To calculate the pressure of the gas the partial pressure of the water must be subtracted from the pressure in the container. The amount of water vapor the gas picks up only depends on the temperature. The reason for this is as the gas bubbles through the water the gas picks up water vapor.

To obtain the pressure of gas collected over water the partial pressure of the water must be taken into consideration. Gases properties can be compared using STP as a reference. STP is O o Celcius and 1 atmosphere of pressure. STP is Standard Temperature and Pressure. Note: Charles's Law is fairly accurate but gases tend to deviate from it at very high and low pressures. Important: Charles's Law only works when the pressure is constant.

T is the absolute temperature (measured in Kelvin)Д¬harles's Law can be rearranged into two other useful equations.

If the pressure is increased to 800mm and the temperature remains constant then according to Boyle's Law the new volume is 42.8 ml.Д¬harles's Law can be stated as the volume occupied by any sample of gas at a constant pressure is directly proportional to the absolute temperature. Suppose you have a gas with 45.0 ml of volume and has a pressure of 760.mm. Mathematically Boyle's law can be expressed as P 1V 1 = P 2V 2 Properties of Gases | Boyle's Law | Charles's Law | STP and Gas Collected over Water | Combined Law | Ideal Gas Law | Top of Page | Questions | GlossaryД«oyle's Law states the volume of a definite quantity of dry gas is inversely proportional to the pressure, provided the temperature remains constant. This dimensional analysis method of canceling the units will work for changing from any unit to another. If you are in atms and want to convert to mmHg then # of atms * (760 mmHg / 1 atm) = # of mmHg because the atms cancel. Here is a list of equivalent amounts of pressure: To achieve this there has to be a conversion factor to move from one unit to another. Conversion from one unit of pressure to another is very important. Many of the properties of gases can be measured in different ways. The picture illustrates the compressing of a gas. However, if the gas is compressed to only take up one half a liter then the density will change to 1 gram/liter. 50 grams and the volume of the gas is one liter then the density of the gas is. This can be observed by using the density equation D=m/V. Since the mass remains the same and the volume decreases, the density of the gas is greater. The mass of the gas will remain unchanged. Since one of the properties of a gas is compressiblity, a gas at a certain volume can be compressed by adding pressure. An example of effusion is if a coke bottle had a small hole in it just small enough for the gas inside to escape. An example of diffusion is the ammonia mentioned earlier where the ammonia moves into the room with the air. Effusion occurs when a gas moves through a small hole in its current container into another container. Diffusion is a process in which a gas enters a container with another gas and the two mix to form a uniform mixture.

The average kinetic energy of a molecule is proportional to the absolute temperature.Д®ffusion and Diffusion are the two ways that gases mix with other gases.

When molecules collide with one another, the collisions are elastic no kinetic energy is lost.

The forces of attraction or repulsion between two molecules in a gas are very weak or negligible, except when they collide.

Molecules move randomly in straight lines in all directions and at various speeds.

Gases are composed of molecules whose size is negligible compared to the average distance between them.

The five postulates to the Kinetic Theory are as follows: The Kinetic Molecular Theory is the basis of the many properties of gases. An example of this is a bottle of ammonia being opened in a room and the smell traveling throughout the room. A gas will fill whatever container that it is in. Gas has a low density because its molecules are spread apart over a large volume. It can be measured in several units such as kilopascals (kPa), atmospheres (atm), and millimeters of Mercury (mmHg). Pressure is defined as force exerted per unit area of surface. Gases are easily expandable and compressible unlike solids and liquids.

Don't get it wrong, just because they are the simplest doesn't mean that they are not one of the most interesting and useful states of matter.

Gases are also the least complex state of matter. The main distinguishing property of gases is their uncanny ability to be compressed into smaller and smaller spaces.

18.7 mmhg to atm