Chemistry, 18.07.2019 16:00, elitehairnerd1964

During an effusion experiment, a certain number of moles of an unknown gas passed through a tiny hole in 50 seconds. under the same conditions, the same number of moles of oxygen gas passed through the hole in 35 seconds. what is the molar mass of the unknown gas?

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Chemistry, 01.07.2019 08:30, mikisims

In an effusion experiment it required 40 s for a certain number of moles of a gas of unknown molar mass to pass through a small orifice into a vacuum. under the same conditions 16 s were required for the same number of moles of o2 to effuse. what is the molar mass of the unknown gas?

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Chemistry, 31.07.2019 03:00, avaverretkj

During an effusion experiment, oxygen gas passed through a tiny hole 2.5 times faster than the same number of moles of another gas under the same conditions. what is the molar mass of the unknown gas? (note: the molar mass of oxygen gas is 32.0 g/mol.) 2.0 × 102 g

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Chemistry, 01.11.2019 02:31, doritasanchez

In the first part of your analysis, you completed an effusion experiment to gain some more information about the unknown gas. in the effusion experiment, 25.0 ml of the unknown gas required 27.3 seconds to effuse from your apparatus. under the same conditions, 30.0 ml of nitrogen effused in 42.0 seconds. a. name the law that you used

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Chemistry, 15.11.2019 01:31, shrinu

Gas effusion 1. it takes 354 seconds for 1.00 ml of xe to effuse through a small hole. under the same conditions, how long will it take for 1.00 ml of nitrogen to effuse? 2.what is the rate of effusion for a gas that has a molar mass twice that of a gas that effuses at a rate of 4.2 mol/min? 3. it takes 110. seconds for a sample of carbon dioxide to effuse through a porous plug and 275 seconds for the same volume of an unknown gas to effuse under the same conditions. what is the molar mass of the unknown gas (in g/mol)? 4. if a gas effuses 4.25 times faster than iodine gas (i2), what is its molar mass? 5. calculate the density of a gas at stp, if a given volume of the gas effuses through an apparatus in 6.60 min and the same volume of nitrogen, at the same temperature and pressure, effuses through this apparatus in 8.50 minutes. ideal vs non-ideal gases an ideal gas is one in which the molecules don't interact with each other and don't take up any space. in an ideal world, collisions between gas molecules are completely elastic. all gases in the real world have molecules with diameters and which interact with each other, so there's always a bit of error involved in using any form of the ideal gas law and van der waal's equation. however, noble gases act much like ideal gases because they don't participate in chemical reactions with other gases. helium, in particular, acts like an ideal gas because each atom is so tiny. other gases behave much like ideal gases when they are at low pressures and temperatures low pressure means few interactions between gas molecules occur . low temperature means the gas molecules have less kinetic energy, so they don't move around as much to interact with each other or their container. a 4.25-l flask contains 3.46 mol co2 : (a) from the ideal gas law (b) from the van der waals equation (c) explain the reason(s) for the difference 229 °c. calculate the pressure of this sample of co2

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