Truly chaotic – the gaseous state
The kinetic-molecular model of gases describes the gaseous state as one in which gas particles are spaced out relative to one another and are moving around with rapid, random motion.
Calculations based on this model reveal a number of interesting facts:
The average distance between particles is about 10 times the particle diameter – for oxygen, this distance is 3.54 nm.
There is a wide range of particle speeds within this rapid random motion, and it is possible to calculate an average value, which depends on the temperature of the gas and the mass of the gas particle. For example, at standard temperature (0°C) and pressure (101.3 kPa), referred to as STP, the average speed of an oxygen molecule is 425 m/s and the average speed of a hydrogen molecule is 1845 m/s. These are staggeringly high speeds!
The mean free path is the distance a given gas particle moves before colliding either with the walls of the container or with another particle. For oxygen at STP, the mean free path is 63 nm. This is an exceptionally small distance.
The number of collisions occurring per second for a given molecule can be calculated by dividing the average speed by the mean free path. For an oxygen molecule at STP, this is close to 7 billion collisions per second!
Oxygen on a macro and molecular level
The gaseous state is truly chaotic on the molecular level, but at the macroscopic level, external inspection of a sample of oxygen gas at STP reveals a colourless gas that seems to be sitting still in its containing vessel.
Properties of gases explained
Properties of gases explained
The kinetic-molecular model helps to explain some of the properties of gases.
Relationship between gas pressure and gas volume
While studying the compressibility of gases, Robert Boyle (1627–1691) discovered that, for a fixed amount of gas at a given temperature, if the pressure acting on it is doubled, the volume of the gas is halved.
This inverse relationship between the pressure acting on a gas and its volume is known as Boyle’s Law, which takes the mathematical form P1V1=P2V2. In each case, the product of the pressure and the volume is a constant.
Relationship between gas volume and gas temperature
In 1787, French scientist Jacques Charles discovered that the volume of a fixed amount of gas held at constant pressure decreased with decreasing temperature. If the temperature is measured in kelvin rather than °C, the relationship is a directly proportional one. Charles’s Law takes the mathematical form V1/T1 = V2/T2.
Combining Boyle’s Law and Charles’s Law
For a fixed amount of gas, these three relationships can be combined to give the form P1V1/T1 = P2V2/T2. This equation is known as the general gas law.
The general gas law
For a fixed amount of gas, the relationships between gas volume, gas temperature and gas pressure can be combined to give the equation known as the general gas law.
Here is an example of how the general gas law is applied. Weather balloons are filled with helium (or less expensive hydrogen) gas. When released, they move up through the troposphere, and the attached instruments send back information about temperature, pressure, wind speed and humidity.
Suppose a 5000 L balloon is launched when the temperature is 17°C and the pressure 1000 hPa. If it ascends to a height of 35 km where the temperature is -33°C and the pressure 150 hPa, what will the volume of the balloon now be?
Now P1V1/T1 = P2V2/T2 and P1= 1000 hPa; V1 = 5000 L; T1 = 17 + 273 = 290 K
P2= 150 hPa; V2 = ? L; T2 = -33 + 273 = 240 K
Rearranging for V2 gives:
V2 = P1V1T2/P2T1
= (1000 x 5000 x 240)/150 x 290
= 27586.2 L
The balloon has expanded to 5.5 times its original volume. It is most likely that the balloon would have burst before reaching this altitude.
Weather balloon being released
A weather balloon filled with hydrogen gas is about to be released. As it ascends through the atmosphere, the attached instrument package relays information about temperature, pressure, humidity and wind speed to the ground operator.
Nature of science
A scientific law is a statement of fact meant to explain, in simple terms, an action or set of actions. It is generally accepted to be true and universal and can sometimes be expressed in terms of a single mathematical equation. For example, the changing volume of a gas with changing pressure embodied in Boyle’s Law can be expressed as P1V1=P2V2.
Related content
Use this timeline for a look at some of the historical aspects in the development of our understanding of gases and plasmas.
Activity ideas
Try these activities with your students, to help them understand more about fases and plasmas
Diffusion and effusion – students complete a laboratory experiment to gain a basic understanding of diffusion and effusion and then investigate carbon monoxide and hydrogen sulfide.
Gas properties – students investigate gas compressibility and gas expansion in a quantitative way – the end result will be an appreciation of Boyle’s Law and Charles’s Law.
Atmospheric pressure – students indirectly measure atmospheric pressure using a plastic drink bottle and a ping pong ball, they will then use this measure to calculate the force acting on the outside of a soft drink can.
Relative humidity and thermal comfort – students measure the relative humidity in their classroom and in a sheltered playground location and relate the relative humidity and temperature in the classroom to thermal comfort levels.
