Gas Law Worksheets - WS: Boyle s and Charles Law Boyle s Law states that the volume of a gas varies inversely with its pressure if temperature is held constant. (If one goes up the, other goes down.) We use the formula: P x V = P x V Solve the following problems (assuming constant temperature).. A sample of oxygen gas occupies a volume of 50.mL at 740. torr pressure. What volume will it occupy at 800. torr pressure?. A sample of carbon dioxide occupies a volume of 3.50 liters at 5 kpa pressure. What pressure would the gas exert if the volume was decreased to.00 liters? 3. A.0 liter container of nitrogen had a pressure of 3. atm. What volume would be necessary to decrease the pressure to.0 atm. 4. Ammonia gas occupies a volume of 450. ml at a pressure of 70. mm Hg. What volume will it occupy at standard pressure? 5. A 75 ml sample of neon had its pressure changed from 75 kpa to 50 kpa. What is its new volume? 6. A sample of hydrogen at.5 atm had its pressure decreased to 0.50 atm producing a new volume of 750 ml. What was its original volume? 7. Chlorine gas occupies a volume of. liters at 70 torr pressure. What volume will it occupy at atm pressure? 8. Fluorine gas exerts a pressure of 900. torr. When the pressure is changed to.50 atm, its volume is 50. ml. What was the original volume?
WS Boyle s & Charles Law continued Charles Law states that the volume of a gas varies directly with the Kelvin temperature, assuming that the pressure is constant. We use the following formulas: V V or V x K C 73 V x Solve the following problems assuming a constant pressure. 9. A sample of nitrogen occupies a volume of 50 ml at 5 C. What volume will it occupy at 95 C? 0. Oxygen gas is at a temperature of 40 C when it occupies a volume of.3 liters. o what temperature should it be raised to occupy a volume of 6.5 liters?. Hydrogen gas was cooled from 50. C to 50. C. Its new volume is 75 ml. What was the original volume?. Chlorine gas occupies a volume of 5 ml a 300. K. What volume will it occupy at 600 K? 3. A sample of neon gas at 50. C and a volume of.5 liters is cooled to 5 C. What is the new volume? 4. Fluorine gas at 300. K occupies a volume of 500. ml. o what temperature should it be lowered to bring the volume to 300. ml? 5. Helium occupies a volume of 3.8 liters at -45 C. What volume will it occupy at 45 C? 6. A sample or argon gas is cooled and its volume went from 380. ml to 50. ml. If its final temperature was -55 C, what was its original temperature?
WS # - COMBINED GAS LAW In practical terms, it is often difficult to hold any of the variables constant. When there is a change in pressure, volume and temperature, the combined gas law is used. P x V P x V or P V P V Complete the following chart. P V P V 3 4 5 6 7 8.5 atm 3.0 L 0. C.5 atm 30. C 70 torr 56 ml 5 C 50 ml 50. C 600. mmhg.5 L C 760 mmhg.8 L 750 ml 0.0 C.0 atm 500. ml 5 C 95 kpa 4.0 L 0 kpa 6.0 L 98 C 650. torr 00. C 900. torr 5 ml 50. C 850 mmhg.5 L 5 C.5 L 30. C 5 ml 5 ml 00. kpa 00. ml 75 C Show your work here for at least the first example:
WS #3 - DALON S LAW OF PARIAL PRESSURES Dalton s Law says that the sum of the individual pressures of all gases that make up a mixture is equal to the total pressure or: P = P + P + P3 + he particle pressure of each gas is equal to the mole fraction of each gas total pressure. P P P P...or 3 moles gas x x P total moles Px Solve the following problems.. A 50 ml sample of oxygen is collected over water at 5 C and 760.0 torr pressure. What is the pressure of the dry gas alone? (Vapor pressure of water at 5 C = 3.8 torr). A 3.0 ml sample of hydrogen is collected over water at 0. C and 750.0 torr pressure. What is the volume of the dry gas at SP? (Vapor pressure of water at 0. C = 7.5 torr) 3. A 54.0 ml sample of oxygen is collected over water at 3 C and 770.0 torr pressure. What is the volume of the dry gas at SP? (Vapor pressure of water at 3 C =. torr) 4. A mixture of.00 moles of H, 3.00 moles of NH3, 4.00 moles of CO and 5.00 moles of N exerts a total pressure of 800. torr. What is the partial pressure of each gas? 5. he partial pressure of F in a mixture of gases where the total pressure is.00 atm is 300. torr. What is the mole fraction of F?
