NTRODUCTION In this experiment the validity of Gas Laws were observed and the relationship of two variables, temperature and volume, against pressure was tested. Gas Laws are encompassed by the Ideal Gas Law in which PV=nRT observes the general behavior of a gas under ideal conditions in terms of pressure(P), volume(V), moles of gas(n), gas constant(R), and temperature(T). The Ideal Gas Law is a combination of Boyle 's Law, Charles ' Law and Avogadro 's Law and was first introduced in 1834 by Emile Clapeyron. For the purposes of this experiment, attention is given to Boyle 's Law and Guy-Lussac 's Law. British scientist Robert Boyle discovered the relationship between volume and pressure by using a J-tube and observing the volume that the gas
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The appropriate units for the constant is kPa/K as the pressure is measured in kPa and the temperature is measured in Kelvin and Pressure was divided by Temperature. The expected pressure of the gaseous sample at a temperature of -50 degree Celsius or 223 Kelvin is calculated to be 72.525kPa and the pressure at a temperature of 200 degree Celsius or 473 Kelvin is calculated to be 153.83kPa using the constant .3252225kPa/K and the equation P=TK according to Gay-Lussac 's Law. The expected pressures of the gaseous sample at temperatures of 223Kelvin and 473Kelvin, using the equation for the trendline in the Part B graph y=0.2643x+19.98, is calculated to be 78.9189kPa and 144.9939kPa respectively. The results are similar but not quite exact compared to the calculated pressures from question 7. A source of error within the experiment that could account for this discrepancy could be the fact that the constant is made up of only the averages of four values compared to the numerous data pairs that the graph uses. A difference in constant may cause differences in the calculated
The appropriate units for the constant is kPa/K as the pressure is measured in kPa and the temperature is measured in Kelvin and Pressure was divided by Temperature. The expected pressure of the gaseous sample at a temperature of -50 degree Celsius or 223 Kelvin is calculated to be 72.525kPa and the pressure at a temperature of 200 degree Celsius or 473 Kelvin is calculated to be 153.83kPa using the constant .3252225kPa/K and the equation P=TK according to Gay-Lussac 's Law. The expected pressures of the gaseous sample at temperatures of 223Kelvin and 473Kelvin, using the equation for the trendline in the Part B graph y=0.2643x+19.98, is calculated to be 78.9189kPa and 144.9939kPa respectively. The results are similar but not quite exact compared to the calculated pressures from question 7. A source of error within the experiment that could account for this discrepancy could be the fact that the constant is made up of only the averages of four values compared to the numerous data pairs that the graph uses. A difference in constant may cause differences in the calculated