The molecules in a gas at 100k
The volume occupied by gas molecules is negligible when compared to volume occupied by the gas.The collisions between gas molecules-gas molecules and gas molecules-walls of the container are perfectly elastic.
Gas pressure is caused by the molecules of gas striking the walls of a container, or in the case of Earth's atmosphere, the molecules of air hitting the earth. In a vacuum, there are no gas molecules. No molecules, no pressure.
Nitrogen gas consists of N2 molecules.
when air(gas) is cooled(thermal energy is removed) its molecules slow down and it becomes a liquid(condensation) when air(gas) is heated(thermal energy is added) its molecules speed up, but it wont change into a different phase until gas is heated to a temperature above 10,000 C, which removes electrons from the atoms
The molecules in a liquid are bound by moderate attractions, neither weak nor strong. So, liquid molecules move around a bit, but they are not as free-flowing as the molecules of a gas. Still, attractions are continually created and broken in a liquid.
Water does not behave exactly like an ideal gas because water is a polar molecule. And, the polar molecules of water, if properly oriented in space, have strong attraction to one another, and may form a hydrogen bond and condense back into liquid form. Also, when a gaseous water molecule has a collision with liquid water, if it is oriented in the right way (i.e. an oxygen atom comes into contact with a hydrogen atom), it will move back into the liquid phase. So, because water molecules move back into the liquid phase much more easily than ideal gas molecules, water vapor does not behave exactly as an ideal gas would.
The molecules in a gas at 100k
Solids - Bonds between molecules are strong, holding a constant form with a definite mass. Liquids - Bonds between molecules are not as strong, still have a definite mass due to their temperature and take the form of the container. Gases - Molecules float freely with and are impossible to get a definite mass or volume on an open sample.
The volume occupied by gas molecules is negligible when compared to volume occupied by the gas.The collisions between gas molecules-gas molecules and gas molecules-walls of the container are perfectly elastic.
a gas can be molecules
Gas pressure is caused by the molecules of gas striking the walls of a container, or in the case of Earth's atmosphere, the molecules of air hitting the earth. In a vacuum, there are no gas molecules. No molecules, no pressure.
Polar molecules have charges that non-polar molecules do not have. It is the reason why non-polar molecules can move through the lipid bilayer quicker than the polar molecules.
The atmosphere is made of gas molecules.
Gas expands the quickest because gas molecules are farther apart than molecules of other substances. Gas molecules also move faster.
NH3, as in Ammonia, like all real gases, are not ideal. Ideal gases follow the ideal gas laws, but ammonia does not adhere to a few of them. First of all, the volume of its molecules in a container is not negliggible. Next, NH3 molecules have intermolecular hydrogen bonding, which is a strong intermolecular bond. Thus, the forces of attaction between molecules is not neglible. All real gases have a certain degree of an ideal gas, but no real gas is actually ideal, with H2 being the closest to ideal.
liquid molecules forming a gas and gas molecule forming a liquid are equal in number