In the kinetic molecular modelof an ideal gas, which of thefollowing statements is TRUEwhen a gas molecule collideswith the container wall?The speed of the molecule becomeszero.The speed of the molecule does notchange.The speed of the moleculeincreases after the collision.The speed of the moleculedecreases after the collision.All of the above statements areTRUE.All of the above statements are NOTtrue.

According to kinetic molecular model of an ideal gas : The collision between molecules and the wall…

Answered: In the kinetic molecular model of an…

University Physics Volume 2

18th Edition

ISBN:9781938168161

Author:OpenStax

Publisher:OpenStax

Chapter2: The Kinetic Theory Of Gases

Section: Chapter Questions

Problem 88AP: Find the total number of collisions between molecules in 1.00 s in 1.00 L of nitrogen gas at...

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In the simple kinetic theory of a gas we discussed in class, the molecules are assumed to be point-like objects (without any volume) so that they rarely collide with one another. In reality, each molecule has a small volume and so there are collisions. Let's assume that a molecule is a hard sphere of radius r. Then the molecules will occasionally collide with each other. The average distance traveled between two successive collisions (called mean free path) is λ = V/(4π √2 r2N) where V is the volume of the gas containing N molecules. Calculate the mean free path of a H2 molecule in a hydrogen gas tank at STP. Assume the molecular radius to be 10-10 a) 2.1*10-7 m b) 4.2*10-7 m c) none of these.
Determine how many times per second each molecule moving with rms speed would move back and forth across a 6.6 mm-long room on average, assuming it made very few collisions with other molecules.To find Vx use the equation v^2=v^2x+v^2y+v^2zand the fact that molecules have no preferred direction.
Suppose a 2.5 g oxygen gas is in a 4 L container. Assume the diameter of oxygen is 3.55 Angstroms. a/ Calculate the mean free path of the molecules. b/ If the total translational kinetic energy of the oxygen gas is 0.98 kJ, compute the pressure of the gas.
Calculate rms velocity of CO2 molecule at NTP.
You measure the average free path λ and the average collision time τ of the molecules of a diatomic gas of molecular mass 6.00 × 10-²⁵ kg and radius r = 1.0 x 10-¹⁰ m. From these microscopic data can we obtain macroscopic properties such as temperature T and pressure P? If so, consider λ = 4.32 x 10-⁸ m and τ = 3.00 x 10-¹⁰ s and calculate T and P. indicate the correct answer: 1- Not possible2- Yes, T =150 K and P ~ 2.04 atm.3- Yes, T = 150 K and P ~ 4.08 atm.4- Yes, T = 300 K and P ~ 4.08 atm.5- Yes, T = 300 K and P ~ 5.32 atm6- Yes, T = 400 K and P ~ 4.08 atm.7- Yes, T = 400 K and P ~ 5.32 atm. obs.: If necessary, consider: R = 8.314 J/mol∙K1 cal = 4.19 Jkb =1,38 x 10⁻²³ m² kg s⁻² K⁻¹
A box contains N molecules. Consider two configurations:configuration A with an equal division of the molecules betweenthe two halves of the box, and configuration B with 60.0% of themolecules in the left half of the box and 40.0% in the right half. ForN = 50, what are (a) the multiplicity WA of configuration A, (b) themultiplicityWB of configuration B, and (c) the ratio fB/A of the timethe system spends in configuration B to the time it spends in configurationA? For N = 100, what are (d) WA, (e) WB, and (f) fB/A?For N = 200, what are (g) WA, (h) WB, and (i) fB/A? ( j) With increasingN, does f increase, decrease, or remain the same?
Calculate the RMS velocity of hydrogen molecule at 127 deg C. The density of hydrogen at NTP is 0.09 kg/m3
Write the Ideal gas law in terms of molecules?
The temperature of a gas consisting a rigid diatomic molecules is T K. Calculate the angular root mean square velocity of the rotating molecules if moment of inertia is I.
One mole of an ideal gas at standard temperature and pressure occupies 22.4 L (molar volume). What is the ratio of molar volume to the atomic volume of a mole of hydrogen ? (Take the size of hydrogen molecule to be about 1 Å). Why is this ratio so large ?
A rigid container contains a mixture of 2mols of a polyatomic gas at a temperature of 3000K. You then heat the mixture providing 39907.02J of heat. At the end of the process, the mixture is at a temperature of 3600K.If at 3000K the translational as well as the 3 rotational degrees of freedom of the polyatomic gas are already activated, how many vibrational degrees of freedom does it have activated in this temperature range? (Assume the number of degrees of freedom does not change during the process).
The density of the distribution of the speed of motion of a molecule along the positive X axis has the form p(s) = 4*squreroot(a3/pi)*s2exp(-as2) (The constant a is determined by the temperature of the gas and the mass of the particle observed; a = m/ (2kT), wherek is the Boltzmann constant)• Find the mean distance traversed by the molecule in a unit of time.• Find the mean value of the kinetic energy of the molecule.

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