WS #4 - Graham s Law of Diffusion/Effusion Graham s Law says that gas will effuse at a rate that is inversely proportional to the square root of its molecular mass,. Express mathematically: rate rate Solve the following problems.. Under the same conditions of temperature and pressure, how many times faster will hydrogen effuse compared to carbon dioxide?. If the carbon dioxide in Problem takes 3 sec to effuse, how long will the hydrogen take? 3. What is the relative rate of diffusion of NH3 compared to He? Does NH3 effuse faster or slower than He? 4. If the He in Problem 3 takes 0 sec to effuse, how long will the NH3 take? 5. An unknown gas diffuses 0.5 times as fast as He. What is the molecular mass of the unknown gas?
Chapter 4 Study Guide Gases (CP) (page of ) Objectives:. Use Boyle s Law, Charles Law, Avogadro s Law, and the combined gas law, as appropriate, to calculate changes in pressure, volume, temperature, and amount of gas.. Use the ideal gas law equation to do calculations about a sample of gas. 3. Do calculations involving gas densities and the standard molar volume. 4. Use the law of partial pressure to calculate the pressure exerted by gases in a mixture (including gases collected over a liquid; factor in vapor pressure of the liquid) 5. Describe the kinetic-molecular theory of gases, and how this theory is consistent with the observed gas laws. Equations: Combined gas law: Ideal gas law: PV / = PV / PV = nr, where R = 0.08 L atm / mol K Partial pressure: Ptotal = P + P + P3 + Pgas = Patm PHO Graham s Law of Effusion: rate rate = Problems:. A 50.0 ml volume of gas is collected at 30.0 C. What volume would the sample of gas occupy at 0.0 C, assuming constant pressure? (Charles Law) (4 ml). A 3.00 L pocket of air at sea level has a pressure of.00 atm. Suppose the air pocket rises in the atmosphere to a certain height and expands to a volume of 0.0 L. What is the pressure of the air at the new volume? (assume constant temperature, Boyle s Law) (0.300 atm) 3. A weather balloon has a volume of 750. L at.0 atm. he balloon is released into the atmosphere. At the highest point above the ground, the pressure on the balloon is 0.350 atm. What is the new volume of the balloon at this height? (assume constant temp. Boyle s Law) (5.50x0 3 L) 4. A gas with a pressure of 875 mm Hg at 305 C occupies.50 L. What volume will the gas occupy at SP? (Combined Gas Law) (.36 L) 5. A 3.0 ml sample of hydrogen gas is collected at 0oC and 750 torr. What would the temperature of the gas be if the volume is increased to 40. ml with a pressure of 740 torr? (Combined Gas Law) (363 ml) Continue onto next page
Review Guide continued (Page of ) 6. A 54.76 g sample of carbon dioxide gas is sealed in a 7.55 L container and heated to a temperature of 354 C. What is the pressure of the gas? (Ideal Gas Law) (8.49 atm) 7. Calculate the mass of oxygen gas, O, measured at 765 mm Hg and 35.5 C in 4.35 L. (Ideal Gas Law) (0.398mol.8 go) 8. How many grams of helium, He, will be required to fill balloons at SP, assuming that each balloon has a volume of 455 ml? (Ideal Gas Law or molar volume) (step: How many liters of helium total is used? 5.46L; step, How many moles of He is this? 0.436 mol; step 3: How many grams of He is this? 0.974 g) 9. A 300.0 ml sample of hydrogen was collected over water.0 C on a day when the atmospheric pressure was 748 mm Hg. (water vapor pressure at that temperature is 8.65 mm Hg) a) What is the partial pressure of the hydrogen gas? (Partial Pressure) (79mmHg) b) How many moles of H were present? (Ideal Gas Law) (0.09mol H) c) What would be the mass of the hydrogen sample if it were dry? (mole map) (0.039gH) 0. How much faster does chlorine gas diffuse compared to xenon? (remember, chlorine is diatomic! Graham s Law) (.36)