Unlike solids and liquids, gases are known to have both variable volume and pressure. The gas laws were formulated in the late 18th century by various scientists to develop a relationship between the volume, pressure, temperature, and the number of moles of a gas.1 This has allowed scientists today to manipulate these variables in controlled lab settings, to utilize these laws in new innovations such as ventilation systems, and to explain observed biological phenomenon like breathing.
Boyle’s Law, the first of these gas laws, was published in 1662, and developed an inverse relationship between pressure and volume, provided that the temperature and the number of moles of gas remained constant.1 It is illustrated by the equation PV = k1, where …show more content…
The constants are then used to measure pressure values at different volumes or temperatures. The experimental volume and pressure are multiplied to calculate the constant for Boyle’s law in part A. To calculate the constant for Gay-Lussac’s Law in part B, the pressure readings are divided by the temperature readings. The four values for the constant obtained with both these equations are added and divided by four to obtain the average value for the constants. To find pressure at a different volume, the constant for Boyle’s law is divided by the new volume. To find pressure at a different temperature, the constant for Gay-Lussac’s Law is multiplied by the new …show more content…
The mode was changed to “Events with Entry” so that data could be collected at the appropriate pressures. The plunger of a 20 mL syringe was pulled to the 10 mL mark, and was then connected to the valve of the gas pressure sensor. To account for the volume of air in the valve, 0.8 mL was added to the volume readings recorded in the LabQuest. A boiling water bath was started in a 600 mL beaker filled to the 400 mL mark for part B of the experiment.
Then, the plunger was depressed to the 5 mL mark, and a data point was collected for the pressure and volume once the readings had stabilized. The volume was recorded to be 5.8 mL to account for the volume of air in the sensor. These steps were repeated to obtain data points for 7 mL, 9 mL, 11 mL, 13 mL, 15 mL, 17 mL, and 19 mL. A volume of 0.8 mL was added to each of these volumes to account for air in the sensor. After data collection was completed, the data was saved on a
Boyle’s Law, the first of these gas laws, was published in 1662, and developed an inverse relationship between pressure and volume, provided that the temperature and the number of moles of gas remained constant.1 It is illustrated by the equation PV = k1, where …show more content…
The constants are then used to measure pressure values at different volumes or temperatures. The experimental volume and pressure are multiplied to calculate the constant for Boyle’s law in part A. To calculate the constant for Gay-Lussac’s Law in part B, the pressure readings are divided by the temperature readings. The four values for the constant obtained with both these equations are added and divided by four to obtain the average value for the constants. To find pressure at a different volume, the constant for Boyle’s law is divided by the new volume. To find pressure at a different temperature, the constant for Gay-Lussac’s Law is multiplied by the new …show more content…
The mode was changed to “Events with Entry” so that data could be collected at the appropriate pressures. The plunger of a 20 mL syringe was pulled to the 10 mL mark, and was then connected to the valve of the gas pressure sensor. To account for the volume of air in the valve, 0.8 mL was added to the volume readings recorded in the LabQuest. A boiling water bath was started in a 600 mL beaker filled to the 400 mL mark for part B of the experiment.
Then, the plunger was depressed to the 5 mL mark, and a data point was collected for the pressure and volume once the readings had stabilized. The volume was recorded to be 5.8 mL to account for the volume of air in the sensor. These steps were repeated to obtain data points for 7 mL, 9 mL, 11 mL, 13 mL, 15 mL, 17 mL, and 19 mL. A volume of 0.8 mL was added to each of these volumes to account for air in the sensor. After data collection was completed, the data was saved on a