However, if you are more interested in the units of the gas constant then you can click on this link. First let us look at some examples to get an idea of what we will be asked of us. Examples : Solve for the following ideal gas law problems. If the volume of a gas container is 3L and the amount of moles is 2. What is the Pressure in atmospheres given that the gas constant R is 0. A container of gas is ml at torr, and 23 C.
If the gas constant is 0. Answer: 0. Then what is the volume? Answer: The information we are given red. Answer: Divide both sides by the gas constant and the temperature red.
Keep in mind the gas constant is always 0. If the pressure of a gas is 4 atm at 3 mol and K, then what is the volume? Answer: C…. R has the value 0. In other scenarios with pressures of bars instead, you may also use 0. However, temperature must always be in Kelvin K , as R uses units of K. Avogadro's law. Avogadro's law states that, "equal volumes of all gases, at the same temperature and pressure, have the same number of molecules.
Value of the Gas Constant. The value of the gas constant ' R ' depends on the units used for pressure, volume and temperature. Write Your Answer. Similar Asks What is 1 N? What are the N type material? How much do they pay at In N Out? What does the unit N stand for? What does nh4 N mean? What is N 30 in accounting? 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.
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