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 = 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-m?/s²). What is the rms speed of F, molecules at 485 K?
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 = 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-m?/s²). What is the rms speed of F, molecules at 485 K?
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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
\[
\text{rms speed} = \sqrt{\frac{3RT}{\mathcal{M}}}
\]
where \( R = 8.314 \, \text{J/(mol} \cdot \text{K)} \) and \( \mathcal{M} \) is molar mass in kilograms per mole. Note that a joule is the same as a kilogram-meter squared per second squared (\( \text{kg} \cdot \text{m}^2/\text{s}^2 \)).
What is the rms speed of \( \text{F}_2 \) molecules at 485 K?](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fc6ae9165-8c64-40e9-9a68-65bc31ca98b7%2F2fadd012-8fc8-4161-ba1f-f6e9e80eca13%2F3od6e0l_processed.png&w=3840&q=75)
Transcribed Image Text: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
\[
\text{rms speed} = \sqrt{\frac{3RT}{\mathcal{M}}}
\]
where \( R = 8.314 \, \text{J/(mol} \cdot \text{K)} \) and \( \mathcal{M} \) is molar mass in kilograms per mole. Note that a joule is the same as a kilogram-meter squared per second squared (\( \text{kg} \cdot \text{m}^2/\text{s}^2 \)).
What is the rms speed of \( \text{F}_2 \) molecules at 485 K?
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Step 1
Given
R = 8.314 J/(mol.K)
T = 485 K
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