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 3 RT 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/s3). What is the rms speed of N, molecules at 365 K? rms speed: m/s What is the rms speed of He atoms at 365 K? rms speed: m/s

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 3 RT 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/s3). What is the rms speed of N, molecules at 365 K? rms speed: m/s What is the rms speed of He atoms at 365 K? rms speed: m/s

Chemistry

10th Edition

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. However, given the same kinetic energies, a lighter molecule will move faster than a heavier molecule, as shown in the equation for rms speed 3 RT 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-mIs²). What is the rms speed of O, molecules at 307 K? rms speed: m/s What is the rms speed of He atoms at 307 K? rms speed: m/s
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Suppose you have 1.25 moles of gaseous napthalene (C10H8) at T = 292 K. What is the average kinetic energy of one molecule of napthalene? (The molar mass of napthalene is 128 g/mol. You may assume that the gas molecules behave ideally.)
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Consider separate 1.0-L gaseous samples of He, Kr, Cl2, and O2 all at STP. a Rank the gases in order of increasing average kinetic energy. O (KE)avg (He) < (KE),vg (Kr) < (KE)avg (Cl2) = (KE),vg (O2) O (KE)avg (He) = (KE)avg (Kr) < (KE)avg (Cl2) < (KE),vg (O2) O (KE)avg (Kr) < (KE),vg(Cl2) = (KE),vg (O2) < (KE),vg (He) (KE)avg (He) = (KE),vg (Kr) = (KE)vg (Cl2) = (KE),vg (O2) b Rank the gases in order of increasing average velocity. Uavg (Kr) = uavg (Cl2) = uavg (He) = uavg (O2) O uavg (Kr) < uavg (Cl2) < uavg (He) < uavg (O2) O Uavg (Kr) < uavg (O2) < Uavg (Cl2) < Uavg (He) O uavg (Kr) < uavg (Cl2) < Uavg (O2) < uavg (He) C How can separate 1.0-L samples of O2 and He each have the same average velocity? Separate samples of He and O2 can only have the same average velocities if the temperature of the O2 sample is He sample. - the temperature of the
The average kinetic energy of the molecules in a gas sample depends only on the temperature T. R=8.314. What is the rms speed 02 molecules at 443 K? What is the rms speed of He atoms at 443 K?