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IQuestion 532ptsTne € quantity of aliquid in a closed container is halved at constant temperature Howdoes this affect the vapor pressure ofithe Iliquid? the v...

Question

IQuestion 532ptsTne € quantity of aliquid in a closed container is halved at constant temperature Howdoes this affect the vapor pressure ofithe Iliquid? the vapor pressure decreasesdepending on theliquid the vapor pressure may increase or decreasethe vapor pressure stays the samethe vapor pressure increasesQuestion 54How many oxvren atoms are in 15.3 gof glucose CallizO6? (The molar mass of glucose is 180 [email protected] 1.5*10230 3.1*102391.82 pts

IQuestion 53 2pts Tne € quantity of aliquid in a closed container is halved at constant temperature Howdoes this affect the vapor pressure ofithe Iliquid? the vapor pressure decreases depending on theliquid the vapor pressure may increase or decrease the vapor pressure stays the same the vapor pressure increases Question 54 How many oxvren atoms are in 15.3 gof glucose CallizO6? (The molar mass of glucose is 180 glmoll @ 1.5*1023 0 3.1*1023 91.8 2 pts



Answers

Calculate the vapor pressure at $25^{\circ} \mathrm{C}$ of a solution containing $165 \mathrm{g}$ of the nonvolatile solute, glucose, $\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6},$ in $685 \mathrm{g} \mathrm{H}_{2} \mathrm{O}$. The vapor pressure of water at $25^{\circ} \mathrm{C}$ is $23.8 \mathrm{mmHg}$.

Percentage of the vapor pressure of 3% is 19.8 you know, veggie 0.1 model because it into this water but the population of the resulting solution. Okay, so we have to identify what is the vapor pressure of the solution. So formula is what? Keynote minus the barbell pino mole fraction of the sunday. So this one is down. You can cause so more agriculture zero and one more of what we have to calculate. So full of water will be well 1 78.2 they were by eating there will come out more. It's going to be equal to 9.9. So the north is a part of that 19 Minour T they were by 19.8 Moral of solo will be 0.1. The barber is 0.1 plus 9.9. Thanks. So 9.9 yeah, let's 0.1. This is a good time. So 19.8 -7 0.1 into the 19.8 then. Okay, So 1.98 point right, So he will be 19.8 -9.19. There will comes out to get 19.6 amount of energy. So correct that we use the correct option. Okay

So we're gonna decompose a solid and we're going to produce some nitrogen gas. Okay? We're going to collect that nitrogen gas over water. So, we're gonna have to pay attention to the partial pressure of water as well. But let's go ahead and write down some of the things we know. Okay, we're collecting it in a 500 millim flask. So our volume is going to be .5. There are zero leaders. Okay. The temperature It's 19°C.. Let's go ahead and change that into Kelvin right away By adding to 73. So 2 92 Kelvin. All right. The partial pressure of nitrogen plus the partial pressure of the water is going to equal our total pressure. Okay? And they give us our total pressure as 745 mm of mercury. And they give us the partial pressure of water. Okay, 16.48 mm of Mercury at 19°.. Okay. So, we've got lots of information here. So, we want to know what's the partial pressure of nitrogen? Well, that's gonna be pretty simple, Right? Because we're just going to use this relationship right here. All right. So, the partial pressure of nitrogen is just going to be our total pressure minus the partial pressure of water. All right. So, we're gonna take our 745 mm of mercury. All right. And we're gonna subtract The 1648 And we'll get 729 mm of Mercury. Okay? So that's the answer to part A Okay. Now, we want to know how many moles of water are there in the wet gas? Well, we've got the partial pressure of the water, so we'll go ahead and use that to find our moles. Okay. So moles of water is just gonna be PV over. RT right from our ideal gas law. So, we'll take our the partial pressure of the water, which is 16 4 8. And I'm going to divide that by 760 so that we're in atmospheres. Okay, We're gonna multiply by the volume which is .5 l Our is .08-1. That's our constant. And our temperatures to 92 Kelvin. So that's going to give us zero 452 moles Of our H 20. Okay, so there's your answer there. Mhm. And now we want to know how many moles of the dry gas or the nitrogen. So same idea here. But we're going to use the the pressure of the nitrogen to find this out. Okay, so again, now we're going to use that pressure of nitrogen that we found which is 7 29. Okay, Again, I'm going to change it to atmospheric by dividing by 760. Multiply by the volume. Uh huh. Are this .08-1 and our temperature? So this will give us our moles of nitrogen which is .0-00 moles and two Mhm. So now we're gonna take our flask and we're gonna add some neon to it. Okay, so this is going to increase the pressure of our flask And we're gonna add .128 g. Okay, 0.128g of neon. And we want to know, first of all just what's the partial pressure of our neon? Okay, so first we're gonna go ahead and change that to moles. Okay, so we'll change grams to moles. Alright, Indians 20.18 which gives us our moles of neon. And then again, we're just going to use our ideal gas law, right? P is an R. T over B. We'll make sure we use the moles of our neon .00634 moles Times .08-1 times are temperature, which hasn't changed all over our volume, Which again is still .5 L. So that's gonna give us um .304 ATM Or if you'd rather have it in mm of mercury were multiplied by 760 And we'll get 231 millimeters of mercury. Okay, That would be the partial pressure of our neon. We're going to see if we can find the total pressure in our flask. So we've got three different gases going on here now. Okay, so let's remind ourselves from before we've got our moles of H 20 gas. We've got our malls of nitrogen gas. Okay. And we've got the malls of our neon gas. All right, they're all going to contribute to our partial pressure. So I'm gonna go ahead and get the total moles here. Okay, .0268 moles total. And then I'm just gonna go ahead again and use my ideal gas off and find the pressure. Using the total moles. Remember the pressure you find is always for the moles that you use. So, if you use the moles of something, you get the pressure. That's something. So, we're going to use the total moles to get the total pressure Put 0268 moles .08-1 for our Temperature hasn't changed, so it's still 292 And the volume of our flask hasn't changed. It's still .5 L. So, the total pressure in the flask now is going to be 1.28 ATM. Or if you prefer, you can multiply it by 760 And you'll get 976 mm of mercury

