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Name: _______________________Date: _________ Period: ______Gas Laws Worksheet Part 1Boyle’s LawCharles’s LawGuy-Lassac’s LawCombined Gas LawFor a given mass of gas at constant temperature, the volume of a gasvaries inversely withpressureThe volume of a fixedmass of gas is directlyproportional to itsKelvin temperature ifthe pressure is keptconstant.The pressure of a gas isdirectly proportional tothe Kelvin temperature ifthe volume is bines Boyle’s,Charles’, and theTemperature-Pressurerelationship into oneequation. Each of theselaws can be derived fromthis law.P1×V1=P2×V2V1T1=V2T2OrV1×T2=V2×T1P1T1=P2T2OrP1×T2=P2×T1P1×V1T1=P2×V2T2OrP1×V1×T2=P2×V2×T1Ideal Gas LawDalton’s LawGraham’s LawThe Ideal Gas Law relates thepressure, temperature, volume,and mass of a gas through thegas constant “R”.At constant volume andtemperature, the total pressureexerted by a mixture of gases isequal to the sum of the pressuresexerted by each gas,The rate of effusion/diffusion oftwo gases (A and B) are inverselyproportional to the square rootsof their formula masses. P×V=n×R×TOrPV=nRTPtotal=P1+P2+P3+ . . . . RateARateB=molar massAmolar massBAbbreviationStandard conditionsatm = atmospheremm Hg = millimeters of mercurytorr = another name for mm HgPa = Pascal kPa = kilopascalK = Kelvin°C = degrees Celsius0°C = 273 K1.00 atm = 760.0 mm Hg = 76 cm Hg =101.3 kPa = 101, 300 Pa = 29.9 in HgConversionsGas Law’s Equation SymbolsK = °C + 273°F ??1.8°C ??32°C =°F -321.81 cm3 (cubic centimeter) = 1 mL (milliliter)1 dm3 (cubic decimeter) = 1 L (liter) = 1000 mLSubscript (1) = old condition or initial conditionSubscript (2) = new condition or final conditionTemperature must be in Kelvinsn = number of moles = grams/Molar massR = 8.31 L·kPaK·mol or 0.0821 L·atmK·mol You must have a common set of units in theproblem1. Convert the following temperatures to K.a) 104 Cb) -3 C2. Convert the following temperatures to C.a) 67 Kb) 1671 K3. A sample of nitrogen gas has a volume of 478 L and a pressure of 104.1 kPa. What volume would the gas occupy at 88.2 kPa if the temperature remains constant?4. 8.98 mL of hydrogen gas is collected at 38.8 °C. Find the volume the gas will occupy at -39.9 °C if the pressure remains constant.5. A sample of gas has a volume of 215 L at 23.5 °C and 84.6 kPa. What volume will the gas occupy at STP (standard temperature and pressure)?6. A 495 mL of oxygen gas at 25.0 °C and 114.7 kPa, is put in a 536 mL flask. Find the total pressure in the flask, assumingthe temperature remains constant.7. A sample of gas is transferred from a 75 mL vessel to a 500.0 mL vessel. If the initial pressure of the gas is 145 atm and if the temperature is held constant, what is the pressure of the gas sample in the 500.0 mL vessel?8. A sample of gas occupies a volume of 450.0 mL at 740 mm Hg and 16°C. Determine the volume of this sample at760 mm Hg and 37°C.9. Convert a pressure of 0.0248 mm Hg to the equivalent pressure in kPa.10. Air in a closed cylinder is heated from 25°C to 36°C. If the initial pressure is 3.80 atm, what is the final pressure?11. A bubble of helium gas has a volume of 0.650 mL near the bottom of a large aquarium where the pressure is 1.54 atm and the temperature is 12°C. Determine the bubble’s volume upon rising near the top where the pressure is 760 torr and 16°C.12. What is the pressure in mm of Hg , of a gas mixture that contains 1g of H2, and 8.0 g of Ar in a 3.0 L container at 27°C.Name: _______________________Date: _________ Period: ______Gas Laws Worksheet Part 213. To what temperature must32.0 ft3 of a gas at 2°C be heated for it to occupy 100.0 ft3 at the samepressure? {HINT: ft3 is a unit of volume)14. A bag of potato chips is packaged at sea level (1.00 atm) and has a volume of 315 mL. If this bag of chips is transported to Denver (0.775 atm), what will the new volume of the bag be?15. A Los Angeles class nuclear submarine has an internal volume of eleven million liters at a pressure of 1.250 atm. If a crewman were to open one of the hatches to the outside ocean while it was underwater (pressure = 15.75 atm), what be would the new volume of the air inside the submarine?16. A child has a toy balloon with a volume of 1.80 liters. The temperature of the balloon when it was filled was 200 C and the pressure was 1.00 atm. If the child were to let go of the balloon and it rose 3 kilometers into the sky where the pressure is 0.667 atm and the temperature is -100 C, what would the new volume of the balloon be?17. A commercial airliner has an internal pressure of 1.00 atm and temperature of 250 C at takeoff. If the temperature of the airliner drops to 170 C during the flight, what is the new cabin pressure?18. If divers rise too quickly from a deep dive, they get a condition called “the bends” which is caused by the expansion of very small nitrogen bubbles in the blood due to decreased pressure. If the initial volume of the bubbles in a diver’s blood is 15 mL and the initial pressure is 12.75 atm, what is the volume of the bubbles when the diver has surfaced to 1.00 atm pressure?19. The temperature inside my refrigerator is about 40 Celsius. If I place a balloon in my fridge that initially has a temperature of 220 C and a volume of 0.5 liters, what will be the volume of the balloon when it is fully cooled by my refrigerator?20. 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 600 C, what will the new volume of the bag be?21. 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 L) at room temperature (25 0C), what will the new volume be if you put it in your freezer (-4 0C)?22. I have made a thermometer which measures temperature by the compressing and expanding of gas in a piston. I have measured that at 1000 C the volume of the piston is 20 L. What is the temperature outside if the piston has a volume of 15 L? What would be appropriate clothing for the weather?23. 1.00 L of a gas at standard temperature and pressure is compressed to 473 mL. What is the new pressure of the gas?24. 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?25. 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?26. 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?27. 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?Ideal gas law problems28. At what temperature Celsius will 19.4 g of molecular oxygen, O2, exert a pressure of 1820 mm Hg in a 5.12 L cylinder?29. A sample of nitrogen gas,N2, is collected in a100 mL container at a pressure of 688 mm Hg and a temperature of 565 °C. How many grams of nitrogen gas are present in this sample?30. What is the pressure in atm exerted by 2.48 moles of a gas in a 250.0 mL container at 58°C? ................
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