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Ch.6 - Gases
Tro - Chemistry: A Molecular Approach 6th Edition
Tro6th EditionChemistry: A Molecular ApproachISBN: 9780137832217Not the one you use?Change textbook
All textbooksTro 6th EditionCh.6 - GasesProblem 92
Chapter 6, Problem 92

Calculate the root mean square velocity and kinetic energy of CO, CO2, and SO3 at 298 K. Which gas has the greatest velocity? The greatest kinetic energy? The greatest effusion rate?

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1
Identify the formula for root mean square velocity: \(v_{rms} = \sqrt{\frac{3RT}{M}}\), where \(R\) is the ideal gas constant, \(T\) is the temperature in Kelvin, and \(M\) is the molar mass in kg/mol.
Convert the molar masses of CO, CO2, and SO3 from g/mol to kg/mol. For CO, it's 28.01 g/mol, for CO2, it's 44.01 g/mol, and for SO3, it's 80.06 g/mol.
Calculate the root mean square velocity for each gas using the formula from step 1, substituting the appropriate molar mass and the given temperature of 298 K.
Use the kinetic energy formula \(KE = \frac{1}{2}mv^2\) to compare the kinetic energies of the gases, where \(m\) is the molar mass and \(v\) is the velocity calculated in step 3.
Apply Graham's law of effusion, which states that the rate of effusion is inversely proportional to the square root of the molar mass, to determine which gas has the greatest effusion rate.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Root Mean Square Velocity

Root mean square (RMS) velocity is a measure of the average speed of gas molecules in a sample. It is calculated using the formula v_rms = sqrt(3RT/M), where R is the ideal gas constant, T is the temperature in Kelvin, and M is the molar mass of the gas in kg/mol. This concept is crucial for comparing the velocities of different gases at the same temperature.
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Kinetic Energy of Gases

The kinetic energy of a gas is related to the motion of its molecules and is given by the formula KE = (1/2)mv^2, where m is the mass of the molecule and v is its velocity. For an ideal gas, the average kinetic energy can also be expressed as KE_avg = (3/2)RT. Understanding this concept helps in determining which gas has the greatest kinetic energy at a given temperature.
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Graham's Law of Effusion

Graham's Law states that the rate of effusion of a gas is inversely proportional to the square root of its molar mass. This means lighter gases effuse faster than heavier gases. This principle is essential for determining which gas will effuse more quickly under the same conditions, allowing for comparisons between CO, CO2, and SO3.
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Related Practice
Textbook Question

Calculate the root mean square velocity and kinetic energy of F2, Cl2, and Br2 at 298 K. Rank these three halogens with respect to their rate of effusion.

Textbook Question

A sample of argon effuses from a container in 112 seconds. The same amount of an unknown noble gas requires 79.6 seconds. Identify the second gas.

Textbook Question

Calculate the ratio of effusion rates for Ar and Kr.

Textbook Question

Calculate the root mean square velocity of F2, Cl2, and Br2 at 298 K.

Textbook Question

Calculate the kinetic energy of F2, Cl2, and Br2 at 298 K.

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Textbook Question

We separate U-235 from U-238 by fluorinating a sample of uranium to form UF6 (which is a gas) and then taking advantage of the different rates of effusion and diffusion for compounds containing the two isotopes. Calculate the ratio of effusion rates for 238UF6 and 235UF6. The atomic mass of U-235 is 235.054 amu and that of U-238 is 238.051 amu.