At a reasonably high (and equal) temperature, one mole of which of the following has the greatest entropy?
This section requires Javascript.
You are seeing this because something didn't load right. We suggest you, (a) try
refreshing the page, (b) enabling javascript if it is disabled on your browser and,
finally, (c)
loading the
non-javascript version of this page
. We're sorry about the hassle.
Dioxygen is a diatomic gas. How does one uniquely state the configuration of a dioxygen molecule?
There are six degrees of freedom. You need three parameters to locate the first atom, two more to locate the second, and one more to specify the vibration of the bonds.
Carbon dioxide is triatomic linear.
There are seven degrees of freedom. Three to locate the first atom and two for the second. This fixes the third atom. We need two more for the two bonds.
There are more ways to distribute energy amongst the Carbon dioxide molecules.
This is why it has higher entropy.
Reality Check!
Standard Molar Entropy for Oxygen: 205.15 J/mol/K
Standard Molar Entropy for Carbon Dioxide: 213.79 J/mol/K
Source