Q Boyle’s Law Practice Name Abbreviations atm - atmosphere mm Hg - millimeters of mercury torr - another name for mm Hg P1V1 = P2V2 Example 1: 2.00 L of a gas is at 740.0 mmHg pressure. What is its volume at 760 mmHg pressure? Answer: this problem is solved by inserting values into P1V1 = P2V2. (740.0 mmHg) (2.00 L) =(760.0 mmHg) (x) Example #1: 2.00 L of a gas is at 740.0 mmHg pressure. What is its volume at standard pressure? Answer: this problem is solved by inserting values into P1V1 = P2V2. (740.0 mmHg) (2.00 L) =(760.0 mmHg) (x) Problems: 1. A gas occupies 12.3 liters at a pressure of 40.0 mm Hg. What is the volume when the pressure is increased to 60.0 mm Hg? 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? 3. 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? 4. A gas occupies 11.2 liters at 0.860 atm. What is the pressure if the volume becomes 15.0 L? 5. 500.0 mL of a gas is collected at 745.0 mm Hg. What will the volume be at standard pressure? 6. Convert 350.0 mL at 740.0 mm of Hg to its new volume at standard pressure. 7. Convert 338 L at 63.0 atm to its new volume at standard pressure. Name: ____________________ Date: _______________ Period: ________ B oyles’ Law Directions: Solve the following problems showing ALL work. You MUST identify what variable that each number goes with. 1) 1.00 L of a gas at standard temperature and pressure is compressed to 473 mL. What is the new pressure of the gas? 2) In a thermonuclear device, the pressure of 0.050 liters of gas within the bomb casing reaches 4.0 x 106 atm. When the bomb casing is destroyed by the explosion, the gas is released into the atmosphere where it reaches a pressure of 1.00 atm. What is the volume of the gas after the explosion? 3) Synthetic diamonds can be manufactured at pressures of 6.00 x 104 atm. If we took 2.00 liters of gas at 1.00 atm and compressed it to a pressure of 6.00 x 104 atm, what would the volume of that gas be? 4) The highest pressure ever produced in a laboratory setting was about 2.0 x 106 atm. If we have a 1.0 x 10- 5 liter sample of a gas at that pressure, then release the pressure until it is equal to 0.275 atm, what would the new volume of that gas be? 5) Atmospheric pressure on the peak of Mt. Everest can be as low as 150 mm Hg, which is why climbers need to bring oxygen tanks for the last part of the climb. If the climbers carry 10.0 liter tanks with an internal gas pressure of 3.04 x 104 mm Hg, what will be the volume of the gas when it is released from the tanks? 6) Part of the reason that conventional explosives cause so much damage is that their detonation produces a strong shock wave that can knock things down. While using explosives to knock down a building, the shock wave can be so strong that 12 liters of gas will reach a pressure of 3.8 x 104 mm Hg. When the shock wave passes and the gas returns to a pressure of 760 mm Hg, what will the volume of that gas be? 7) Submarines need to be extremely strong to withstand the extremely high pressure of water pushing down on them. An experimental research submarine with a volume of 15,000 liters has an internal pressure of 1.2 atm. If the pressure of the ocean breaks the submarine forming a bubble with a pressure of 250 atm pushing on it, how big will that bubble be? 8) Divers get “the bends” if they come up too fast because gas in their blood expands, forming bubbles in their blood. If a diver has 0.050 L of gas in his blood under a pressure of 250 atm, then rises instantaneously to a depth where his blood has a pressure of 50.0 atm, what will the volume of gas in his blood be? Boyle’s Law Answers (depending on unit of pressure used for STP problem #1 may have a different answer) 1) 2.11 atm 2) 200,000L 3) 0.0000333L 4) 72.72 L 5) 2026.7 L 6) 600 L 7) 72 L 8) 0.25 L Name: ____________________ Date: _______________ Period: ________ Charles’ Law Worksheet Directions: Solve the following problems showing ALL work. You MUST identify what variable that each number goes with. 1) The temperature inside my refrigerator is about 4.00 Celsius. If I place a balloon in my fridge that initially has a temperature of 220 C and a volume of 0.50 liters, what will be the volume of the balloon when it is fully cooled by my refrigerator? 