Describe in detail what you know about the enthalpy, entropy, and free energy changes when a sample of gas condenses to a liquid. How does temperature affect these changes? (3 points) do not copy from yahoo answers please!!

Question

frostbite · Answer

Depending on your thermodynamics this may come rather easy to you:
The enthalpy:
The enthalpy of vaporization is always positive: $\Delta_{vap}H>0$ and is not that surprising. Using the relation:$$\Large \Delta H ^{\Theta}(A \to B)=-\Delta H ^{\Theta}(B \to A)$$
We may conclude that $\Delta_{con}H<0$

For entropy:
The entropy of a substance changes as a result of changes in the orderliness with which the molecules pack together and the extent to which the energy is localized or dispersed. Mathematically we can account for the entropy change using the relation:
$$\Large \Delta_{con}S=\frac{ \Delta_{con}H }{ T _{con} }$$
We remember from before that $\Delta_{con}H<0$, if we use that information and put it into the equation above we see that: $\Delta_{con}S<0$.

I leave you to think about The Gibbs free energy.

frostbite · Answer

Or want me to explain that as well? We can actually make a fine little graph which explain it quite well.

frostbite · Answer

Increasing temperature we can take when the Gibbs free energy is understood.

frostbite · Answer

I assume you came to the answers?