what-ef-ect-does-changing-the-number-of-gas-particles-in-a-container-have-on-the-gas-pressure-in-the

Name: what ef ect does changing the number of gas particles in a container have on the gas pressure in the
Uploaded: 2020-10-14
Duration: 1 min 17 s
Channel: Numerade
Description: What ef ect does changing the number of gas particles in a container have on the gas pressure in the container? Use the kinetic theory of gases in your explanation.

Question

What ef ect does changing the number of gas particles in a container have on the gas pressure in the container? Use the kinetic theory of gases in your explanation.

David Collins · Accepted Answer

question Number four is very similar to question number two and that we will use the kinetic molecular theory in order to explain why pressure increases as we increase the number of gas particles. So I&#x27;ll use this same picture that we had before and the number density equation. The number density equation tells us that if we increase the number of particles according to this algebraic expression, we have to increase this, so both of them increased proportionally according to the proportionality constant. However, according to the molecular kinetic molecular theory, we&#x27;re going to increase the pressure because as we increase the number of gas particles, pressure in the kinetic molecular theory is due to the collisions with the walls of the container. More gas particles result in more collisions, which result in greater pressure, greater collisions, greater pressure. So that&#x27;s why increasing the number of gas particles will increase the pressure in the container

Sherry Tsui · Answer

The kinetic molecular theory states that gas particles are in constant motion and exhibit perfectly elastic collisions. So when the temperature is increased, the molecular motion in the speed of how the gas molecules move, also increases. First, the convict energy of the gas molecules increases as well be faster. The molecules can move, the more frequent they would collide with the walls of the container, thus increasing the pressure of gas.

William Braaton · Answer

we&#x27;re gonna be using kinetic molecular theory to explain how temperature and pressure interact in a gas. So let&#x27;s say that we have our early my flask here, and we put a stopper in it. So now we have a sealed, rigid container, and within our container there are a lot of gas molecules, and these molecules are moving around, running into the walls, running into each other, taking up the space, behaving as a gas would. Now we know, let&#x27;s well, let&#x27;s say that we were to increase the temperature of this gas. Kinetic molecular theory tells us that, um, the temperature in Kelvin is proportional to the kinetic energy of the molecules in the yes. So now we know that with this increase in temperature, we&#x27;re also going to see an increase in kinetic energy of the molecules in the gas. Some means these have a lot more energy in them. The molecules are moving faster, and because of the increasing connect energy, there&#x27;s also an increase and momentum of the particles. So now these are moving around faster, with more mo mentum running into each other more often and running into the edges of container more often Because thes have a higher momentum, the container has to exert a higher force to push back and change the direction. We know also from kinetic molecular theory that the force upon the container from molecules is what creates pressure. So we know that after this increase in temperature, there&#x27;s more kinetic energy. There&#x27;s more collisions, and that leads to more pressure on the inside of our container.

Theodore Donnell · Answer

Hello. Today we&#x27;ll be talking about chapter 12 Question 70 which asks us to consider the kinetic molecular theory of gases and how it relates temperature and pressure. So if we have a box of gas here at constant volume, the boxes rigid and will not expand or contract. We have some amount of gas in the box and it had given temperature. That gas has a given amount of kinetic energy by the kinetic molecular theory. And it uses that energy to bounce off all of the walls and all of Thea other molecules in the box. And so we&#x27;re applying a force every time we have a collision, we have a force applied to the walls over the area, the surface area of the box. And this is equal to the pressure inside the box because pressure is force over area. Now, if we increase the temperature, we have the same box. So it is the same volume in the same surface area, have the same number of particles of gas in it. But now these gases have more energy, they might be able to rebound more. We&#x27;re gonna draw more arrows all over the box. It&#x27;s gonna look a little cluttered, but gas is air. Not exactly a ah, you know, tight, clean, neat situation. So we have more energy, all float oId bouncing all over the box and hitting the walls more frequently. And thus for a given amount of time, more force is applied to the walls. Force applied to walls goes up, it increases. Where is the surface area of the box is the same, and thus we have an increase in the pressure. And so as we increase the temperature of a gas at a constant volume in a constant number of moles, we increased the kinetic energy of that cast the average kinetic energy, and thus we increased the collisions with walls of the container increasing the force applied to that container at the same surface area. And thus overall, we increase the pressure as we increase the temperature. Thanks.

Madeline Currie · Answer

this question asked us to explain why the pressure of a gas and a continual increase as its temperature increases. So if you think about a container of gas, um, the thing that causes pressure in that container is these gas particles hitting the walls of the container, those collisions or what caused the pressure? Now the speed that these gas molecules are moving is determined in part by their kinetic energy, and the kinetic energy is proportional to the temperature in Calvin&#x27;s. So the higher the temperature, the higher the kinetic energy will be, and therefore the faster these will be moving around and the more collisions will make and the more pressure in the container. We can also see this in the ideal gas equation. Um, pressure and temperature are on opposite sides of the equation. So if one side of the equation increases the temperature increases over here, then something on the other side also have to increase to match that, um, so temperature goes out, pressure goes up

Marissa Turner · Answer

This is questioned two from Chapter 11 Section three and it&#x27;s asking how pressure Berries with yeah, trapped gas volume. So when volume changes, it can either increase or decrease if the temperature is staying constant, so temperature is constant and volume decreases. The molecules have a deal with a smaller space, and this causes greater collisions, therefore causing an increase in pressure. That&#x27;s the first relationship we&#x27;re dealing with, so a decrease in role youm causes an increase in pressure. Now, if you haven&#x27;t increase in roll you, though the increase in volume will let the molecules have more space to move around. This actually causes left collisions and causes a decrease and pressure. So the relationship between pressure and volume is an inverse relationship. So when so pressure, it varies when volumes of the gas changes

Problem

Name three ways that you can increase the pressur…

Problem 4 Easy Difficulty

What ef ect does changing the number of gas particles in a container have on the gas pressure in the container? Use the kinetic theory of gases in your explanation.

Answer

In this way, the relationship between gas pressure and number of gas particles can be well explained by the Kinetic Molecular Theory of Gases

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In this way, the relationship between gas pressure and number of gas particles can be well explained by the Kinetic Molecular Theory of Gases

Living by Chemistry

Theodore D.

Nadia L.

Jacquelin H.

Jake R.

Intro To Chem - Introduction

Classification and Properties of Matter

Angelica M. StacyLiving by Chemistry

Theodore D.

Nadia L.

Jacquelin H.

Jake R.

Angelica M. Stacy

Living by Chemistry