The Gas Laws A Tutorial on the Behavior of Gases.

Kinetic Molecular Theory of Gases  Gases consist of small particles that are in constant random motion and are separated by great distances from one another.  The individual particles occupy a negligible volume.

 Collisions with walls of container are elastic and exert a measurable pressure.  Particles do not interact with one another.  Average kinetic energy is directly proportional to the Kelvin (absolute) temperature. Kinetic Molecular Theory of Gases

P – Pressure V – Volume n – Moles R – Gas Constant T – Kelvin Temperature Abbreviations

Units of Pressure atm - atmospheres mm Hg - millimeters of mercury torr – same as mm Hg Pa - Pascal kPa - kiloPascal

1.00 atm = 760 mm Hg = kPa = 101,300 Pa Converting Pressures

Units of Temperature K - Kelvin °C - degrees Celsius °F - degrees Fahrenheit

(  C x 1.8) + 32 =  F Converting Temperatures (  F - 32)/1.8 =  C  C = K

Standard Conditions STP: Standard Temperature and Pressure Temperature: 273 K = 0.0 °C Pressure: 1.00 atm = 760 mm Hg

Boyles Law

Boyle’s Law: the volume of a fixed mass of gas varies inversely with the pressure at constant temperature. Mathematically, it is expressed as PV = k Where k is a constant, V is volume and P is pressure. Robert Boyle ( )

A gas occupies 12.3 liters at a pressure of 400 mm Hg. What is the volume when the pressure is increased to 600 mm Hg and the temperature remains constant? Sample Boyle’s Law Problem P1V1 = P2V2 #1

Answer #1

Sample Boyle’s Law Problem P1V1 = P2V2 #2 A container has volume of 13,240 L has a pressure of 4.78 atm. If the pressure inside the container becomes 260 atm, what would the new volume be?

A sample of neon occupies L at a pressure of 190 kPa. At constant temperature, what is the volume of the neon when the pressure is increased to 631 kPa? Sample Boyle’s Law Problem P1V1 = P2V2 #3