GRAHAMS LAW OF EFFUSION 1|A mixture of 0.50 mole H₂ and 0.50 mole of SO₂ is introduced into a 10.0 L container at 25^oC. The container has pinhole leak. After a period of time:
(Atomic weights: H = 1.008, S = 32.06, O = 16.00).||1|the partial pressure of SO₂ exceeds that of H₂ in the remaining gas|the partial pressure of H₂ exceeds that of SO₂ in the remaining gas|the partial pressures of the two gases remain equal throughout this time 2|A mixture of 0.50 mole N₂ and 0.50 mole of CO₂ is introduced into a 10.0 L container at 25^oC. The container has pinhole leak. After a period of time:
(Atomic weights: N = 14.01, C = 12.01, O = 16.00).||1|the partial pressure of CO₂ exceeds that of N₂ in the remaining gas|the partial pressure of N₂ exceeds that of CO₂ in the remaining gas|the partial pressures of the two gases remain equal throughout this time 3|Which gases, N₂O, C₂H₂, NO, diffuse more slowly than O₂ under identical experimental conditions?
(Atomic weights: N = 14.01, O = 16.00, C = 12.01, H = 1.008).||1|N₂O only|C₂H₂ only |NO only|NO and C₂H₂|N₂O and C₂H₂ 4|Which gases, Ne, Cl₂, H₂S diffuse more slowly than O₂ under identical expermimental conditions?
(Atomic weights: Ne = 20.2, Cl = 35.45, O = 16.00, H = 1.008).||1|Cl₂ and H₂S|Cl₂ only|Ne, Cl₂ and H₂S|H₂S only|Ne only 5|Heavy water, D₂O (mol. wt. = 20.03) can be separated from ordinary water by the difference in the relative rates of diffusion of the molecules in the gas phase. Calculate the relative rate of diffusion of H₂O to D₂O.
(Atomic weights: O = 16.00, H = 1.00).||1|1.05|1.11|0.898|0.972|0.947 6|Calculate the relative rate of diffusion of HF compared to HCl.
(Atomic weights: H = 1.008, Cl = 35.45, F = 19.00).||1|1.35|0.741|1.82|1.21|0.549 7|Calculate the relative rate of diffusion of O₂ compared to O₃.
(Atomic weight: O = 16.00).||1|1.22|0.672|1.49|1.30|0.820 8|Calculate the relative rate of diffusion of CO₂ compared to SO₂.
(Atomic weights: C = 12.00, O = 16.00, S = 32.06).||1|1.21|1.46|0.424|0.826|0.685 9|An unknown gas diffuses at the rate of 83.3 mL/s in a diffusion apparatus in which a second gas whose molecular weight is 44.0, diffuses at a rate of 102 mL/s. Calculate the molecular weight of the first gas.||1|66.0|29.3|49.2|53.9|71.5 10|Under standard conditions, the density of He is 0.179 g/L and of Xe is 5.86 g/L. In an apparatus, helium effuses at the rate of 15 mL/min. At what rate will xenon effuse in the same apparatus?||1|2.6|6.2|33.8|1.9|1.2 11|In an effusion apparatus, H₂ is found to effuse at the rate of 5.9 mL/s. Another gas in the same apparatus effuses at the rate of 0.55 mL/s. What is the molecular weight of the gas?
(Atomic weight: H = 1.008).||1|230|21|52|132|430 12|In an effusion apparatus, HCl was found to travel 43.3 cm in one minute. How far will NH₃ travel in one minute in the same apparatus?
(Atomic weights: H = 1.008, N = 14.01, Cl = 35.45).||1|63.4|52.4|42.8|35.8|29.5 13|Two identical balloons are filled, one with helium and one with nitrogen at the same temperature. If the nitrogen balloon leaks at the rate of 75 mL per hour, what will be the rate of leakage from the helium balloon?
(Atomic weights: He = 4.00, N = 14.01).||1|198 mL/hr|28 mL/hr|75 mL/hr|122 mL/hr|14 mL/hr 14|It takes 145 s for 1.0 mL of nitrogen to effuse from a porous container. It takes 230 s for 1.0 mL of an unknown gas to effuse under the same conditions from the porous container. What is the molecular weight of the gas?
(Atomic weight: N = 14.01).||1|70|86|44|36|32 15|Two identical porous containers are filled, one with hydrogen and the other with carbon dioxide. If under the same conditions, 1.50 mL of carbon dioxide leaks from the container in one day, how much hydrogen will leak out?
(Atomic weights: H = 1.008, C = 12.01, O = 16.00).||1|7.04 mL|3.40 mL|2.12 mL|33 mL|26 mL 16|A sample of N₂ gas is contaminated with a gas (A) of unknown molecular weight. The partial pressure of each gas is known to be 200 torr at 25^oC. The gases are allowed to effuse through a pinhole, and it is found that gas A escapes at three times the rate of N₂. What is the molecular weight of gas A?
(Atomic weight: N = 14.01).||1|3.11|252|84.0|9.33|28.0 17|A sample of N₂ gas is contaminated with a gas (A) of unknown molecular weight. The partial pressure of each gas is known to be 200 torr at 25^oC. The gases are allowed to effuse through a pinhole, and it is found that gas A escapes at a rate one third that of N₂. What is the molecular weight of gas A?
(Atomic weight: N = 14.01).||1|252|84.0|9.33|28.0|3.11 18|A gas mixture designed to be breathed by deep sea divers is 5.0% O₂, 10.0% N₂ and 85.0% He by volume. The air is breathed underwater at 100 feet where the total pressure is 4.1 atm. What is the partial pressure (atm) of oxygen under these conditions?||1|0.21|0.05|0.86|0.38|0.52 19|Expired air is 74.5% N₂, 15.7% O₂, 3.6% CO₂ and 6.2% H₂O by volume. What is the partial pressure (mm Hg) of the oxygen at 37^oC and 745 mm Hg?||1|117|121|112|127|105