Questions tagged [kinetic-theory-of-gases]

Questions about the assumptions, equations, and properties of gases derived from kinetic theory. For questions pertaining to rates of reactions, please use the kinetics tag instead.

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Latent Heat and Kinetic Energy

The kinetic theory says that temperature is the measure of the average kinetic energy. That would mean then: The temperature rises with the rise in kinetic energy. We know that when matter changes ...
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1answer
1k views

Speed distribution of lighter vs heavier gases

I cannot understand why the range of molecular speed is not always wider for a lighter gas as compared to a heavier gas . If the same energy is supplied to both gases then wouldn't the molecular ...
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2answers
833 views

Is this a violation of Equipartition theorem?

My book has a question asking to calculate average kinetic energy of the molecules in 8g of methane. By the Equipartition theorem, I calculated that energy: 1. per molecule per degree of freedom = $(...
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1answer
98 views

What is the value of the gas constant derived from the kinetic model of gases?

I used this resource (http://digitalcommons.unl.edu/cgi/viewcontent.cgi?article=1151&context=physicskatz) to derive the ideal gas law from the kinetic model of gases: $$PV=n(2/3)N_oT$$ with T ...
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1answer
50 views

Direction of gas molecules in kinetic model of gases?

So when learning about the kinetic model of gases, my teacher said that in a volume $A*v_{x}*\Delta t$, exactly half the molecules will have a velocity component of $v_x$ and the other half will have ...
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2answers
354 views

is avogadro's law for the same gas?

Avogadro's law is V1/n1 = v2/n2 - volume and number of moles are directly proportional. My question is - can this law apply to two different gases - for example, Hydrogen with volume v1 and number n1,...
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1answer
2k views

Joule–Thomson effect: why does temperature decrease during expansion

When a gas under a high pressure in a piston (isolated from surrounding is allowed to pass through a valve), why does its temperature decrease once during expansion? I haven't still studied ...
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1answer
36 views

How fast do it take a gas kinetic energy to react to intense heat? [closed]

Let's say I have argon gas in a small container. And opened the flap of the container and stuck a rode that was around 2000-3000 Degrees Fahrenheit, And was only in there for a millisecond. How long ...
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1answer
284 views

How is the Maxwell-Boltzmann curve obtained?

Is it purely qualitative and determined by experiment? Or is there some function which defines the familiar graph? (Image source: Wikipedia)
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1answer
552 views

Does lowering temperature of a gas make it easier to compress?

My teacher said that for ideal gases, the lower the temperature, the lower the kinetic energy of a gas will be, and it will be easier to compress the gas. Using the ideal gas equation $PV=nRT$, if ...
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1answer
777 views

Derivation of Ideal Gas Law with Boltzmann's Constant

I was reading about the Kinetic Theory of Gases and I came to know about This Particular equation which piqued my interest. I know about the Ideal Gas Law which gives us $PV=nRT$. But this one ...
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5answers
897 views

Why do we need to assume that gas is made up of large number of small particles in kinetic molecular theory of gases?

Among the five postulates or assumptions of kinetic molecular theory of gases (KMT), only the assumption that a gas is made up of large number of small particles doesn't seem to make any sense to me. ...
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2answers
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Derivation of mean kinetic energy

I read from a book that average kinetic energy is equal to $3kT/2$ where $k$ is Boltzmann's constant and $T$ is the kelvin temperature. I don't know how the formula was derived. Any help to gain ...
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1answer
591 views

Temperature in the Maxwell-Boltzmann Distribution

I am attempting to generate the probability for the specific speed of a molecule using the Maxwell-Boltzmann distribution, but I cannot decide on which temperature I should use in the equation. For ...
2
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2answers
438 views

How to get the first step of the derivation of the Maxwell-Boltzmann distribution

To derive the Maxwell-Boltzmann distribution the first step requires the knowledge that the equation will take the form $$f(v)=Ke^{-\epsilon/ kT}$$ where $\epsilon$ is the sum of the kinetic energies ...
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1answer
185 views

When temperature is decreased, why do reactions occur at all?

I admit that my knowledge of collision theory may be lacking, but, as I understand it, when particles collide, a reaction will not occur without overcoming the activation energy. That being said, as ...
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1answer
11k views

Why do we need the rms, mean, and most probable velocities?

In the kinetic theory of gases, we have rms (root mean square), mean, and mp (most probable) velocities. I understand the concept well. But my question is why do we have three different kinds of ...
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0answers
73 views

Estimating Surface Reactions - Liquid, Turbulent Flow

So, I need a method of estimating the influence of a surface (rate constant would do for a start), the idea is to estimate just Reactant + Surface -> Product in a turbulent liquid flow. Now I am ...
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1answer
143 views

Change in pressure?

Consider a sample of gas in a fixed volume container . From the arguments of Kinetic Theory of Gases on quadrupling the temperature what will be the effect on pressure . Basically I thought that the ...
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1answer
2k views

Ideal gas law derivation from kinetic theory

Consider the derivation of the ideal gas law from kinetic theory presented here: http://en.wikipedia.org/wiki/Kinetic_theory I have some questions This derivation assumes the container is a cube, ...
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2answers
470 views

Kinetic theory of gases

The intermolecular distance between the molecules are much greater than the diameter of the gas molecules so we neglect their volume compared to the volume of container. "The rapidly moving particles ...

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