Are there gases that cool down as energy is added? If there are, please provide examples. Lee Smolin suggests that there are such gases in his book, Time Reborn, but on searching on my own, I could not find examples, and it seems hard to accept that this is possible.
I am adding the excerpt of the text from the book below to provide more context. 

"Energy would flow from the warm side, cooling it, to the cooler side, warming it, so that soon the temperature is uniform again.  Most systems work this way.  But not all.  Imagine there's a gas that works the other way, cooling down when you add energy to it and heating up when you take energy away.  This may seem counterintuitive, but there are such gases."

 A: With a liberal interpretation of "gas," this is one example: a globular cluster of stars bound together by gravity, where the stars are the "atoms" in this astronomically-sized "gas."  This system has a negative heat capacity, which means adding more energy makes it colder. Heuristically, this is because temperature is related to the average kinetic energy of the "atoms," and adding more energy pushes the "atoms" farther away from each other (statistically speaking), which means they are moving more slowly — just like a satellite in a higher orbit moves more slowly.
For more information, see "On the negative specific heat paradox," http://adsabs.harvard.edu/full/1977MNRAS.181..405L
A: I have never heard of Lee Smolin's book "Time Reborn", but yes gasses can cool down as energy is added. The first law of thermodynamics for a closed system is 
$$\Delta U=Q-W$$
Where $\Delta U$ is the change in internal energy of the gas, $Q$ is the heat added to the gas (energy into the gas), and $W$ is the work done by the gas (energy out of the gas). For an ideal gas, the change in internal energy, $\Delta U$ depends only on the change in temperature and equals $C_{v}\Delta T$. So if the energy added to the gas, in the form of heat, $Q$, is less than the work done by the gas, $W$, the change in internal energy will be negative, meaning the temperature of the gas will drop (cool).
An example is the adiabatic expansion of a gas where $Q=0$. In order to envision an adiabatic expansion of a gas, think about a perfectly thermally insulated cylinder fitted with a piston. The insulation prevents any heat transfer between the gas and the surroundings. The pressure of the gas is greater than the surroundings so that it expands so that it does work. Then $\Delta U=-W$. For an adiabatic  expansion $W$ is positive and therefore $\Delta U$ is negative, meaning the temperature decreases.
Hope this helps.
A: If a volume of gas is much hotter than its surroundings, so that it is radiating heat energy faster than a smaller  amount of heat energy added to it is the only way.
If any gas is at thermal equilibrium with its surroundings, adding heat energy mill raise its temperature per conservation of energy.
