suppose-container-a-contains-1-mathrmmol-mathrmcs-and-1-mathrmmol-mathrmo_2g-and-container-mathrmb-c

Question

Suppose Container A contains 1 $\mathrm{mol} \mathrm{C}(s)$ and $1 \mathrm{mol} \mathrm{O}_{2}(g),$ and Container $\mathrm{B}$ contains 1 $\mathrm{mol} \mathrm{CO}_{2}(g) .$ Both containers are closed and both are the same size. Compare the containers in each of these ways.
a. number of atoms
b. number of gas molecules
c. mass
d. gas pressure

Ethan Fuhrman · Accepted Answer

Okay, so we&#x27;ve got two containers. We&#x27;ve got container A. We&#x27;ve got container container. A has one mole of solid carbon. Um, and one mole of extra guests. Container B has one more off carbon dioxide gas. Both containers are closed. I should probably draw. And they&#x27;re the same size. So we need to figure out which container A has the, um, greatest number. Adams be the greatest number of gas molecules. And C c uh, greatest mass and D, uh, greatest gas pressure. All right, so starting with a number of Adams, Uh, so we&#x27;ve got carbon here, which is a solid, um, and we&#x27;ve got oxygen, which is a gas, and we&#x27;ve got carbon dioxide, which is a gas. So taking a look at which one has the most number of Adam&#x27;s. Let&#x27;s break down carbon dioxide. So Seo, too. There&#x27;s one wall of for one wall of CO two, but there is here. There&#x27;s one bowl of carbon and one mole of molecular oxygen that looks to be the same as the contents of container A. So I&#x27;ll say that in terms of the number of Adams, they are equivalent. All right, now let&#x27;s move on to the number of gas molecules. All right, so we&#x27;ve got a mole of carbon dioxide molecules, and that is I see double bond into two oxygen&#x27;s, um, and we&#x27;ve got oxygen here, which is just oxygen double bonded to itself. There&#x27;s one mole of each gas. So I&#x27;d say, uh, number gas mall. You&#x27;ll those are the same. All right, well, let&#x27;s take a look at the map. So we&#x27;ve got one mole of CO two, which has one mole of C and one mole of 02 um, in both. So in terms of mass, they are equal again. Um, And since they have the same number of gas molecules, that means that they should have the same pressure for the same volume and temperature. I&#x27;m assuming so, pressure that should be equal between the two, and that&#x27;s that

Joanna Josey · Answer

So for this problem, we&#x27;re being asked to consider two different gases A and B each and one leader containers with both gases at the same temperature and also both gases in the same at the same pressure. Soapy. The pressure of a equals the pressure of B. I&#x27;m are being asked, um or that we also have the masses of the containers. The container, um A has a massive 0.34 grams, and the mass of B is 0.48 grams were being asked which sample has the most molecules present. So thinking about the equation for number one PV equals and our tea, we know that our is constant. We know that our temperature between the two is equal. The pressure between the two is equal, and the volume between the two is equal. The only way that that is possible is that the number of moles in A is also equal to the number of moles and be so therefore, they have an equal number of, um, molecules for part B. The second question is, which gas sample has the largest average kinetic energy. Um, in this case, we&#x27;re gonna be thinking about our our equation for kinetic energy is kinetic. Energy equals three halves are times t times the number of moles. Well, again, since the temperature is the same and the number of moles is the same than the kinetic energy for a is equal to the kinetic energy of B. The third part of the question is asking which gas sample has the fastest average velocity? Um, so both gases have an equal number of moles, but B is heavier, so B has a massive 0.48 So even though they&#x27;re moles are equal, B has a massive point for eight, and A has a massive 80.34 So, therefore be is heavier than a so because B is heavier than a um, it will move more slowly and therefore have a MME. Is a lower velocity than a. And then finally, Part four is asking in this situation. Um, which how can the pressure in the two containers be equal to each other since the larger guests be molecules collide with the container walls more forcefully? Well, so in this gift, we have to think about this in terms of not just the force that they&#x27;re there, that they have, but also how quickly they&#x27;re moving. So guess B can exert more for exert more force, but it&#x27;s moving more slowly, so it has a has a smaller velocity, so it&#x27;s colliding less often. Gas. I&#x27;m sorry that was Guess B. Guess A has a higher velocity, and so is it. Actually, therefore it hits more. It&#x27;s more often, um so even though it has less force, it is hitting more often, and so therefore the pressures are equal.

