Boyle's Law
Examples and problems only

Ten examples

Example #1: 2.00 L of a gas is at 740.0 mmHg pressure. What is its volume at standard pressure?

Example #2: 5.00 L of a gas is at 1.08 atm. What pressure is obtained when the volume is 10.0 L?

Example #3: 9.48 L of a gas was at an unknown pressure. However, at standard pressure, its volume was measured to be 8.00 L. What was the unknown pressure?

Example #4: If we have 6.00 cm³ of gas at a pressure of 10.0 N/cm² and we increase the pressure to 20.0 N/cm², what volume will the gas occupy?

Example #5: What pressure is required to compress 196.0 liters of air at 1.00 atmosphere into a cylinder whose volume is 26.0 liters?

Example #6: The volume of a gas is 6.10 L, measured at 1.00 atm. What is the pressure of the gas in mmHg if the volume is changed to 9.74 L?

Example #7: At 46.0 °C a sample of ammonia gas exerts a pressure of 5.30 atm. What is the pressure when the volume of the gas is reduced to one-eighth (0.125) of the original value at the same temperature?

Example #8: In order to measure the volume of a piece of apparatus, a chemist filled a 750. mL flask with 46.65 kPa pressure of gas, then expanded it into the apparatus. The final pressure was 14.95 kPa. Calculate the total volume occupied by the gas.

Example #9: Boyle's Law deals with the relationship between two of the variables (of four) that describe gas behavior. Which two variables are held constant in Boyle's Law problems?

(a) pressure/moles
(b) temperature/volume
(c) pressure/volume
(d) temperature/moles
(e) volume/moles

Example #10: A balloon contains 7.20 L of He. The pressure is reduced to 2.00 atm and the balloon expands to occupy a volume of 25.2 L. What was the initial pressure exerted on the balloon?

Bonus Example #1: An evacuated flask A, which has a volume of 30 mL, is attached to a second flask B containing an ideal gas at a pressure of 5 atm. When the two flasks are connected the pressure in the system drops to 2 atm. Calculate the volume of flask B.

Bonus Example #2: Three bulbs are connected by tubing, and the tubing is evacuated. The volume of the tubing is 39.0 mL. The first bulb has a volume of 56.0 mL and contains 5.92 atm of argon, the second bulb has a volume of 250.0 mL and contains 1.28 atm of neon, and the third bulb has a volume of 37.0 mL and contains 8.50 atm of hydrogen. If the stopcocks (valves) that isolate all three bulbs are opened, what is the final pressure of the whole system in atm?

Problems 1-15

Problem #1: A gas occupies 12.3 liters at a pressure of 40.0 mmHg. What is the volume when the pressure is increased to 60.0 mmHg?

Problem #2: If a gas at 25.0 °C occupies 3.60 liters at a pressure of 1.00 atm, what will be its volume at a pressure of 2.50 atm?

Problem #3: To what pressure must a gas be compressed in order to get into a 3.00 cubic foot tank the entire weight of a gas that occupies 400.0 cu. ft. at standard pressure?

Problem #4: A gas occupies 1.56 L at 1.00 atm. What will be the volume of this gas if the pressure becomes 3.00 atm?

Problem #5: A gas occupies 11.2 liters at 0.860 atm. What is the pressure if the volume becomes 15.0 L?

Problem #6: 500.0 mL of a gas is collected at 745.0 mmHg. What will the volume be at standard pressure?

Problem #7: Convert 350.0 mL at 740.0 mmHg to its new volume at standard pressure.

Problem #8: Convert 338 L at 63.0 atm to its new volume at standard pressure.

Problem #9: Convert 273.15 mL at 166.0 kPa to its new volume at standard pressure.

Problem #10: Convert 77.0 L at 18.0 mmHg to its new volume at standard pressure.

Problem #11: When the pressure on a gas increases, will the volume increase or decrease?

Problem #12: If the pressure on a gas is decreased by one-half, how large will the volume change be?

