Chapter 10: Properties of Gases
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a form of matter that does not have a definite volume or shape
3 main properties of a fixed amount of gas
temperature, pressure and volume
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17 Terms
gas
a form of matter that does not have a definite volume or shape
3 main properties of a fixed amount of gas
temperature, pressure and volume
2 scales of temperature used in science
Celsius scale and Kelvin scale
Celsius scale range
0°C to 100°C
Kelvin scale range
0K to 273K
standard temperature
273K
Five Gas Laws
Boyle's Law, Charles' Law, The Combined Gas Laws, Gay-Lussac's Law, Avogadro's Law
Boyle's Law
At constant temperature, the volume of a fixed mass of gas is inversely proportional to its pressure.
Charles' Law
at constant pressure, the volume of a fixed mass of gas is directly proportional to its temperature measured on the Kelvin Scale
Gay-Lussac's Law of Combining Volumes
In a reaction between gases, the volumes of the reacting gases and the volumes of any gaseous products are in the ratio of small whole numbers provided the volumes are measured at the same temperature and pressure
The Combined Gas Law
P1V1/T1 = P2V2/T2
Avogadro's Law
Equal volumes of gases, under the same conditions of temperature and pressure, contain equal numbers of molecules.
molar volume of all gases at s.t.p
22.4L
5 assumptions of the kinetic theory of gases
1: Gas molecules move in continuous random motion, colliding with one another and their boundaries.
2: There are no forces of attraction and repulsion between gas molecules.
3: Due to gas molecules being tiny, the volume of gas molecules is negligible compared with distances between gas molecules and the space they occupy.
4: When molecules collide, the collisions are perfectly elastic.
5: The average kinetic energy of gas molecules is proportional to the temperature.
Kinetic theory limitations
In real gases: forces of attraction and repulsion exist between molecules.
The volume of the gas molecules is not negligible.
ideal gas
an imaginary gas that obeys all the assumptions of the kinetic theory of gases under all conditions of temperature and pressure
real gas
a gas that does not behave completely according to the assumptions of the kinetic theory of gases