00:02
Hi there.
00:03
In this question, we have two containers, container a and container b.
00:07
Container a has 1 .0 .0 mole of oxygen gas, so that is 02, and we're told its molar mass is 32 .0 .0 grams per mole.
00:24
The second container contains 0 .70 moles of nitrogen gas, and its molar mass is 28 .0 grams per mole.
00:42
We're told that the temperature and the pressure are equal in each of these boxes.
00:52
Okay, so let's start off with the idea of temperature.
00:55
Temperature is a measure of average kinetic energy.
00:59
So if these are at the same temperature, they have the same average kinetic energy since the same temperature, because temperature measures kinetic energy.
01:18
Okay, furthermore, let's look at the equation for kinetic energy.
01:22
Kinetic energy is equal to one half mass times velocity squared.
01:31
So velocity is a measure of how fast they're moving or their speed.
01:37
So looking at this, since these are both at the same kinetic energy, that means that the mass and the velocity or the speed are inverse.
01:52
In other words, a greater mass will have have a lower speed, while a lesser mass will have a greater speed or velocity.
02:20
Okay, with all these things in mind, let's look at the answer choices.
02:25
The first one says the average speed of the molecules in container b is greater than that of the molecules in container a.
02:35
Now look what we just said.
02:37
We said the one with the greater mass will have a lower speed, while the one with the lesser mass will have a greater speed.
02:45
So that one looks correct.
02:49
The average speed of the molecules in b is greater than the molecules in a.
03:03
So that first answer option looks like our correct answer.
03:07
Let's check out the others though, just to make sure that they are not also correct and we have to pick the most correct one...