2) A man heats a balloon in the oven. If the balloon initially has a volume of 0.40 liters and a temperature of 20. 0C, what will the volume of the balloon be after he heats it to a temperature of 250 0C? 3) On hot days, you may have noticed that potato chip bags seem to “inflate”, even though they have not been opened. If I have a 250 mL bag at a temperature of 19 0C, and I leave it in my car which has a temperature of 60.00 C, what will the new volume of the bag be? 4) A soda bottle is flexible enough that the volume of the bottle can change even without opening it. If you have an empty soda bottle (volume of 2.0 L) at room temperature (25 0C), what will the new volume be if you put it in your freezer (-4.0 0C)? 5) Some students believe that teachers are full of hot air. If I inhale 2.2 liters of gas at a temperature of 180 C and it heats to a temperature of 380 C in my lungs, what is the new volume of the gas? 6) How hot will a 2.3 L balloon have to get to expand to a volume of 400. L? Assume that the initial temperature of the balloon is 25 0C. 7) I have made a thermometer which measures temperature by the compressing and expanding of gas in a piston. I have measured that at 100.0 0 C the volume of the piston is 20.0 L. What is the temperature outside if the piston has a volume of 15 L? What would be appropriate clothing for the weather? Name: Date: Period: Combined Gas Law Problems: 1. A gas balloon has a volume of 106.0 liters when the temperature is 45.0 °C and the pressure is 740.0 mm of mercury. What will its volume be at 20.0 °C and 780 .0 mm of mercury pressure? 2. If 10.0 liters of oxygen at STP are heated to 512 °C, what will be the new volume of gas if the pressure is also increased to 1520.0 mm of mercury? 3. A gas is heated from 263.0 K to 298.0 K and the volume is increased from 24.0 liters to 35.0 liters by moving a large piston within a cylinder. If the original pressure was 1.00 atm, what would the final pressure be? 4. The pressure of a gas is reduced from 1200.0 mm Hg to 850.0 mm Hg as the volume of its container is increased by moving a piston from 85.0 mL to 350.0 mL. What would the final temperature be if the original temperature was 90.0 °C? Gas Laws Packet #2 Ideal Gas Law Worksheet PV = nRT Use the ideal gas law, “PV-nRT”, and the universal gas constant R = 0.0821 L*atm to solve the following problems: K*mol If pressure is needed in kPa then convert by multiplying by 101.3kPa / 1atm to get R =8.31 L*kPa / (K*mole) 1) If I have 4 moles of a gas at a pressure of 5.6 atm and a volume of 12 liters, what is the temperature? 2) If I have an unknown quantity of gas at a pressure of 1.2 atm, a volume of 31 liters, and a temperature of 87 0C, how many moles of gas do I have? 3) If I contain 3 moles of gas in a container with a volume of 60 liters and at a temperature of 400 K, what is the pressure inside the container? 4) If I have 7.7 moles of gas at a pressure of 0.09 atm and at a temperature of 56 0C, what is the volume of the container that the gas is in? 5) If I have 17 moles of gas at a temperature of 67 0C, and a volume of 88.89 liters, what is the pressure of the gas? 6) If I have an unknown quantity of gas at a pressure of 0.5 atm, a volume of 25 liters, and a temperature of 300 K, how many moles of gas do I have? 7) If I have 21 moles of gas held at a pressure of 78 atm and a temperature of 900 K, what is the volume of the gas? 8) If I have 1.9 moles of gas held at a pressure of 5 atm and in a container with a volume of 50 liters, what is the temperature of the gas? 9) If I have 2.4 moles of gas held at a temperature of 97 0C and in a container with a volume of 45 liters, what is the pressure of the gas? 10) If I have an unknown quantity of gas held at a temperature of 1195 K in a container with a volume of 25 liters and a pressure of 560 atm, how many moles of gas do I have? 11) If I have 0.275 moles of gas at a temperature of 75 K and a pressure of 1.75 atmospheres, what is the volume of the gas? 12) If I have 72 liters of gas held at a pressure of 3.4 atm and a temperature of 225 K, how many moles of gas do I have?

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