Its worth noting that the relationship of temperature and pressure in a gas can be confusing.
I understand it as such and hopefully this will help others to have a better understanding of how they are related.
Molecules in a gas are constantly moving in random directions at random speeds, think of it as a load of balls flying around bashing into each other etc. Now consider increasing the temperature of that gas, the end results are that those molecules are moving at an increased speed.
What is pressure? Its important to understand you cant have pressure unless a you have a container. Pressure then is the effect on the container of all those balls banging against the walls of that container transferring some of their energy to push against the wall. Therefore if you increase temperature those balls are moving faster and hit the walls harder. Again if you add more balls into the container you have more balls banging against the walls.
Another important thing to consider is gas flow. Imagine now that instead of all those gas molecules are moving randomly they band together and charge against a common enemy (albeit still lightly randomly but theres definately a trend) in this case our turbos rotor. This is what the flow of a gas (or liquid is) its just a general trend in those molecules towards moving in one direction.
So you can see now that the ability of a gas/liquid to do work is a function of how many molecules there, how fast they are moving and in what direction.
This is my understanding, I hope it helps others and is in fact correct at least at some level

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Tom