Boyles Law Apparatus

Abstract

The objective of this lab was to determine the relationship (if any), between the pressure and volume of a gas given the temperature and # of molecules remained constant. Using the Boyle’s law apparatus, and textbooks to demonstrate pressure it was concluded that there was a relationship between pressure and volume. However, the relationship was not a direct relationship, and it was determined that the pressure and volume of a gas are inversely proportioned. Thus,proving Boyle’s theory correct.

Introduction

Objectives: The main objective of this lab was to determine the relationship between the volume and pressure when the temperature and number of molecules remains the same throughout. Other minor objectives of this lab were to determine any possible source of error, so there is more awareness of these errors when conducting another experiment.

Theory: Gases are matter with no definite volume or shape. They will take on the volume and shape of whatever they are being contained in. There are three gas laws. The first is Boyle’s Law. Boyle’s law states that at a maintained temperature, and number of molecules, the volume and pressure of a gas are inversely proportional to each other. Which simply means that the higher the pressure is on a gas, the lower the volume of the gas will be, and vice-versa. The formula for this law is: P№V№=PІVІ. V№ is the old volume, and P№ is the old pressure. VІ is the new volume and PІ is the old pressure. The second gas law is Charles Law. Charles Law states that there is a direct relationship between volume & temperature(K). As Volume increases, so does Temperature, by the same ratio. The third gas law is the Combined Law. The combined law deals with any combination of Pressure, Volume and temperature. The combined law states that Pressure and Temperature are directly proportioned. P№V№ Over T№ = PІVІ Over TІ.

The Kinetic Theory of Gases states that:

1) A gas is composed of particles that are in continuous random motion.

2) There is a transfer of energy between colliding particles, but no energy is lost.

3) The volume of gas particles is almost non-significant in comparison with the volume of space they are in. There is much space between particles.

4) Gas particles are considered as having no force of attraction for each other.

This Kinetic theory applies to all ideal gases.