Boyle's law and charle's law  (Page 4/6)

Boyle's law

1. An unknown gas has an initial pressure of 150 kPa and a volume of 1 L. If the volume is increased to 1.5 L, what will the pressure now be?
2. A bicycle pump contains 250 cm ${}^3$ of air at a pressure of 90 kPa. If the air is compressed, the volume is reduced to 200 cm ${}^3$ . What is the pressure of the air inside the pump?
3. The air inside a syringe occupies a volume of 10 cm ${}^3$ and exerts a pressure of 100 kPa. If the end of the syringe is sealed and the plunger is pushed down, the pressure increases to 120 kPa. What is the volume of the air in the syringe?
4. During an investigation to find the relationship between the pressure and volume of an enclosed gas at constant temperature, the following results were obtained.

   Volume (cm ${}^3$ )	Pressure (kPa)
   40	125.0
   30	166.7
   25	200.0

   1. For the results given in the above table, plot a graph of pressure (y-axis) against the inverse of volume (x-axis).
   2. From the graph, deduce the relationship between the pressure and volume of an enclosed gas at constant temperature.
   3. Use the graph to predict what the volume of the gas would be at a pressure of 40 kPa. Show on your graph how you arrived at your answer.
   ( IEB 2004 Paper 2 )

Charles' law: volume and temperature of an enclosed gas

Charles' law describes the relationship between the volume and temperature of a gas. The law was first published by Joseph Louis Gay-Lussac in 1802, but he referenced unpublished work by Jacques Charles from around 1787. This law states that at constant pressure, the volume of a given mass of an ideal gas increases or decreases by the same factor as its temperature (in kelvin) increases or decreases. Another way of saying this is that temperature and volume are directly proportional .