Cathy Geisel · Answer

we&#x27;ve got gas and gas be. We know that gas a is sulfur dioxide gas be is unknown. We are comparing the pressure of the two gases. We know that there is one mole of eso to and there are two moles of gas be. We know that the volume of gas A is one and the volume of gas be is too. So if we&#x27;re looking at just those factors in leaving temperature out because you increase both the moles and container B and the volume and container B two to that cancels each other out cause volume is twice Aziz much for twice the number of moles. So up until the difference in temperature pressure shouldn&#x27;t gas a and gas be would have the same pressure because you increase the number of moles. You also increased volume differences temperature So we know that a is that to 80 and B is at 5 to 60. So the pressure Excuse me? The temperature of B is twice the temperature of a so that means that gas B is gonna be two times greater in pressure than gas. A

Marissa Turner · Answer

this is questioned 74 from chapter 11. And we have three boxes with the blue, red and green gas, and we&#x27;re gonna be finding mole fractions, pressure and total pressure. So first, we&#x27;re going to find the smallest small fraction. And what do you do that you have to first on the total of each box. So box one, a total of nine, like he said, makes me this come up. Um, add up all the color dots. So we have nine in box one 12 in box two. And we have 15 in box three. So after that, we would be finding the mole fraction for the red cat. Okay. And so in box one, we have three red dots out of nine total. Okay, so three over nine, it&#x27;s gonna be equal to 1/3. Just a mole. Fraction for right gassing one and two, we have four out of 12 and this also goes down to 1/3. And the more fraction for number three. You have five red dots at a 15 total, and this is equal to 1/3. So the answer to a is that what has a small a small fraction? Well, all of them. Okay. Next that one to find the highest partial pressure for the green gas. Okay, so for one, we have to out of nine, and this is equal to point 222 For box number two, we have three green dots out of 12 and this is equal to a 4.25 And for three, we have four green dots out of 15 and this is equal 2.27 So which one has the highest box number? Three for the green grass. Okay. And the last one is asking which one has the highest total pressure. So this was actually easier, because all you have to do is add up. How many dots on each? In the highest number of particles is the highest toll pressure. So this is also number three, cause it has 15

A. Elizabeth Hildreth · Answer

problem 63 tells you to consider to supper gas campaigners at the following conditions. So the conditions listed in this table here and it asks how the pressure and container B is related to the pressure on container, eh? So just part looking at this table here, Um, there&#x27;s not so much of, ah recognizable pattern as as it&#x27;s filled out. But of course, remember when filling out the ideal gas law equation. Temperature needs to be in Calvin. So actually helps, um, Thio draw out an obvious pattern. Um, that we can prove by solving the equation for each of these two different containers here. So let me convert the temperature from Celsius to Calvin for each of these containers. Um, Container one has a temperature of 280 Calvin and container to has a temperature of 560. Calvin. So this now draws out a, um, a relationship between container and container B where, um, container B, where the pressure and container B iss two times that of container, eh? We can solve the math here to proof that to ourselves. Um, so first we&#x27;ll solve for container, eh? So the pressure and a here is what will be solving for you know that this container has a volume of one leader. You know that there&#x27;s one mole of gas in this container. We can plug in the ideal gas constant and the temperature and Calvin. And when we saw for the pressure here we get 23 atmospheres so likewise on the right hand side. Here, weaken, solve for the pressure and container B. And in this container we have a volume of two leaders. There are two moles of gas in this container. Again, we can plug in the ideal gas constant and the temperature of this container. And when solving for the pressure than container B, we get 46 atmospheres. So when you compare, um, container B to container, eh? You can see that the pressure and container B is double that A container? A which verifies, um, this pressure and container B is equal to two times the pressure of container. A relationship that we talked about before

Matthew Confer · Answer

using the ideal gas law of P V is equal The n r T. We can answer all of these questions. So for part A if we assume that all of these are ideal and they&#x27;re all the same temperature, we know that the lowest pressure will be the largest. Volume has the fewest molecules, and the highest pressure will be the smallest volume that has the most molecules. So for your through with this, we have that to m six are less than 145 and eight, which is less than three and seven for part B. We know that the average kinetic energy must be the same for all of these because it&#x27;s the same temperature for Percy is in cat. Um, we can look at the density, and here we need to actually bring in the molecular weights of neon and are gone, um, there roughly two times each other. So we know here that too, has the least density. Well, 14 and six come after that. Then we have 35 and eight, and then we have seven. All we&#x27;re doing is counting molecules and dividing by volume and then four part D as in dog, which is the root means square velocity. All that is is, um Mu r m s is equal to three r t over the molecular weight to the 1/2. So we know here is that the smaller molecular weight you have the larger European squared velocity, which means that 567 and eight are all less than one too three and four. So all the ah organs list rolled in neon.

Problem 8 Hard Difficulty

Answer

a. Both have same no of atoms.
b. Both have same no of gaseous moles
c. Both have the same mass
d. Gas pressure inside the containers is equal

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a. Both have same no of atoms.b. Both have same no of gaseous molesc. Both have the same massd. Gas pressure inside the containers is equal

Living by Chemistry

Theodore D.

Stephanie C.

Lizabeth T.

Jake R.

Intro To Chem - Introduction

Classification and Properties of Matter

Angelica M. StacyLiving by Chemistry

Theodore D.

Stephanie C.

Lizabeth T.

Jake R.

a. Both have same no of atoms.
b. Both have same no of gaseous moles
c. Both have the same mass
d. Gas pressure inside the containers is equal

Angelica M. Stacy

Living by Chemistry