Consider the following compound. Yes, I seal too. See age three to that is dyke Loro Dime Essel styling his boiling point, a 70.3 degree Celsius. And we can plot a relationship between its pressure in the inverse of its temperature photograph like this, we have a temperature pressure will be and millimeters of mercury temperature in Celsius. Let's set up our scale. I'm breaking the scale down for temperature in increments of 25 and what we'll see is that we have a linear relationship. We have a temperature of negative point four degree Celsius. We have a pressure of about 40 if we have a temperature of 17.5 degrees Celsius, more pressure is about 100. We have a temperature of 51.9 More pressure is about 400 and if we have a temperature of about 70.3, have a much higher pressure. About 760. And we can connect those values, Ah, to give us a almost linear relationship. If we have a pressure of 2 50 millimeters of mercury, our temperatures should be approximately 39.6 degrees Celsius. We have a pressure of 650 degrees. I'm sorry. 650 millimeters of mercury. Our temperature will be about 65 degrees Celsius. We can plug these values in to the classiest clapper on equation to figure out the Moeller entropy of vaporization. So our formula looks like this. It's important to note for pressures one and two, and temperatures one and two are see. Put the numbers in the correct spots. Are is a constant 0.83145 killer jewels. Her talent mole Well, then temperature. It's one over 312.6, minus one over 338. Quite seven. When we plugged that information into our calculator, our value is 30 to kill a jewels, Permal.

Chemistry. And so we have the major component of the solution. This is identified as the solvent. And we often find out this will be in the same phase as the solution and the minor component. So we can have one or more. These are identified as the sole cute. So here we're looking at collaborative properties and these are the properties of solutions and mixtures that depend upon the concentration. So they do not depend on which sold it is added to the pure substance. For example, we can have the freezing point depression, boiling point elevation, vapor pressure lowering and osmotic pressure. So here's what we have is the following equation. So we have delta P. So that's the formula for vapor pressure lowering. That's equal to I. P. A. Star XB. So here the eyes is the number of irons. And then when we have P. A. Start, this is the vapor pressure of the pure solvent and XP is the mole fraction of the salt lake. So here we can fastly calculate the number of moles of 24.8 g of sucrose, so and be is equal to 9.9725 moles. And then we can calculate the number of moles of 17.1 g of sucrose. So that's an A. It's equal to 3.89 moles. So the mole fraction of sucrose, that is XB. That is equal to N. B. So that's not points, not 7 to 5, divided by 9.97 to 5 at 3.89 So what we get is not point not one A three. So then we can go back to our equation for delta P. So that is equal to 11 I are multiplied by 42 point to miller meters of mercury, multiplied by 9.9183 The value we just calculated to get 9.772 millimeters of mercury.


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