use-the-kinetic-theory-of-gases-to-explain-why-decreasing-the-gas-temperature-decreases-the-gas-pr-2

Name: use the kinetic theory of gases to explain why decreasing the gas temperature decreases the gas pr 2
Uploaded: 2020-10-15
Duration: 1 min 35 s
Channel: Numerade
Description: Use the kinetic theory of gases to explain why decreasing the gas temperature decreases the gas pressure.

Question

Use the kinetic theory of gases to explain why decreasing the gas temperature decreases the gas pressure.

David Collins · Accepted Answer

This next question is also associated with the kinetic molecular theory of gas. But it asks us to use the kinetic molecular theory of gas is to explain why decreasing the gas temperature decreases the gas pressure. So if we have a container of this size and we have a certain number of molecules in here, say 12 then the pressure is going to be a function of the frequency and the force at which they collide with the walls of the container. So if we have a high temperature here and then we have a container of the exact same size at a low temperature with the same number of molecules at the higher temperature, they&#x27;re going to collide with the walls of the container with greater force more readily. Why? Because the velocity is going to be greater. So at higher temperatures they&#x27;re moving more quickly here because they&#x27;re moving more quickly. They&#x27;ll collide with the walls of the container more readily and with greater force, so the pressure is going to increase

Madeline Currie · Answer

this question asked us to explain why the pressure of a gas will increase as its volume decreases if the temperature is constant. So if we think about what causes the pressure of the gas, it&#x27;s the collisions of the gas particles with walls of the container. So if we look over here, this container is fairly large and has safe five gas particles in it. These particles are all gonna be randomly colliding with the walls of the container. And that&#x27;s gonna cause the pressure, uh, in the container if we were to reduce the size that container to this size. Now this purple container now takes up the same model space as just a piece of that bigger container. Right, So over here we have the same five molecules. Where is in the big container? We would have a fraction of those five molecules in that purple amount of space at any given time. So the amount of collisions happening in the purple box big in the big container is a lot less collisions than what is happening in the purple box when all the molecules air in that box and a smaller container. So because the volume has decreased, the number of collisions will increase and that will increase the pressure. We can also see this if we look at the ideal gas equation, so pressure and volume are going to equal this quantity. So if the temperature is kept constant and we&#x27;re assuming that we have a constant amount of moles, are is also a constant. This number is not gonna change so that therefore, if the volume decreases, the pressure has to increase in order to keep this number the same.

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

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.

Katie Mcalpine · Answer

um So this question we want to explain why, If you keep the temperature of the same, um, and you reduce the volume, why does the pressure increase? And so let&#x27;s write out the ideal gas law and figure this out. So ideal gas law stays PV equals and r t So our is gonna stay the same. Let&#x27;s assume that the whole particle number will stay the same and, um so the volume goes down and what else temperature is. Constance always put dot over it. Um, and so if this whole right side of the equation stays constant and V goes down, the P needs to go up, Um, in order to keep the product of PNV constant. So that&#x27;s That&#x27;s why U P

Marissa Turner · Answer

is this question 154 from chapter 11. And we&#x27;re gonna be using the average kinetic energy to explain why hot air rises. Okay, so harder air. Typically, Ning&#x27;s has a higher temperature. And when there&#x27;s a higher temperature hotter later, this needs is gonna be any average medic in your deeds. It&#x27;s going. Do you going to be higher for the okay? So when they have more energy, this is gonna mean after got have more frequent collisions with me should. And you&#x27;re gonna be more spread out because when we weren&#x27;t spread out because when there&#x27;s heat, it means that the gas was expanding. Okay, Teoh, when the gas is expanding, this this is going to cause This causes air to rise and causes a lower dispensary to which means why you can hot air drives rested. Things tend to rise to the top

Problem

Suppose that the pressure of a gas in a cylinder …

Problem 2 Easy Difficulty

Use the kinetic theory of gases to explain why decreasing the gas temperature decreases the gas pressure.

Answer

When temperature is increased, the gas molecules gain kinetic energy and move faster.Because of this gas molecules exert high pressure.
Pressure is directly proportional to temperature.
P1/T1= P2/T2

Related Courses

Living by Chemistry

Related Topics

Discussion

Top Chemistry 101 Educators

Stephanie C.

Lizabeth T.

Stephen P.

Jacquelin H.

Chemistry 101 Courses

Intro To Chem - Introduction

Classification and Properties of Matter

Recommended Videos

Watch More Solved Questions in Chapter 11

Video Transcript

Angelica M. Stacy

Living by Chemistry

Stephanie C.

Lizabeth T.

Stephen P.

Jacquelin H.

Intro To Chem - Introduction

Classification and Properties of Matter

What do you need help with?

Textbooks

Ask a question

Courses

AI Tutor

When temperature is increased, the gas molecules gain kinetic energy and move faster.Because of this gas molecules exert high pressure.Pressure is directly proportional to temperature.P1/T1= P2/T2

Living by Chemistry

Stephanie C.

Lizabeth T.

Stephen P.

Jacquelin H.

Intro To Chem - Introduction

Classification and Properties of Matter

Angelica M. StacyLiving by Chemistry

Stephanie C.

Lizabeth T.

Stephen P.

Jacquelin H.

When temperature is increased, the gas molecules gain kinetic energy and move faster.Because of this gas molecules exert high pressure.
Pressure is directly proportional to temperature.
P1/T1= P2/T2

Angelica M. Stacy

Living by Chemistry