dear Science people:

[Nayr]

Do you guys know any real life examples of any of these laws:
Boyle's Law
Charle's Law
Gay-Lussac's Law
Avogadro's Law
Diffusion
Effusion
Dalton's Law
Combined Gas Law
Ideal Gas Law

[Kuya]

Gay-Lussac's Law

[Tyche]

Im the real life example of Murphy's law.


Sorry, had to say it because it was gonna be said eventually

[aurik]

Wikipedia.

A real world example?

Boyle's Law: if you buy a bottle of coke at a convenience store in the winter, open it and re-seal it inside, then take it outside, it will go flat almost instantly.

[Charla]

First of all, some of those are similar or the same thing. Boyle's law if I recall is a subcase of the ideal gas law (with the rest of the variables fixed). Also, do you want an example of where the law describes the real world, or a case where the behavior described by the law is easialy created and observable? For instance, a "real world example" of the diffusion law could be oxygen entering the bloodstream through the lungs, but that's not particularly useful in most cases.

Also, wikipedia ftw.

[Devek]

Charles' Law

Intercooler's used in turbo charging systems cool the hot air leaving the compressor so it becomes more dense before entering the combustion chamber.

[Elesirdur]

Here's a very easy one for the Ideal Gas Law, pV=nRT

The air pressure in your car's tyres varies over time. This is due to a lot of factors, not the least that air is escaping from the tyre enclosure. One of the major factors that affects what pressure the air is in your tyre is the temperature of the air. If you fill up your tyres on a cold day, and then it turns hot a week or so later, you will notice that the pressure is actually higher. Similiairly, if you happen to have a fancy new car with internal tyre pressure monitors you could conceivably watch the air pressure increase as you drove faster, say on the highway, than when you just started the car or are just in stop-and-go traffic.

In a typical hard-walled street tyre (not a soft-walled drag racing tyre) one can assume that the internal volume, V, will remain constant. Let's also assume that the amount of air in the tyre doesn't vary greatly, eliminating n, the molar amount of gas, and that the ideal gas constant, R, just stays the same (because it does). Therefore, in this example V ~ T. So, if the temperature increases, the pressure of the air in the tyre will increase because its container does not change. If you do a lot of highway driving it's not a bad idea to only fill your tyres to about 90% or so of their recommended pressure as excessive highway driving will increase the temperature in the tyres while underway and bring the pressure up to their nominal standard. Additionally, when the weather starts to get warmer it's always advisable to re-check your tyre pressure as the proper amount you put in during winter may be over-filling the tyres now due to heat expansion of the air.

Ninja edit: I think what I'm describing can more easily be thought of with Boyle's Law in the P1•V1=P2•V2 kind of equation. But then again, so does the Combined Gas Law, pV/T=r or (P1•V1)/T1=(P2•V2)/T2

[Nirokun!]

diffusion? it happens in all cells of the body?

um let me try and remember my A&P..

cells maintain a membrane potential by creating an electron gradient, high potassium ion environment inside, high sodium ion environment outside. then, when a cell opens channels between the inside and the outside, the electron flow is harvested for cellular activities >_>

if i got any of that wrong, someone yell at me

[divisortheory]

Do you guys know any real life examples of any of these laws:
Boyle's Law
Charle's Law
Gay-Lussac's Law
Avogadro's Law
Diffusion
Effusion
Dalton's Law
Combined Gas Law
Ideal Gas Law

The fuck? Do your own homework I don't know shit about these laws and I could do this homework assignment in about 10 minutes.

[Takeno]

Avogadro's Law is used for measuring really small quantities for the most part. Usually compounds, elements. 6.02 x 10^23

Gay-Lussac's law is when you take it in da butt by a french dude.

Someone had to say it

わたしはがるかです。。。

[Yensho]

in all of these, k is the constant.(does not mean it is temp for Boyle's, Pressure for charles, etc.)

Boyle's Law = PV=k An example would be a syringe, open all the way, then capped, and then pressed, the oxygen is given less volume because of the increased Pressure, so long as temperature remains constant.

Charles' Law = T/V=k Example: basically, anything to do with kinetic energy. it's known that molecules speed up in higher temperature, therefore increasing the volume of the container because of the more rapid collisions on the container wall, so long as Pressure remains constant.

Gay-Lussac's Law = T/P=k Example: This one is best explained with any carbonated or pressurized products. If you leave a coke can in your car in the summer, the heat will cause the volume to increase, but since, in the coke can, the volume is a constant, the pressure must increase, and if it increases enough, it explodes. Same with cold; if it gets to cold, the molecules in the can will go closer together, and since volume is once again at the constant, the atmosphere's pressure pushes it inward, causing it to implode.

That's all the ones I know, just now starting Avogadro's Law.

[Priran]

Avogadro's Law is used for measuring really small quantities for the most part. Usually compounds, elements. 6.02 x 10^23

that's avogadro's constant or number, which is used to determine the amount of molecules in a mole.

[VZX]

Do you guys know any real life examples of any of these laws:
Boyle's Law
Charle's Law
Gay-Lussac's Law
Avogadro's Law
Diffusion
Effusion
Dalton's Law
Combined Gas Law
Ideal Gas Law

The fuck? Do your own homework I don't know shit about these laws and I could do this homework assignment in about 10 minutes.

And Wikipedia makes students' life easier than ever before.

[zoobernut]

Avogadro's Law is used for measuring really small quantities for the most part. Usually compounds, elements. 6.02 x 10^23

Gay-Lussac's law is when you take it in da butt by a french dude.

Someone had to say it

わたしはがるかです。。。

Avogadro's Law actually has to do with the volume of different gasses at the same temperature and preasure.

(p1*V1)/(T1*n1)=(p2*V2)/(T1*n1)=Constant

Equal volume of gasses at the same temperature and pressure contain the same quantity of molecules or particles.

You were thinking of Avogadro's number or the molar number of an element.

To the OP I think there is a way to prove this in real life using the weight of a gas and its volume, my chemistry teacher in highschool showed us this law in a demonstration but I totally forget how he did it.

[Cheerios]

Fuck math.

[divisortheory]

Fuck math.

Too bad this post isn't about math, dumbass.

[Skyylya]

Diffusion is the movementof a substance from a point of high concentration to a point of low concentration.

For cellular diffusion, it is the exchange that goes on between the cellular membranes for oxygen, energy and wastes that get passed between. When the cell uses it's oxygen and the oxygenated blood is passing by, the oxygenated blood (point of high concentration) will diffuse into the cell full of Co2 (point of low concentration) and same goes for the Co2 into the blood cell.

Edit: Not sure if this is important but there are different types of diffusion, there is facilitated diffusion, in which energy is required by the cell in order to make it happen, and passive diffusion, in which the molecules can diffuse without any energy from the cell. The energy is in the form of ATP

A real world example would be something like, take a full glass of water and set it on the counter (or where ever), then take another fluid of a different color, like food coloring or something, and drop some in. You'll see the food coloring start to diffuse from the area's of high concentration (the drops) to the area's of low concentration (areas without any coloring).