 The total pressure, the total pressure is, the total pressure is, the total pressure exerted by, the total pressure exerted by a mixture of non-reacting gases in a container at a given temperature, exerted by a mixture of non-reacting gases in a container at a given temperature is equals to, is equals to the sum of the partial pressure is equals to the sum of the partial pressure of each gases. Sir, where does the gap, if you occupy the same volume? So, volume has to be constant to both them? No, not this volume. Sir, in that case, can we use partial pressure and get the total pressure? Here you can use, actually when you write P a is equals to v and P a v is equals to n r t. Sir, if you have more than one gas present, then we can use the partial pressure equation over here. Sir, like adding the more than that, you just calculate, what you break is added? You are talking about these two. That is what we did, where the temperature is same. What is given in this statement, that at a given temperature? That is what we did. So, when you open the stock stock, these two mix, this has negligible volume. So, it is something like in a container, we have this much of O2NH2 present, non-reacting. Same thing with O2NH2. So, partial pressure is equals to what? Some of the partial pressure. So, in a gas, in a container, if you have, suppose, two, three gaseous molecules are present, non-reacting. So, total pressure will be the pressure of A, pressure of B and the pressure of C. The partial pressure of each component has a given temperature. That also we can write. One more relation we have, the partial pressure of any gas X is equals to the mole fraction of this into the total pressure. That is also another relation. Right? Partial pressure of any gas A is equals to the mole fraction of A into the total pressure. So, if the partial pressure is more for a given component, it means its mole fraction is also more. Right? It means its number of moles is more, more composition will be. Okay? So, write down if partial pressure increases for a given mixture, if partial pressure for a given mixture increases, then its mole, then its number of moles also increases. Okay? One question you see. Calculate the mole fraction and partial pressure. Calculate the mole fraction and partial pressure of each gaseous. So, in a container, and we are assuming that all the gaseous are non-reacting. Okay? This is the assumption we have. 16 gram of O2, 80 gram of SO3, 24 gram of CH4, and 96 gram of O3. Partial pressure and mole fraction. And once you know the partial pressure, you can find out total pressure also. Find out all these values. So, we need to find the partial pressure of each component. O2, SO3, CH4. Temperature is given. Write down temperature is 227 degree Celsius. Volume is 10 liter. Temperature is given. Temperature is 227 degree Celsius. Volume is 10 liter. And R value you can use 0.08. That is 1 by 12. 1.5 by 12. What is our partial pressure? S. 8. 4. 3. 2.2. 3. 4. 4. 2.2. 3. 4. 4. 3. 2.2. 4. 3. 2.2. It's somewhere around 70, 80, 20 you get. Check your capital. It's somewhere around 70. Yes, it's 17 points of capital. Okay, it will be number of fours of capital. It's half. It's half. It's half. It's half. It's half. It's half. 1 more of moles of CH moles. 1.5. 3 by 2. 3 by 2, 1.5. 7 by 2. 7 by 2. 7 by 2. 9 by 6. 9 by 6. Yeah, that's 1.5. 1.5. and 1.5 moles of Total pressure is what? P is equals to 5 into r is 1 by 12. Temperature is this plus 270 degrees, 5 by 2 divided by, volume is what? 10 liters. So, this will get 250 by 12. And mole fraction if you have to find out that will be partial pressure is lost to what? Total fraction total. Total fraction mole fraction of 1 by 2 divided by 5, 1 by 10. So, mole fraction of O2 is 1 by 10, mole fraction of SO3 is 1 by 5, mole fraction of CH4 is 0.3, mole fraction of O3 is 0.4, correct? The one which has maximum value of mole fraction will have maximum partial pressure. So, partial pressure of O3 we can write directly here, O3 is more than to that of partial pressure of CH4 which is more than the partial pressure of SO3 which is more than the partial pressure of O2. Sometimes they ask you to find out this order also. You don't have to calculate partial pressure just to find out mole fraction and see which one has maximum value of mole fraction and that will be the order of partial pressure. Total pressure. Just calculate mole fraction. Yes, that is okay. Even total pressure is not required. This is required when you want to calculate this. So, one will do here P O3 is equals to what? Mole fraction of O3 into Pt mole fraction of O3 is 0.4 into 250 by 12. So, 100 by 1 by 12, 10 by 12, so 5 by 6. 