Molecular Speed of Gases Formula With Boltzmann's Constant | Summary and Q&A

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November 26, 2017
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The Organic Chemistry Tutor
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Molecular Speed of Gases Formula With Boltzmann's Constant

TL;DR

Learn two methods for calculating the root mean square molecular speed of nitrogen gas at 300 Kelvin.

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Questions & Answers

Q: What is the formula for calculating the root mean square molecular speed of nitrogen gas at 300 Kelvin?

The formula is 3kt/mass, where k is Boltzmann's constant and mass is the mass of a single nitrogen gas molecule.

Q: How can the atomic mass of nitrogen be converted to kilograms?

The atomic mass of nitrogen is 14.01 atomic mass units, so by multiplying it by 1.66 x 10^-27, we get 4.651 x 10^-26 kilograms.

Q: What is the alternative formula for calculating the root mean square velocity?

The alternative formula is 3rt/molar mass, where r is the ideal gas constant and molar mass is the molar mass of N2.

Q: How can the molar mass of nitrogen gas be converted to kilograms per mole?

The molar mass of N2 is 28.02 atomic mass units, which can be converted to grams per mole (28.02 grams per mole). By further converting grams to kilograms (0.02802 kilograms per mole), we get the desired conversion.

Summary & Key Takeaways

  • The root mean square molecular speed of nitrogen gas at 300 Kelvin can be calculated using the formula 3kt/mass, where k is Boltzmann's constant and mass is the mass of a single nitrogen gas molecule.

  • The atomic mass of nitrogen is 14.01, but since we have two nitrogen gas molecules in this problem, the mass is 28.02 atomic mass units, which can be converted to 4.651 x 10^-26 kilograms.

  • Another equation that can be used is 3rt/molar mass, where r is the ideal gas constant, and molar mass is the molar mass of N2. By converting the atomic mass to grams and then to kilograms, the molar mass is calculated as 0.02802 kilograms per mole.

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