1 1.2 Lab Activities
Utilizing the equations from the workbook, the examples below, and other resources, you will complete the following questions on a separate sheet of paper and discuss the answers with your lab partner and then submit your responses to your laboratory instructor by the end of class.
Boyle’s Law
An example of Boyle’s Law would be the act of breathing when the diaphragm drops, and the pressure drops in the thorax. There will be gas moving into the lungs.
1. The initial volume is 6,400 mL, and the initial pressure is 720 mm Hg. What is the new pressure if the volume changes to 4.75 L?
2. The first volume is 2.22 L, which exerts a pressure of 450 mm Hg. If the volume changes to 4.8 L, what is the new pressure exerted by the gas?
3. The initial volume of the gas is 1.85 L, and the initial pressure is 755 mm Hg. What is the new volume if the pressure changes to 740 mm Hg?
4. The first volume is 3.64 L, which exerts a pressure of 760 mm Hg. If the pressure changes to 725 mm Hg, what is the new volume of the gas?
Charles’s Law
An example of Charles’s Law is when tire pressure in the summer increases due to the warmer weather, and in the winter the tire pressure decreases due to the colder weather.
1. The temperature of the gas is 36° C, with a gas volume of 5.12 L. What is the new volume if the temperature increases to 39° C?
2. The temperature of the gas is 41° C, with a gas volume of 4.66 L. What will be the new volume if the temperature decreases to 23° C?
3. The temperature of the gas is 37° C, with a gas volume of 2.98 L. What will be the new volume if the temperature decreased to 25° C?
Gay-Lussac’s Law
An example of Gay-Lussac’s Law is an oxygen cylinder in the trunk of a car will have an increase in pressure when the temperature increases from 80 to 100 degrees Fahrenheit.
1. The temperature of the gas is 22° C, and it exerts a gas pressure of 740 mm Hg. What is the new pressure if the temperature increases to 35° C?
2. The temperature of the gas is 21° C, and it exerts a gas pressure of 545 mm Hg. What is the new pressure if the temperature increases to 25° C?
3. The temperature of the gas is 25° C and exerts a gas pressure of 695 mm Hg. What is the new pressure if the temperature increases to 37° C?
Combined Gas Law
The Combined Gas Law is really just a combination of all three gas laws affecting pressure, temperature, and volume.
1. The temperature of a gas is 25° C, with a gas volume of 5.25 L, which exerts a pressure of 740 mm Hg. What will the new pressure be if the temperature increases to 36° C, and the volume decreases to 4.7 L?
2. The temperature of a gas is 39° C, with a gas volume of 6.1 L, which exerts a pressure of 688 mm Hg. What will be the new volume if the temperature decreases to 29° C, and the pressure decreases to 515 mm Hg?
3. The temperature of a gas is 28° C, with a gas volume of 6.3 L, which exerts a pressure of 752 mm Hg. What will be the new temperature if the pressure decreases to 720 mm Hg, and the volume increases to 6.8 L?
Dalton’s Law
An example of Dalton’s Law would be a high-altitude climber (i.e., Mount Everest) where the air is so thin, people must breathe pressurized O2, or they will not be able to remember the event due to the very low O2 concentrations at that height. Another example is a hyperbaric chamber where a patient will breathe 100% O2 at barometric pressure or when treating a patient with carbon monoxide exposure after the CO is liberated from the hemoglobin with the O2 at that higher pressure.
1. What is the total pressure of a gas mixture if the PO2 = 90 mm Hg, PCO2 = 40 mm Hg, PN2 = 573 mm Hg, and PH2O = 47 mm Hg?
2. The total pressure of a gas mixture is 847 mm Hg. If the PCO2 = 47 mm Hg and the PH2O = 47 mm Hg, what is the pressure of the remaining gases?