Problem #13: A gas occupies 4.31 liters at a pressure of 0.755 atm. Determine the volume if the pressure is increased to 1.25 atm.

Problem #14: 600.0 mL of a gas is at a pressure of 8.00 atm. What is the volume of the gas at 2.00 atm?

Problem #15: 400.0 mL of a gas are under a pressure of 800.0 torr. What would the volume of the gas be at a pressure of 1000.0 torr?

Bonus Problem: A particular balloon is designed by its manufacturer to be inflated to a volume of no more than 2.5 liters. If the balloon is filled with 2.0 liters of helium at sea level (101.3 kPa), and rises to an altitude at which the boiling temperature of water is only 88 degrees Celsius, will the balloon burst?

Problems 16-30

Problem #16: 4.00 L of a gas are under a pressure of 6.00 atm. What is the volume of the gas at 2.00 atm?

Problem #17: A gas occupies 25.3 mL at a pressure of 790.5 mmHg. Determine the volume if the pressure is reduced to 0.804 atm.

Problem #18: A sample of gas has a volume of 12.0 L and a pressure of 1.00 atm. If the pressure of gas is increased to 2.00 atm, what is the new volume of the gas?

Problem #19: A container of oxygen has a volume of 30.0 mL and a pressure of 4.00 atm. If the pressure of the oxygen gas is reduced to 2.00 atm and the temperature is kept constant, what is the new volume of the oxygen gas?

Problem #20: A tank of nitrogen has a volume of 14.0 L and a pressure of 760.0 mmHg. Find the volume of the nitrogen when its pressure is changed to 400.0 mmHg while the temperature is held constant.

Problem #21: A 40.0 L tank of ammonia has a pressure of 8.00 atm. Calculate the volume of the ammonia if its pressure is changed to 12.0 atm while its temperature remains constant.

Problem #22: Two hundred liters of helium at 2.00 atm and 28.0 °C is placed into a tank with an internal pressure of 600.0 kPa. Find the volume of the helium after it is compressed into the tank when the temperature of the tank remains 28.0 °C.

Problem #23: You are now wearing scuba gear and swimming under water at a depth of 66.0 ft. You are breathing air at 3.00 atm and your lung volume is 10.0 L. Your scuba gauge indicates that your air supply is low so, to conserve air, you make a terrible and fatal mistake: you hold your breath while you surface. What happens to your lungs? Why?

Problem #24: Solve Boyle's Law equation for V₂.

Problem #25: Boyle's Law deals with what quantities?

(a) pressure/temperature
(b) pressure/volume
(c) volume/temperature
(d) moles/pressure
(e) none of these

Problem #26: A 1.5 liter flask is filled with nitrogen at a pressure of 12 atmospheres. What size flask would be required to hold this gas at a pressure of 2.0 atmospheres?

Problem #27: 300 mL of O₂ are collected at a pressure of 645 mm of mercury. What volume will this gas have at one atmosphere pressure?

Problem #28: How many cubic feet of air at standard conditions (1.00 atm.) are required to inflate a bicycle tire of 0.50 cu. ft. to a pressure of 3.00 atmospheres?

Problem #29: How much will the volume of 75.0 mL of neon change if the pressure is lowered from 50.0 torr to 8.00 torr?

Problem #30: A tank of helium has a volume of 50.0 liters and is under a pressure of 2000.0 p.s.i.. This gas is allowed to flow into a blimp until the pressure in the tank drops to 40.00 p.s.i. and the pressure in the blimp is 30.00 p.s.i.. What will be the volume of the blimp?

Bonus Problem: A spherical weather balloon is constructed so that the gas inside can expand as the balloon ascends to higher altitudes where the pressure is lower. If the radius of the spherical balloon is 2.5 m at sea level where the pressure is 1.004 x 10⁵ Pa, what will be the radius at an altitude of about 10 km where the pressure of the gas is 2.799 x 10⁴ Pa? For simplicity, assume the temperature has not changed.