<p>:) s'ok... i was havin a bad day</p>
<p>E. I m pretty sure about that.</p>
<p>Chemistry major to the rescue
The answer is E - not D folks.</p>
<p>I. molar mass in uneffected obviously
II. a gas will always occupy the entire container it's in, and the volume stays constant. The temperature decrease does decrease the kinetic energy.. but kinetic energy is .5mv^2, nothing to do with spacing.. mass is constant, just the velocity of the particles decreases. Just because they are moving slower doesn't mean they are closer together.
III. Since the atoms are moving slower, there are less collisions with the sides of the container per unit time, thus the pressure exerted on the container has decreased.</p>
<p>It makes sense to believe someone who is majoring/has majored in Chem. I would've gotten something like that right in my real test had it appeared.</p>
<p>Chemistry grad student to the rescue as well! Pearlinthemist is correct - the answer is E.</p>
<p>Lower temperature = lower number of collisions = lower pressure.<br>
The volume for the entire gas stays constant. Also, the number of argon molecules stays constant. If you take the volume of the gas and divided by the number of molecules, you'll get the average volume that each molecule occupies, which is proportional to the average distance between molecules. This number doesn't change even if you assume that the gas is non-ideal.</p>