Experiment: Boyle´s Law And Gay-Lussac's Law

In this experiment, Boyle’s Law and Gay-Lussac’s law were tested, using a gas pressure sensor and a temperature probe, in order to produce constants for both these laws. In Part A, a setup with a 20 mL syringe and a gas pressure sensor was used to measure the effect of a change in volume on the pressure of a gas, and to obtain various data points that were used to measure 4 values for a Boyle’s Law constant. In part B, a setup with a water bath, and a rubber stopper assembly in an Erlenmeyer flask was used to measure the change in pressure of a gas when temperature was changed, and to obtain 4 values for a Gay-Lussac’s Law constant. These sets of four values were averaged to provide 2 average constants, which were used to measure pressure at different volumes and temperatures respectively.
The data from Part A was used to confirm an inverse relationship between the volume of a confined gas, and its pressure. If the volume in the syringe was decreased, the pressure of the gas inside the syringe was observed to increase. This relationship was described by the equation for Boyle’s law, PV = kPartA, where P was pressure in kilo Pascals, V was volume in milliliters, and kPartA was the constant for part A. This …show more content…
At -50℃, or 223 K, the pressure was found to be 72.81 kPa. At 200℃, or 473 K, the pressure was found to be 154.44 kPa. These values were also calculated using the equation of the trendline from the graph, to predict a more accurate value. The equation y=mx+b was used to calculate this value, where y was the pressure in kilo Pascals, m was 0.2735 kPa/K, the slope of the trendline, x was the temperature in Kelvin, and b was 17.39 kPa, the y-intercept of the trendline. Using this equation, the pressure at -50℃ was found to be 78.38 kPa and the temperature at 200℃ was found to be 146.76