Laboratory Report 1:

Chemistry 1502ENG

Date of Experiment: 17/08/2010

Due Date: 31/08/2010

Introduction:

In comparison to solids and liquids, gases have many distinctive characteristics such as, it’s compressibility and it’s ability to obtain the volume (shape) of its container. Such properties of gases are vital to society and industries for essential science based theory. Boyle’s Law sometimes referred as the Boyle-Mariotte Law is one of several gas laws as well as a special case of the Ideal Gas Law. Generally, Boyle’s laws explain the inversely comparative relationship among the complete pressure and capacity of gas, if the temperature is reserved in stable within a closed system. The mathematical expression for Boyles Law is:

V=K(1/P) or PV=K (Constant T and n)

Where, P and V are the pressure and volume of the gas sample respectively. K is a constant and dependent of the temperature (T) and the amount of gas (n, moles).

The Graph below successfully indicates Boyle’s Law visually:

A: Volume Verses Pressure

B: Volume Verses 1/P

Part I of this experiment was specifically designed to validate Boyle’s Law, through the use of a homemade barometer. The open-end tube of the barometer, when moved to different heights above or below its equilibrium, visually achieves the application of various pressures (P) in which the volume (V) corresponding to it, can be measured. If pressure (P) times the corresponding volume (V) is a constant within the experimental error, it validates Boyle’s Law as the “volume of a sample of gas at a given temperature varies inversely with the applied pressure”.

To conduct this experiment in a simplistic and yet effective way, the one-dimensional variable L – the length of the trapped air was measured instead of the measurement of the gas volume, V- a three dimensional factor. However a new expression of Boyle’s Law can be obtained to met what is preferred for the

References: * Lab Manual - Chemistry Lecture Slides (Gases)