could someone explain:T=PV / nR ???

Question

I believe it has to do with Temperture coefficients

Answer 1

Except for the wise-guy answer, all the answerers are pretty much on point. But I'm not clear they answered your question. Were you asking about the equation itself or were you asking about the physics...this is, after all, the physics, not the math, category.

An ideal gas is really an idealized gas, because there is no such thing in real life. For one thing, the moclecules of an ideal gas are without size. Whereas, even hydrogen gas, the most ideal of the real gas has molecules with some size.

Anyway PV = nRT is an interesting equation to examine for the physics it describes. For one, it says that PV/nT = R, which is a constant. Thus (and here's the physics), if temperature is raised, pressure and/or volume of the gas must also be raised. Otherwise, R would not remain fixed.

So, in practical terms...you're driving your Porsche at about 200 kph on the autobahn. The heat of the tires goes up from friction and the hot burning German sun on asphalt. Your $300 per tire Michelin's will not expand...what happens to the pressue in your expensive tires?

Well, PV/nT = R is what happens. V stays pretty constant (because of the good tires); so the only thing that can vary and keep R a constant is P, the tire pressure. P has to go up; and if your tire pressure was on the high side to start with (better milage), that increased pressure could blow a tire at 200 kph.

Here's another one...suppose you blow up a balloon the morning of a birthday party. It's a cool morning, but as the day drags on, the temperature inside your house rises. What happens to that balloon?

This time V is not constant. So both pressure and volume could rise as the balloon's temperature rises. Which one will it be? It depends, but it could very well be both. In fact, experience (I've had lots of birthdays) tells me that the volume (V) gets noticeably bigger during the hotter day. Sometimes it gets so big that there is no more elasticity left and the balloon bursts.

So there you have it...the physics of your equation. One can also set PV/T = pv/t = R; where P and p are different pressures, T and t are different temperatures, and V and v are different volumes of the same moles (n) of the same gas. This is a cool way to show changes in the factors when one of them is a constant.

For example, you Michelin tires. Since V = v = constant, we can write P/T = p/t; so that P = p(T/t), which clearly shows that if T > t, then P > p...the pressure in your tires has to go up if the temperature rises. This is gratifying because that's what we found earlier using PV = nTR.

Answer 2

Temperature = Pressure X Volume / number of Mols X the constant R

It can be rewritten any number of ways like these:

TnR = PV
T/PV = nR
TnR/P=V

etc.

It is known as the ideal gas law and is a nice relationship between the included units.

Answer 3

PV=nRT
This is the famous ideal gas equation.
This is the combination of Boyle's and Charles' laws.
This is the equation governing the behaviour of gases,and the relationship of three variables of Pressure, Temperature[absolute],and volume.

Answer 4

PV = nRT

This equation is for an ideal gas. An ideal gas is one which obeys certain laws, it might be useful to look them up! Basically, it says that the pressure of the gas multiplied by the volume of the gas is proportional to the temperature of the gas. n, I think is the number of moles in the gas, specific for each element, and R is a constant. I hope this helps :]

Answer 5

the combined equation arrived at from boyle's and charles' laws is PV=nRT
transposing and making Tthe subject
T=PV/nR

Answer 6

Its a good question, here is the answer

it has nothing to do with temprature coefficients
Becouse
1) From Boyle's law: Volume is inversly proportional to Pressure at constant Temprature
{ V prop. (1 / P) } at constant T ----------- (a)
2) From Charle's law: Volume is directly proportional to Temprature at constant Pressure
{ V prop. T } at constant P ------------- (b)

From (a) & (b) we get:
Volume is directly proportional to (Temprature divided by Pressure)
{ V prop. (T / P) }

Therefor: V = constant * (T / P)
let the constant = R

(P*V) / T = R ------> (General law of gases)

Therefor: T = (P*V) / R ------> For 1 mole of gas
OR
T = (P*V)/(n*R) -------> For n moles

i hope u got ur point from my explanation