A-level Physics (Advancing Physics)/Ideal Gases
Real-world gases can be modelled as ideal gases. An ideal gas consists of lots of point particles moving at random, colliding with each other elastically. There are four simple laws which apply to an ideal gas which you need to know about:
Boyle's Law states that the pressure of an ideal gas is inversely proportional to its volume, assuming that the mass and temperature of the gas remain constant. If I compress an ideal gas into half the space, the pressure on the outsides of the container will double. So:
Charles' Law states that the volume of an ideal gas is proportional to its temperature:
T must be measured in kelvin, where a rise of 1°K is equal to a rise 1°C, and 0°C = 273°K. If we double the temperature of a gas, the particles move around twice as much, and so the volume also doubles.
This law states that the pressure of an ideal gas is proportional to the amount of gas. If we have twice the number of gas particles N, then twice the pressure is exerted on the container they are in:
A mole is a number of particles. 1 mole = 6.02 x 1023 particles. So, the pressure of a gas is also proportional to the number of moles of gas present n:
The pressure law states that the pressure of an ideal gas is proportional to its temperature. A gas at twice the temperature (in °K) exerts twice the pressure on the sides of a container which it is in:
These laws can be put together into larger formulae linking p, V, T and N.
1. I heat some argon from 250K to 300K. If the pressure of the gas at 250K is 0.1 MPa, what is its pressure after heating?
2. The argon is in a 0.5m long cylindrical tank with radius 10cm. What volume does it occupy?
3. The argon is then squeezed with a piston so that in only occupies 0.4m of the tank's length. What is its new pressure?
4. What is its new temperature?
5. 25% of the argon is sucked out. What is its pressure now?