The average kinetic energy of the molecules in a gas sample depends only on the temperature, T.T. However, given the same kinetic energies, a lighter molecule will move faster than a heavier molecule, as shown in the equation for rms speed rms speed=√3RTMrms speed=3RTℳ where R=8.314 J/(mol⋅K)R=8.314 J/(mol⋅K) and Mℳ is molar mass in kilograms per mole. Note that a joule is the same as a kilogram‑meter squared per second squared (kg·m2/s2). What is the rms speed of N2N2 molecules at 347 K? _____m/s What is the rms speed of HeHe atoms at 347 K? _____m/s
The average kinetic energy of the molecules in a gas sample depends only on the temperature, T.T. However, given the same kinetic energies, a lighter molecule will move faster than a heavier molecule, as shown in the equation for rms speed rms speed=√3RTMrms speed=3RTℳ where R=8.314 J/(mol⋅K)R=8.314 J/(mol⋅K) and Mℳ is molar mass in kilograms per mole. Note that a joule is the same as a kilogram‑meter squared per second squared (kg·m2/s2). What is the rms speed of N2N2 molecules at 347 K? _____m/s What is the rms speed of HeHe atoms at 347 K? _____m/s
Chemistry
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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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The average kinetic energy of the molecules in a gas sample depends only on the temperature, T.T. However, given the same kinetic energies, a lighter molecule will move faster than a heavier molecule, as shown in the equation for rms speed
rms speed=√3RTMrms speed=3RTℳ
where R=8.314 J/(mol⋅K)R=8.314 J/(mol⋅K) and Mℳ is molar mass in kilograms per mole. Note that a joule is the same as a kilogram‑meter squared per second squared (kg·m2/s2).
What is the rms speed of N2N2 molecules at 347 K?
_____m/s
What is the rms speed of HeHe atoms at 347 K?
_____m/s
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