Why don't all gasses have infinite entropy? [duplicate]

Entropy of an ideal gas is defined as the logarithm of the number of possible states the gas can have multiplied by Boltzmann's constant:

$$S=k_{\mathrm {B} }\log \Omega .}$$

In deriving the Maxwell-Boltzmann distribution, we initially start by counting a finite number of states, so this definition of entropy makes sense. But in the end we say that the number of possible states is so high that we can acctually say the distribution is continuous. But if the distribution is continuous, the number of possible states is infinite. So why is entropy not always infinite when a continuous distribution is used?

marked as duplicate by doetoe, John Rennie thermodynamics StackExchange.ready(function() { if (StackExchange.options.isMobile) return; $('.dupe-hammer-message-hover:not(.hover-bound)').each(function() { var$hover = $(this).addClass('hover-bound'),$msg = $hover.siblings('.dupe-hammer-message');$hover.hover( function() { $hover.showInfoMessage('', { messageElement:$msg.clone().show(), transient: false, position: { my: 'bottom left', at: 'top center', offsetTop: -7 }, dismissable: false, relativeToBody: true }); }, function() { StackExchange.helpers.removeMessages(); } ); }); }); Nov 9 '18 at 5:31

• Because it's not actually continuous, you're just pretending to make things easier. – Slereah Nov 7 '18 at 18:53
• The distribution isn't absolutely continuous, it is just continuous from a pragmatic point of view. Obviously if a 1 cubic meter box has only 10 molecules of gas, then the gas molecules can't form a continuous distribution. But a cubic meter of air at sea level contains something like $10^{25}$ molecules. – MaxW Nov 7 '18 at 18:55
• It is true that at given pressure and number of particles, $S$ does indeed tend to infinity as the volume tends to infinity. The bottom line is that there is one state per volume $h^3$ of available phase space (that is, position-momentum space) for each particle. – Andrew Steane Nov 7 '18 at 18:58
• May i ask: so for example for an ideal gas in box of volume $V$ for example, all the possible microstates are all the particles being at all points within $V$, which are uncountably many. Then your question in this situation is: why isn't the entropy infinite? – Lorenz Mayer Nov 7 '18 at 20:23
• The classical state space is indeed continuous, even for a single particle. In particular, there are infinitely many states, at least classically. How this can be resolved, is explained in physics.stackexchange.com/a/371686/25794 – doetoe Nov 8 '18 at 8:24

The distribution is continuous is exactly true only in the thermodynamic limit, in which case $$E$$, $$V$$, $$N$$, and $$S$$ are all infinite, while $$E/V$$, $$N/V$$, and $$S/V$$ are all finite (or, equivalently, $$E/N$$, $$V/N$$, and $$S/N$$ are finite). In a real-life situation in which the volume isn't infinite, the distribution is technically discrete. But usually the volume is macroscopic while the length scales in the problem are microscopic, in which case taking the distribution as continuous is an extraordinarily good approximation. Then the total entropy is enormous but finite.
$$S = k_B \ln \Omega$$
where $$\Omega$$ is volume of the region (as opposed to number of points in that region). This is sometimes done in statistical physics (pre - quantum statistical physics).