Under ideal conditions, the rates at which different gases diffuse (spread out) are proportional to their molar masses.
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1 Chemistry Ms. Ye Name Date Block Graham s Law of Diffusion- Under ideal conditions, the rates at which different gases diffuse (spread out) are proportional to their molar masses. In other words, gas molecules will move than smaller gas molecules. 1. Compare the rates of diffusion of H 2 and O 2 gases at the same temperature and pressure. 2. Rank the following gases from slowest to fastest rate of diffusion: H 2, CO 2, Ne, H 2 S. 3. Compare the rates of effusion of nitrogen (N 2 ) and helium at the same temperature and pressure. 4. Compare the rate of effusion of carbon dioxide (CO 2 ) with hydrochloric acid (HCl) at the same temperature and pressure. 1
2 Dalton s Law- P total = 1. Two gases such as oxygen and nitrogen are present in a flask at the following pressures. When combined, what is the pressure of the flask? P Nitrogen =250. mm Hg P Oxygen =300. mm Hg List all variables 2. Neon gas has a pressure of 1.49atm in its container. When added to a container holding helium gas the total pressure is 2.34atm. What is the pressure of the helium gas? List all variables 2
3 Dalton s Law Continued: Water displacement of gas: P atm = Gases given off from the rxn travel through the tube and into the adjacent container for collection Gas is impure and contains some water vapor 1. Oxygen gas from the decomposition of potassium chlorate was collected by water displacement. The barometric pressure and the temperature during the experiment were 731.0torr and 20.0 C respectively. What was the partial pressure of the oxygen collected? The vapor pressure of water at 20 C is 17.5 torr 2. Some hydrogen gas was collected over water at 20.0 C. The partial pressure of hydrogen is torr. What is the barometric pressure of the gas? The vapor pressure of water at 20 C is 17.5 torr 3
4 Dalton and Graham s Law Practice: 1. A mixture of H 2, NH 3, CO 2 and N 2 has a total pressure of 800. Torr. The partial pressures of 3 gases are given. What is the partial pressure of N 2? PH 2 =114 torr PNH 3 =171 torr PCO 2 =229 torr 2. A 250. ml sample of oxygen is collected over water at 25 C and torr pressure. What is the pressure of the dry gas alone? (vapor pressure of water at 25 C=23.8 torr) 3. A 54.0 ml sample of oxygen is collected over water at 23 C and torr pressure. What is the volume of the dry gas at STP (Vapor pressure of water at 23 C=21.1 torr) 4. What is the relative rate of diffusion of NH 3 compared to He (does it diffuse faster or slower)? 5. An unknown gas diffuses 0.25 times as fast as He. Is the molar mass of the unknown gas greater and less than that of He? 4
5 Boyle s Law- 1. A sample of O 2 has a volume of 150. ml at a pressure of 0.947atm. What will the volume of the gas be at a pressure of 0.987atm if temperature stays constant? 2. A gas has a pressure of 726 mmhg and occupies a volume of 7.40L. If the gas is compressed to a volume of 2.93L, what will the pressure be? 5
6 Charles s Law- 1. A sample of neon gas occupies a volume of 752mL at 25 C. What volume will the gas occupy at 50. C if the pressure remains constant? 2. A helium filled balloon has a volume of 2.75L at 20.0 C. The volume of the balloon decreases to 2.46L after it is placed outside on a cold day. What is the outside temperature in K? In C? 6
7 Gay-Lussac s Law- 1. The gas in an aerosol can is at a pressure of 3.00 atm at 25 C. Directions on the can warn users not to keep the can in a place where the temperature exceeds 52 C. What would the gas pressure be at this temperature? 2. Before leaving for a road trip, the pressure of your car tire is 1020 torr at 20 C. At the end of the trip the pressure gauge reads 1110 torr. What is the new temperature inside the tire? 7
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