Need help with parts C, D, and E pls Part CWhat is the rms speed vo of molecules in air at 0° C? Air is composed mostly of N2 molecules, so you may assume that ithas molecules of average mass 28.0 × 1.661 × 10-27 kg = 4.65 × 10¬2° kg.Express your answer in meters per second, to the nearest integer.ηνα ΑΣφ?Vo =285m/sSubmitPrevious Answers Request AnswerX Incorrect; Try Again; 5 attempts remainingNow consider a rigid dumbbell with two masses, each of mass m, spaced a distance d apart.Part DFind1/(w%)avg, the rms angular speed of the dumbbell about a single axis (taken to be the x axis), assuming that thedumbbell is lined up on the z axis and is in equilibrium at temperature T.Express the rms angular speed in terms of T, kB, m, d, and other given quantities. Part EWhat is the typical rotational frequency frot for a molecule like N2 at room temperature (25 °C)? Assume that d for thismolecule is 1 A = 10¬10 m. Take the total mass of an N2 molecule to be mN, = 4.65 × 10¬26 kg. You will need toaccount for rotations around two axes (not just one) to find the correct frequency.Express frot numerically in hertz, to three significant figures.?frotHz%DSubmitRequest Answer

(C) What is the rms speed v0 of molecules in air at 0°C? Air is composed mostly of N2 molecules, so…

Part C °C? Air is composed mostly of N2 molecules, so you may assume that i kg. What is the rms speed vo of molecules in air at -26 has molecules of average mass 28.0 × 1.661 × 10-27 kg = 4.65 × 10° Express your answer in meters per second, to the nearest integer. ΑΣφ ? vo = |285 m/s Submit Previous Answers Request Answer X Incorrect; Try Again; 5 attempts remaining w consider a rigid dumbbell with two masses, each of mass m, spaced a distance d apart. Part D V dumbbell is lined up on the z axis and is in equilibrium at temperature T. Find 1/(w%)avg, the rms angular speed of the dumbbell about a single axis (taken to be the x axis), assuming that the

Part C °C? Air is composed mostly of N2 molecules, so you may assume that i kg. What is the rms speed vo of molecules in air at -26 has molecules of average mass 28.0 × 1.661 × 10-27 kg = 4.65 × 10° Express your answer in meters per second, to the nearest integer. ΑΣφ ? vo = |285 m/s Submit Previous Answers Request Answer X Incorrect; Try Again; 5 attempts remaining w consider a rigid dumbbell with two masses, each of mass m, spaced a distance d apart. Part D V dumbbell is lined up on the z axis and is in equilibrium at temperature T. Find 1/(w%)avg, the rms angular speed of the dumbbell about a single axis (taken to be the x axis), assuming that the

Principles of Physics: A Calculus-Based Text

5th Edition

ISBN:9781133104261

Author:Raymond A. Serway, John W. Jewett

Publisher:Raymond A. Serway, John W. Jewett

Chapter16: Temperature And The Kinetic Theory Of Gases

Section: Chapter Questions

Problem 74P: A cylinder that has a 40.0-cm radius and is 50.0 cm deep is filled with air at 20.0C and 1.00 atm...

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Fifteen identical particles have various speeds: one has a speed of 2.00 m/s, two have speeds of 3.00 m/s, three have speeds of 5.00 m/s, four have speeds of 7.00 m/s, three have speeds of 9.00 m/s, and two have speeds of 12.0 m/s. Find (a) the average speed, (b) the rms speed, and (c) the most probable speed of these particles.
Cylinder A contains oxygen (O2) gas, and cylinder B contains nitrogen (N2) gas. If the molecules in the two cylinders have the same rms speeds, which of the following statements is false? (a) The two gases haw different temperatures. (b) The temperature of cylinder B is less than the temperature of cylinder A. (c) The temperature of cylinder B is greater than the temperature of cylinder A. (d) The average kinetic energy of the nitrogen molecules is less than the average kinetic energy of the oxygen molecules.
Consider the Maxwell-Boltzmann distribution function plotted in Problem 28. For those parameters, determine the rms velocity and the most probable speed, as well as the values of f(v) for each of these values. Compare these values with the graph in Problem 28. 28. Plot the Maxwell-Boltzmann distribution function for a gas composed of nitrogen molecules (N2) at a temperature of 295 K. Identify the points on the curve that have a value of half the maximum value. Estimate these speeds, which represent the range of speeds most of the molecules are likely to have. The mass of a nitrogen molecule is 4.68 1026 kg. Equation 20.18 can be used to find the rms velocity given the temperature, Boltzmanns constant, and the mass of the atom or molecule. The mass of a nitrogen molecule is 4.68 1026 kg. vrms=3kBTm=3(1.381023J/K)4.681026kg=511m/s Using the results of Problem 28 and the rms velocity, we can calculate the value of f(v). f(vrms) = (3.11 108)(511)2 e(5.75106(511)2) = 0.00181 The most probable speed, for which this function has its maximum value, is given by Equation 20.20. vmp=2kBTm=2(1.381023J/K)(295K)4.681026kg=417m/s f(vmp) = (3.11108)(417)2 e(5.75106(417)2) = 0.00199 We plot these points on the speed distribution. The most probable speed is indeed at the peak of the distribution function. Since the function is not symmetric, the rms velocity is somewhat higher than the most probable speed. Figure P20.29ANS
(a) Show that the density of an ideal gas occupying a volume V is given by = PM/KT, where M is the molar mass. (b) Determine the density of oxygen gas at atmospheric pressure and 20.0C.
One cylinder contains helium gas and another contains krypton gas at the same temperature. Mark each of these statements true, false, or impossible to determine from the given information. (a) The rms speeds of atoms in the two gases are the same. (b) The average kinetic energies of atoms in the two gases are the same. (c) The internal energies of 1 mole of gas in each cylinder are the same. (d) The pressures in the two cylinders ale the same.
An ideal gas is contained in a vessel at 300 K. The temperature of the gas is then increased to 900 K. (i) By what factor does the average kinetic energy of the molecules change, (a) a factor of 9, (b) a factor of 3, (c) a factor of 3, (d) a factor of 1, or (e) a factor of 13? Using the same choices as in part (i), by what factor does each of the following change: (ii) the rms molecular speed of the molecules, (iii) the average momentum change that one molecule undergoes in a collision with one particular wall, (iv) the rate of collisions of molecules with walls, and (v) the pressure of the gas?
A gas is at 200 K. If we wish to double the rms speed of the molecules of the gas, to what value must we raise its temperature? (a) 283 K (b) 400 K (c) 566 K (d) 800 K (e) 1 130 K
What is the gauge pressure inside a tank of 4.86104 mol of compressed nitrogen with a volume of 6.56 m3 if the rms speed is 514 m/s?
Using the approximation v1v1+v f(v)dvf(v1)v for small v , estimate the fraction of nitrogen molecules at a temperature of 3.00102 K that have speeds between 290 m/s and 291 m/s.
Find (a) the most probable speed, (b) the average speed, and (c) the rms speed for nitrogen molecules at 295 K.
At what temperature is the average speed of carbon dioxide molecules ( M=44.0 g/mol) 510 m/s?
A cubic container of volume 2.00 L holds 0.500 mol of nitrogen gas at a temperature of 25.0 . What is the net force due to the nitrogen on one wall of the container? Compare that force to the sample's weight.