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Basic properties of gases

In gases, each molecule moves at a relatively high rate independently of the others. This is why gases tend to expand and fill every space available to them. The distance between molecules in gases is very large and therefore there is virtually no effect of molecular forces. Gases do not have a certain volume as liquids, but rather: they must be stored in closed vessels and the volume of the vessel is at the same time a volume of gas, and it is easily changed with pressure, which is not the case for liquids or solids.

If there is an obstacle (the vessel walls) in the path of the gas molecule, they hit that obstacle and put pressure on it. Therefore, gas that is closed to a vessel puts pressure on the court walls everywhere equally.

The gas can also be compressed when the external forces are insignificant, which means that the distance between the gas molecules is large.

The gases expand spontaneously, which means that the attractive forces of their molecules are very weak. Because interactions between gas molecules are weak, the potential energy among gas molecules can be neglected. Therefore, gas molecules can be considered to have only kinetic energy.

The pressure of a certain amount of gas is even greater if the volume of the vessel is smaller, because the molecules then strike the walls of the vessel more often, which causes an increase in pressure. In addition, the gas pressure increases with increasing temperature, because the molecules hit the vessel walls faster. On this basis it can be concluded that gas pressure is constant if its volume and temperature are constant.

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Written by michael

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