50 by 6. So, you gave 0.08 which was approximately 1 by 12. So, but when you use 0.08, you can get 0.6. So, you get exactly 0.6. Yes, fine. You can take that. The point is when you take this as 1 by 12, your cancellation will be much easier. I have seen that because you can take that approximation. In this, if you don't want, don't take, but when you have multiple choice questions and options are, they are closed. Then you can use that approximation. They won't change your answer. Okay? Kind of. The container contains CH4 and SO3 in 3s to 5 weight ratio. CH4 and SO3 in 3s to 5 weight ratio. Find out the ratio of partial pressure of CH4 and SO3. A container contains CH4 and SO3 in 3s to 5 weight ratio. Find out the ratio of partial pressure of CH4 and SO3. So, what do you find? Partial pressure. Ratio of partial pressure. At least 1. At least 1. What is the answer? At least 1. So, partial pressure of CH4 divided by the partial pressure of SO3 is equals to what we can write. Mold fraction of CH4 divided by the mole fraction of SO3. So, 3 divided by 16. 5 divided by 80. So, 3 is 2 month. Okay? Next question. Total pressure exerted by a mixture of 2 gas A and B. We'll have a mixture of 2 gas A and B. The total pressure is given. Pt is equals to 600 mmHg. Partial pressure of A is given. That is 240 mmHg. You need to find out partial pressure of B, mole fraction of A and mole fraction of B. Is the only pressure total and partial of A is given? Yes. 2 by 5. 2 by 5. What is PV? Total pressure is equals to PA plus PV, right? So, PV is equals to 360. And then we have the ratio of PA and PV gives you XA by XB. So, 240 by 360 is equals to XA by XB. That will be? Wait, sir. Can you just say that? This is 240 by 600. Yeah. So, you can say XA is 240 by 600. So, XA is 240 by 600. And then other than the 1 minus 1. Yes, that also you can do. Because partial pressure of A is equals to? Right. That also. Okay. And this we have. So, we have 2XB is equals to? 3XA? 6A. And we have XA plus XB is equals to what? 1. 1. And then you can solve? 3 by 5XB. 2XA plus 2XB. 2XB is equals to 5XA is equals to? Yeah. XA is 0.4, right? Yeah. Is it 0.4? Yeah, it is 0.4. When you solve these two, you get XA is equals to 0.4 and XB is equals to 0.4. See, in the container we have third ones. Mixer of H2 and CH4. H2 and CH4. Equal weight of. Equal weight of H2 and CH4 taken in a container. Equal weight. We need to find out the fraction of. Fraction of total pressure. Total pressure exerted by. Hydrogen. Fraction of total pressure exerted by hydrogen. 8 by 9. Equal weight of. Is it 8 by 9? Yeah, 8 by 9. 8 by 9. Yeah. What we need to find out? What we need to find out in this? Fraction of total pressure exerted by H2. Which means we need to find out? More fraction of. That is what we need to find. The same question they have asked in J exam. This one. It's took like 4, 5 seconds. Okay. You see in this one. H2 and CH4. What is the molecular mass of H2 to 2 gram? And this is? 16. 16 gram. Usually in the question they will give you the gases with molecular mass are multiple official. Like 2 F or 16 O gas. As I could try. Then what you can do is equal weight is taken. So you can assume any weight of these two. So what do you want X and assume 16 gram of it? 16 gram. 32 as you remember. What do you think? Should be multiple of these. Right? Suppose we have here 16 gram of H2 and 16 gram of CH4. What is the number of moles of H2? 8. X of H2 is? 8. And X of CH4 is what? 1. 1 number of moles. Fraction of total pressure. Just a second. Number of moles of CH4. So mole fraction of H2 is what? 8 by 9. Mole fraction of CH4 is what? 1 by 9. Any of these mass you can assume. Fraction of total pressure means whatever total pressure we have. Out of that what is the pressure exerted by H2? Partial pressure. Okay? You can also understand this way. Fraction of total pressure H2 is what? Pressure of H2 divided by what? Pt. Pt total pressure. And what is this? X of H2. Directly any of them. This is the fraction of total pressure exerted by hydrogen. So P H2 by Pt is nothing but X of H2. Mole fraction of H2 we need to find out. Got it?