The average kinetic energy of the molecules in a gas sample depends only on the temperature, 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 3RT rms speed = V M where R = 8.314 J/(mol·K) and M 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 Cl₂ molecules at 489 K? rms speed: What is the rms speed of He atoms at 489 K? rms speed: m/s m/s

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Chapter1: Chemical Foundations
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The average kinetic energy of the molecules in a gas sample depends only on the temperature, 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 =
where R = 8.314 J/(mol·K) and M 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 Cl₂ molecules at 489 K?
rms speed:
3RT
M
What is the rms speed of He atoms at 489 K?
rms speed:
m/s
m/s
Transcribed Image Text:Macmillan Learning The average kinetic energy of the molecules in a gas sample depends only on the temperature, 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 = where R = 8.314 J/(mol·K) and M 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 Cl₂ molecules at 489 K? rms speed: 3RT M What is the rms speed of He atoms at 489 K? rms speed: m/s m/s
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