(l) ΔH° = −278 kJ (per mol C) C2H4(g) + H2O(l) → C2H5OH (l) ΔH° = −44 kJ (per mol C2H4) What is ΔH° for the following reaction? All the answers b...

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... molecules in their vicinity. You get some of this entropy back when urea gives up its bound water to interact with the protein and then both the enthalpy and the entropy of the reaction (to be denatured and go into solution) are favorable. So it really is consistent-it just looks inconsistent ...

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Free energy, entropy and enthalpy:

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