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Learning Goal: In a given sample of gas, the particles move at varying speeds. The root mean square speed (rms speed) of particles in a gas sample, u, is given by the formula 3RT u = √ where T is the Kelvin temperature, M is the molar mass in kg/mol, and R= 8.314 J/(mol. K) is the gas constant. Effusion is the escape of gas molecules through a tiny hole into a vacuum. The rate of effusion of a gas is directly related to the rms speed of the gas molecules, so it's inversely proportional to the square root of its mass. The rms speed is related to kinetic energy, rather than average speed, and is the speed of a molecule possessing a kinetic energy identical to the average kinetic energy of the sample. Given its relationship to the mass of the molecule, you can conclude that the lighter the molecules of the gas, the more rapidly it effuses. Mathematically, this can be expressed as Fm The relative rate of effusion can be expressed in terms of molecular masses mA and mB as effusion rate x rate of gas A effusion mB rate of gas B effusion V MA Part A Calculate the rms speed of an oxygen gas molecule, O2, at 23.0 °C. Express your answer numerically in meters per second. ▸ View Available Hint(s) Submit ▾ Part B Rank the following gases in order of decreasing rate of effusion. Rank from the highest to lowest effusion rate. To rank items as equivalent, overlap them. ▸ View Available Hint(s) Submit - Part C Highest rate of effusion G: ? m/s He PH3 Ar H₂ C4H10 rate of NH3 effusion rate of CO effusion Reset Help Lowest rate of effusion How much faster do ammonia (NH3) molecules effuse than carbon monoxide (CO) molecules? Enter the ratio of the rates of effusion. Express your answer numerically using three significant f ▸ View Available Hint(s) ⒸEB

Learning Goal: In a given sample of gas, the particles move at varying speeds. The root mean square speed (rms speed) of particles in a gas sample, u, is given by the formula 3RT u = √ where T is the Kelvin temperature, M is the molar mass in kg/mol, and R= 8.314 J/(mol. K) is the gas constant. Effusion is the escape of gas molecules through a tiny hole into a vacuum. The rate of effusion of a gas is directly related to the rms speed of the gas molecules, so it's inversely proportional to the square root of its mass. The rms speed is related to kinetic energy, rather than average speed, and is the speed of a molecule possessing a kinetic energy identical to the average kinetic energy of the sample. Given its relationship to the mass of the molecule, you can conclude that the lighter the molecules of the gas, the more rapidly it effuses. Mathematically, this can be expressed as Fm The relative rate of effusion can be expressed in terms of molecular masses mA and mB as effusion rate x rate of gas A effusion mB rate of gas B effusion V MA Part A Calculate the rms speed of an oxygen gas molecule, O2, at 23.0 °C. Express your answer numerically in meters per second. ▸ View Available Hint(s) Submit ▾ Part B Rank the following gases in order of decreasing rate of effusion. Rank from the highest to lowest effusion rate. To rank items as equivalent, overlap them. ▸ View Available Hint(s) Submit - Part C Highest rate of effusion G: ? m/s He PH3 Ar H₂ C4H10 rate of NH3 effusion rate of CO effusion Reset Help Lowest rate of effusion How much faster do ammonia (NH3) molecules effuse than carbon monoxide (CO) molecules? Enter the ratio of the rates of effusion. Express your answer numerically using three significant f ▸ View Available Hint(s) ⒸEB

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Learning Goal: In a given sample of gas, the particles move at varying speeds. The root mean square speed (rms speed) of particles in a gas sample, u, is given by the formula 3RT U = V M where T is the Kelvin temperature, M is the molar mass in kg/mol, and R = 8.314 J/(mol. K) is the gas constant. Effusion is the escape of gas molecules through a tiny hole into a vacuum. The rate of effusion of a gas is directly related to the rms speed of the gas molecules, so it's inversely proportional to the square root of its mass. The rms speed is related to kinetic energy, rather than average speed, and is the speed of a molecule possessing a kinetic energy identical to the average kinetic energy of the sample. Given its relationship to the mass of the molecule, you can conclude that the lighter the molecules of the gas, the more rapidly it effuses. Mathematically, this can be expressed as effusion rate x Vm The relative rate of effusion can be expressed in terms of molecular masses mд and mB as rate of gas A effusion mB rate of gas B effusion √ MA Part A Calculate the rms speed of an oxygen gas molecule, O2, at 23.0 °C Express your answer numerically in meters per second. ▸ View Available Hint(s) Submit Part B 6 Part C Submit ( E3 Rank the following gases in order of decreasing rate of effusion. Rank from the highest to lowest effusion rate. To rank items as equivalent, overlap them. ▸ View Available Hint(s) Highest rate of effusion ? He PH3 Ar H2 C4H10 rate of NH3 effusion rate of CO effusion m/s The sun nk umutima mmmmmi ha datamina i una al Reset Help He Lowest rate of effusion How much faster do ammonia (NH3) molecules effuse than carbon monoxide (CO ) molecules? Enter the ratio of the rates of effusion. Express your answer numerically using three significant figures. ▸ View Available Hint(s) Be = ?
Transcribed Image Text:Learning Goal: In a given sample of gas, the particles move at varying speeds. The root mean square speed (rms speed) of particles in a gas sample, u, is given by the formula 3RT U = V M where T is the Kelvin temperature, M is the molar mass in kg/mol, and R = 8.314 J/(mol. K) is the gas constant. Effusion is the escape of gas molecules through a tiny hole into a vacuum. The rate of effusion of a gas is directly related to the rms speed of the gas molecules, so it's inversely proportional to the square root of its mass. The rms speed is related to kinetic energy, rather than average speed, and is the speed of a molecule possessing a kinetic energy identical to the average kinetic energy of the sample. Given its relationship to the mass of the molecule, you can conclude that the lighter the molecules of the gas, the more rapidly it effuses. Mathematically, this can be expressed as effusion rate x Vm The relative rate of effusion can be expressed in terms of molecular masses mд and mB as rate of gas A effusion mB rate of gas B effusion √ MA Part A Calculate the rms speed of an oxygen gas molecule, O2, at 23.0 °C Express your answer numerically in meters per second. ▸ View Available Hint(s) Submit Part B 6 Part C Submit ( E3 Rank the following gases in order of decreasing rate of effusion. Rank from the highest to lowest effusion rate. To rank items as equivalent, overlap them. ▸ View Available Hint(s) Highest rate of effusion ? He PH3 Ar H2 C4H10 rate of NH3 effusion rate of CO effusion m/s The sun nk umutima mmmmmi ha datamina i una al Reset Help He Lowest rate of effusion How much faster do ammonia (NH3) molecules effuse than carbon monoxide (CO ) molecules? Enter the ratio of the rates of effusion. Express your answer numerically using three significant figures. ▸ View Available Hint(s) Be = ?
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