Calculate the root mean square velocity and kinetic energy of CO, CO 2 , and SO 3 at 298 K. Which gas has the greatest velocity? The greatest kinetic energy? The greatest effusion rate?

Hey everyone. So here we ask to use the root mean square velocity and the kinetic energy of N. H. Two minus NH three and NH four plus to determine the lowest infusion rate, the lowest velocity and the lowest kinetic energy. So the root mean square velocity he goes to square root free R. T. By the molar mass. And the kinetic energy one half of the mass times velocity squared. So for a infusion rate is inversely proportional to the Mueller mass. As the molar mass increases, the rate of effusion decreases. If you look at the molar mass of each, For NH 2 -, We're gonna have 14.007 g. Us too. That was 1.008 grams. And this gives us 16.0-3 grams in the Mueller mass. NH three Gonna give us 14.007g plus three. 1.008. This will give us 17.031 in the Mueller mass. NH four Gonna give us 14.007g plus four Times 1.008. This give us 18.039. The largest smaller mass is gonna have the lowest effusion rate. So NH four plus. And I have the lowest infusion rate. And for b the lower the mass the Lord the velocity NH 2 - has the lowest mass. NH two minus gonna have the lowest velocity. And for c the lower the mass the lower the kinetic energy NH 2 - has the lowest mass. So NH 2 -. Gonna have the lowest kinetic energy. Thanks for watching my video, and I hope it was helpful.

Ch.5 - Gases

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Problem 84

Chapter 5, Problem 84

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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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.

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.

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

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