 The third one is gale stack halal. For a given amount of gas For a given amount of gas The pressure is directly proportional to the temperature For a given amount of gas The pressure is directly proportional to the temperature The pressure is directly proportional to the temperature The pressure is directly proportional to the temperature The pressure is directly proportional to the temperature The pressure is directly proportional to the temperature The pressure is directly proportional to the temperature The pressure is directly proportional to the temperature The pressure is directly proportional to the temperature The pressure is directly proportional to the temperature The pressure is directly proportional to the temperature The pressure is directly proportional to the temperature The pressure is directly proportional to the temperature The pressure is directly proportional to the temperature The pressure is directly proportional to the temperature The pressure is directly proportional to the temperature So P is equals to we can write K and T where K is the function of, K is the function of volume. And we can say what K is inversely proportional to? Volume. The graph? It is of volume. Ah, there is gases law of multiple. There are three law that we know when the gas molecules combine. So one of the law is that in the U.S. Law of multiple proportion, law of definite proportion. What are those? That is, ah. Right, so the pressure and temperature graph is what? V1, V2, V3, V3. And here we have log P and log T. There will be a thing there. What is Y? So maximum volume. So what is the relation of V1, V2 and V3? The slope is, the maximum constant slope is V1. So V1 is the, K is maximum, V1 is minimum. So V1 is less than V2 and then V3. What about this one? Log P and log T. Log P is equal to log T plus log K. That is the same, right? Log will be like this. Angle will be, slope will be 45. This distance is nothing but log. A is less than 1. A is less than 1. Sir, between 1 and T, you go in all the k's. Log is less than 1. A is less than 1. But for this thing, K won't be negative. K won't be. It won't be patched. And the gasses molecule will have some volume. And there are other things also. Temperatures also are very low. Okay, next slide out. We have already discussed this. That is, evergadro's law. What is evergadro's law? Nevee. Evergadro's law. It's the same thing. Okay, right now. And given pressure and temperature, the volume occupied by the gasses molecule is directed closer to the number of moles. P is equal to, right? And we can write B is equal to K. What note do you write down? K is the function of, here we have pressure and temperature both. Directly to the pressure, inversely to the pressure. Write down, if the gasses molecule is unloaded right now. What is the pressure? Directly. Directly to the pressure? I don't think so. B is equal to LRT compared to LRT. What is the softest risk? Combine the pressure. Actually, we'll get that equation from these equations. Okay, right now. If the gasses molecule has equal number of moles, then they must have equal number of molecules. Equal number of moles. Then they must have equal number of molecules. This condition is satisfied. Equal number of molecules. But the number of atoms may or may not be equal due to difference in atomicity. This question is easy. Can you tell me the number of molecules you have? The number of molecules you have? Can you tell me the number of molecules you have? So there's some new values, sir, so now there's some new values, sir, so you used to, before you used to give us different values, yes. So the textbook is written that they changed different values, now they're using some 760, I mean, 760. So there's some slight difference, sir, so an NCR is different value than you. So the NCR is like 0.08, something else is like last two. Also, approximately? Yeah. They changed it for the fifth time. These two you need to memorize, and this is almost equals to this one, because 0.08, if you take, so 8 by 100 is 12. something. So when you take 1 by 12 instead of 0.0821, that will, no. But you take 1 by 12 sometimes approximation, it will be, calculation will be easier. Okay. So this is the, this equation, we call it as equation of state. Equation of state means what? At two different points, if you try to define the position of the gaseous molecule, you can use this equation, right? So for a given number of moles, at two different points, suppose here, and here if you are trying to define, two different positions a and b, if you try to define the solution of gas, you require what? You require pressure at this point, pA, volume at this point, pA, temperature at this point, and the number of moles of the gas that we are using. And here it is, eb, and the number of moles, we can try to eb, pA, volume, this is the equation of state. At two different states, we define the position. So in the first one, 8.314, which, that's for power, that's for power. When pressure is in power, do you think it will, it's a different, it's a different unit. Yeah, it's in dual-cormorant calories, SI unit here, right? Yes. Okay. What is the sum of that sum? Yes. The pA, pA, pA, pA. Yes, one can do two different positions. Yeah. You have to be able to see the same, you have to see the same. I have to see the same. You need to get this. Right? Pv is equals to nRT is the equation of state. The gaseous which follows this equation are called ideal gas equation. Okay, so right on this, for a given number of moles, Na and nB are equal. So this, at this position, we'll define by pA, pA, pA, and dA. This is the relation. Two different positions for a given amount of gas. Okay. Right on. The gaseous molecules. If number of moles is equal to just pA, pA, pA, nA, dA. You have to add that. And that is all. Right on. For a, if the gaseous molecules follows, the gaseous molecules follows the equation of state. It is known as ideal gas. If the gaseous molecules, gaseous follows the equation of state, it is known as ideal gas. It is the theoretical concept or hypothetical concept you can write. Hypothetical concept you write down. It is the hypothetical concept. But none of the gas, none of the gas behaves as ideal gas. And that is why we also call it as ideal gas equation. Okay. But you have to choose the option between ideal gas equation and equation of state. You have to choose equation of state, not ideal gas equation. Because ideal gas has been applied practically. Ideal gas actually not possible. There are two, three more assumptions also that we will discuss in kinetic theory of gaseous. Okay. See the other form of this equation, we can write Tv is equals to nRT. And p number of moles is mass divided by volume into RT by the molar mass of the gas. So mass by volume is nothing but the density. So we can write T is equals to density RT divided by the molar mass of the gas. Which is nothing but Tm is equals to drT where D is the density of the gas. M is the molar mass of the gas. Okay. Another way is what? Mold per liter p is equals to n by V RT we will write. And mole per liter is what? Concentration. Right. Concentration is mole per liter n by V. So we can also write p is equals to CRT. C is the concentration. Molarity.