Which of these graphs would be a pure isotherm? A #V# vs. #n# graph or a #P# vs. #V# graph?

Why is it not the #V# vs. #n# graph? It was made at constant temperature, wasn't it?

1 Answer
Jul 26, 2017

It can be, but it is also an isobar, so it is not just at constant temperature, but also constant pressure. It is also a mechanically-open system, i.e. it allows transfer of gas in and out so that #n# varies, changing the size of the container (e.g. a balloon).


On the other hand, the #P-V# graph has constant mols of ideal gas and constant temperature, i.e. it follows Boyle's law:

#P_1V_1 = P_2V_2#, constant #n# and #T#

We don't really think about the constant mols of gas in this case, as that can easily be accomplished with a closed system containing a single gas, making this a pure isotherm.

But for the #V-n# graph, according to Avogadro's principle:

#V_1/n_1 = V_2/n_2#, constant #T# and #P#

So, the #V-n# graph is not a pure isotherm, but it does involve constant temperature (and pressure). In this case, mols of gas can vary, and thus the system is not mechanically-closed.