Boyles Law
Boyle’s Law
5-1: Boyle’s Law: Pressure and Volume
Robert Boyle, a philosopher and theologian, studied the properties of gases in the 17th century. He noticed that gases behave similarly to springs; when compressed or expanded, they tend to ‘spring’ back to their original volume. He published his findings in 1662 in a monograph entitled The Spring of the Air and Its Effects. You will make observations similar to those of Robert Boyle and learn about the relationship between the pressure and volume of an ideal gas.
1. Start Virtual ChemLab and select Boyle’s Law: Pressure and Volume from the list of assignments. The lab will open in the Gases laboratory.
2. Note that the balloon in the chamber is filled with 0.300 moles of an ideal gas (MW = 4 g/mol) at a temperature of 298 K, a pressure of 1.00 atm, and a volume of 7.336 L. To the left of the Pressure LCD controller is a lever that will decrease and increase the pressure as it is moved up or down; the digit changes depending on how far the lever is moved. Digits may also be clicked directly to type in the desired number. You may want to practice adjusting the lever so that you can decrease and increase the pressure accurately. Make sure the moles, temperature, and pressure are returned to their original values before proceeding.
3. Click on the Lab Book to open it. Back in the laboratory, click on the Save button to start recording P, V, T, and n data to the lab book. Increase the pressure from 1 atm to 10 atm one atmosphere at a time. Click Stop to stop recording data, and a blue data link will appear in the lab book. To help keep track of your data links, enter ‘Ideal Gas 1’ next to the link.
4. Zoom Out by clicking the green arrow next to the Save button. Click Return Tank on the gas cylinder. On the table underneath the experimental chamber is a switch to choose Real gases or Ideal gases. Click on the Ideal Gases and choose the cylinder labeled Ideal 8 (Ideal 8 MW = 222 g/mol). Click on the
5-1: Boyle’s Law: Pressure and Volume
Robert Boyle, a philosopher and theologian, studied the properties of gases in the 17th century. He noticed that gases behave similarly to springs; when compressed or expanded, they tend to ‘spring’ back to their original volume. He published his findings in 1662 in a monograph entitled The Spring of the Air and Its Effects. You will make observations similar to those of Robert Boyle and learn about the relationship between the pressure and volume of an ideal gas.
1. Start Virtual ChemLab and select Boyle’s Law: Pressure and Volume from the list of assignments. The lab will open in the Gases laboratory.
2. Note that the balloon in the chamber is filled with 0.300 moles of an ideal gas (MW = 4 g/mol) at a temperature of 298 K, a pressure of 1.00 atm, and a volume of 7.336 L. To the left of the Pressure LCD controller is a lever that will decrease and increase the pressure as it is moved up or down; the digit changes depending on how far the lever is moved. Digits may also be clicked directly to type in the desired number. You may want to practice adjusting the lever so that you can decrease and increase the pressure accurately. Make sure the moles, temperature, and pressure are returned to their original values before proceeding.
3. Click on the Lab Book to open it. Back in the laboratory, click on the Save button to start recording P, V, T, and n data to the lab book. Increase the pressure from 1 atm to 10 atm one atmosphere at a time. Click Stop to stop recording data, and a blue data link will appear in the lab book. To help keep track of your data links, enter ‘Ideal Gas 1’ next to the link.
4. Zoom Out by clicking the green arrow next to the Save button. Click Return Tank on the gas cylinder. On the table underneath the experimental chamber is a switch to choose Real gases or Ideal gases. Click on the Ideal Gases and choose the cylinder labeled Ideal 8 (Ideal 8 MW = 222 g/mol). Click on the