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Chemistry: Dalton’s Law of Partial Pressure Directions: Solve each of the following problems. Show your work, including proper units, to earn full credit. 1. Container A (with volume 1.23 dm3) contains a gas under 3.24 atm of pressure. Container B (with volume 0.93 dm3) contains a gas under 2.82 atm of
Dalton ’s Law of Partial Pressures Worksheet Name_____ 1. Blast furnaces give off many unpleasant and unhealthy gases. If the total air pressure is 0.99 atm, the partial pressure of carbon dioxide is 0.05 atm, and the partial pressure of hydrogen sulfide is 0.02 atm, what is the partial pressure of the remaining air? 2.
What is the partial pressure of each gas? Solution: 1) Calculate moles of each gas: He: 40.0 g / 4.0026 g/mol = 9.9935 mol O 2: 40.0 g / 31.9988 g/mol = 1.25005 mol. 2) Calculate mole fraction: He: 9.9935 mol / 11.24355 mol = 0.88882. 3) Calculate partial pressure:
Worksheet 19 Dalton’s Law of Partial Pressures – Part 2. mixture of 4.5% H2, 76% O2, and 19.5% N2 has a total pressure of 2.3 atm. What is the partial pressure of each of the gases? A 2.5 L sample at 273 K contains 0.006 mol H2, 0.0024 mol O2, and 0.0002 mol CH4. What is the partial pressure of O2?
Dalton’s Law says that the sum of the individual pressures of all the gases that make up a mixture is equal to the total pressure, or PT = P1 + P2 + P3 + .... The partial pressure of each gas is equal to the mole fraction of each gas times the total pressure.
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Dalton’s Law of Partial Pressure. 1. A metal tank contains three gases: oxygen, helium, and nitrogen. If the partial pressures of the three gases in the tank are 35 atm of O2, 5 atm of N2, and 25 atm of He, what is the total pressure inside of the tank? 2. Blast furnaces give off many unpleasant and unhealthy gases.
