Under standard temperature and pressure, which would be 100 kPa (1.0 bar) and 273.15 K (0 oC). This is not correct. The answer is at high temperature and low pressure, according to my college prof.
There are two assumptions that you make when you say that a gas acts ideally: 1. The molecules have no intermolecular forces, so when they collide they do not stick at all (they have purely elastic collisions) 2. The molecules have no volume, so the space they have to move around in is equal to the volume of the container. In reality: 1. Molecules DO have intermolecular forces, so when they collide they lose energy overcoming the intermolecular forces. This means that there next collisions with the wall will be less forceful because they are moving slower and so the pressure they exert is lower. 2. Molecules DO have volume, and so if you have a lot of molecules and a small space, the pressure turns out to be higher because there is less volume for them to move around in and they impact the walls more frequently. So the following are all ways to make a real gas look ideal: 1. Pick a gas that is small and has really weak intermolecular forces. Helium is a perfect example---really small atom and extremely weak dispersion forces between helium atoms. 2. Make the volume of the container really big. This minimizes the amount of volume lost to the volume of the particles. It also spreads the molecules out so that the number of gas particle collisions decreases, minimizing the effect of intermolecular forces. 3. Crank the temperature way up. This does not help with the volume problem, but with a lot of kinetic energy you will hardly notice the molecules attracting each other because the potential energy of the attraction is so small compared to the molecules' kinetic energies.
Noble or inert gases like helium, argon, neon, and xenon behave most like an ideal gas.
Answer is as the pressure is lowered and or the temperature is increased almost all gases show close agreement with the ideal gas equation
When high temperatures and low pressure are used.
Yes...at 1 atmosphere pressure and70 degrees F.
at high pressure and low temperature.
At higher temperatures and lower pressure
When its the same numbers being added
PV =nRT
At 1 atm, because the pressure is lower.
gases behave ideally at high temperature and low pressure at 273kthe temperature in celcius is o degree which is a very low temperature and atlow temperature forces of attraction becomes significant so they behave non ideally
Yes. The three types of matter are solids, liquids, and gasses.
What causes greenhouse gasses? I dont know why do you even ask?
Helium
PV =nRT
ideal gasses have two properties 1. a low pressure 2. high temperatures
At 1 atm, because the pressure is lower.
They say he is real because they want you to behave
Yes, if the pressure is low.
P waves travel through solids, liquids, and gasses.
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Gases behave most ideally at low pressure and high temperatures. At low pressures, the average distance of separation among atoms or molecules is greatest, minimizing interactive forces. At high temperatures, the atoms and molecules are in rapid motion and are able to overcome interactive forces more easily.
There are real zebras, penguins, giraffes, and lions, but, they do not behave in real life like the animated characters do in the cartoon Madagascar.
[P + a(n/V)2] (V - nb) = nRT As you see this is a correction method for gasses other than ideal. Gasses at high pressure and high/low temperature. The ideal gas equation makes assumptions that are not always applicable to real word conditions as to gasses.