Would the gas become another thing? O2 to O3, for example?
(Sadly I don't know what's an ideal gas, or what it does that a non-ideal one doesn't do.)
(Sadly I don't know what's an ideal gas, or what it does that a non-ideal one doesn't do.)
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http://hyperphysics.phy-astr.gsu.edu/hba…
The information below is from the website above.
An ideal gas is defined as one in which all collisions between atoms or molecules are perfectly elastic and in which there are no intermolecular attractive forces. One can visualize it as a collection of perfectly hard spheres which collide but which otherwise do not interact with each other. In such a gas, all the internal energy is in the form of kinetic energy and any change in internal energy is accompanied by a change in temperature.
In an elastic collision, kinetic energy is conserved. This means no kinetic energy is lost during a collision. In an inelastic collision, heat energy is released during the collision. This means the average velocity of the atoms and molecules would decrease as they collided. This means the average kinetic energy of the atoms and molecules would decrease as time passes. Temperature measures the average kinetic energy of the atoms. So, the temperature of the gas would decrease, without any change of pressure of volume.
Charles’ and Boyles’ gas laws would not work if this happens.
If there are intermolecular attractive forces, some of the atoms and molecules would bond as they collide. Now the number of atoms and molecules is decreasing.
This is like your O2 to O3 example.
And when atoms or molecules bond, during a collision, the collision is perfectly “inelastic”. So KE and temperature decreases as described above.
Let’s say that atoms and molecules were similar to very sticky silly putty. When they collide, they stick together. In a few seconds, the gas molecules will no longer exist.
At STP, one mole of atoms or molecules of an ideal gas occupies 22.4 liters of space.
At STP, one mole of atoms or molecules of a non-ideal gas occupies a tiny space in the bottom of the container.
All of the 6.02 * 10^23 atoms and molecules bonded together into one very small “polymer”.
The information below is from the website above.
An ideal gas is defined as one in which all collisions between atoms or molecules are perfectly elastic and in which there are no intermolecular attractive forces. One can visualize it as a collection of perfectly hard spheres which collide but which otherwise do not interact with each other. In such a gas, all the internal energy is in the form of kinetic energy and any change in internal energy is accompanied by a change in temperature.
In an elastic collision, kinetic energy is conserved. This means no kinetic energy is lost during a collision. In an inelastic collision, heat energy is released during the collision. This means the average velocity of the atoms and molecules would decrease as they collided. This means the average kinetic energy of the atoms and molecules would decrease as time passes. Temperature measures the average kinetic energy of the atoms. So, the temperature of the gas would decrease, without any change of pressure of volume.
Charles’ and Boyles’ gas laws would not work if this happens.
If there are intermolecular attractive forces, some of the atoms and molecules would bond as they collide. Now the number of atoms and molecules is decreasing.
This is like your O2 to O3 example.
And when atoms or molecules bond, during a collision, the collision is perfectly “inelastic”. So KE and temperature decreases as described above.
Let’s say that atoms and molecules were similar to very sticky silly putty. When they collide, they stick together. In a few seconds, the gas molecules will no longer exist.
At STP, one mole of atoms or molecules of an ideal gas occupies 22.4 liters of space.
At STP, one mole of atoms or molecules of a non-ideal gas occupies a tiny space in the bottom of the container.
All of the 6.02 * 10^23 atoms and molecules bonded together into one very small “polymer”.