Volume is how much space something takes up. Moles are how many or how much stuff you have gas molecules or particles in this case. Temperature is how fast the molecules or particles of gas are moving. The ideal gas law equation is below it is very important equation throughout the rest of your chemistry learning :.
The letter P represents Pressure , the letter V represents Volume, the letter n represents Moles , the letter R represents a constant a certain number to make the equation work together , the letter T represents temperature.
The most common units you will see for the ideal gas law are pressure in atmospheres atm , volume in Liters L , moles in moles mol , and temperature in K.
If the equation has all the units stated in the previous sentence then the constant R is 0. However, if the units of the equation change the constant number will also change. They usually call R the gas constant in chemistry books and classes.
The most important thing to know about all gas law equations is that they require you to use the Kelvin temperature scale , which is why I taught you how to convert to the Kelvin temperature scale before I started this section. All other units of pressure, volume, and moles can possibly have different units and the gas law equation will still work although other units tend to make it more difficult because you have to recalculate what the gas constant R will be.
I will now go on to teach you how to solve equations using the ideal gas law. In my demonstrations and example I will not emphasize the units of the gas constant R in the equations because it is too long and complex for this text format.
However, if you are more interested in the units of the gas constant then you can click on this link. If 57 moles of gas is held at a pressure of 5 atmospheres at a temperature of Kelvin what If gas occupies If the gas is compressed to What is the mass of a gas that occupies If a sample of neon gas occupies a volume of 2. See all questions in Gas Laws.
Impact of this question views around the world. Current timeTotal duration Google Classroom Facebook Twitter. Video transcript - [Instructor] In this video we're gonna talk about ideal gasses and how we can describe what's going on with them.
So the first question you might be wondering is, what is an ideal gas? And it really is a bit of a theoretical construct that helps us describe a lot of what's going on in the gas world, or at least close to what's going on in the gas world. So in an ideal gas, we imagined that the individual particles of the gas don't interact.
So particles, particles don't interact. And obviously we know that's not generally true. There's generally some light intermolecular forces as they get close to each other or as they pass by each other or if they collide into each other. But for the sake of what we're going to study in this video, we'll assume that they don't interact.
And we'll also assume that the particles don't take up any volume. Don't take up volume. Now, we know that that isn't exactly true, that individual molecules of course do take up volume. But this is a reasonable assumption, because generally speaking, it might be a very, very infinitesimally small fraction of the total volume of the space that they are bouncing around in.
And so these are the two assumptions we make when we talk about ideal gasses. That's why we're using the word ideal. In future videos we'll talk about non-ideal behavior.
But it allows us to make some simplifications that approximate a lot of the world. So let's think about how we can describe ideal gasses. We can think about the volume of the container that they are in. We could imagine the pressure that they would exert on say the inside of the container.
That's how I visualize it. Although, that pressure would be the same at any point inside of the container. We can think about the temperature. And we wanna do it in absolute scale, so we generally measure temperature in kelvin. And then we could also think about just how much of that gas we have.
0コメント