Physics for Scientists and Engineers
10th Edition
ISBN: 9781337553278
Author: Raymond A. Serway, John W. Jewett
Publisher: Cengage Learning
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Chapter 20, Problem 45CP
(a)
To determine
The average of the velocity
(b)
To determine
The rms velocity is
(c)
To determine
The rms velocity is greater than the average velocity.
(d)
To determine
The condition in which the
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Chapter 20 Solutions
Physics for Scientists and Engineers
Ch. 20.1 - Two containers hold an ideal gas at the same...Ch. 20.2 - (i) How does the internal energy of an ideal gas...Ch. 20.3 - Prob. 20.3QQCh. 20.3 - Prob. 20.4QQCh. 20 - A spherical balloon of volume 4.00 103 cm3...Ch. 20 - A spherical balloon of volume V contains helium at...Ch. 20 - A 2.00-mol sample of oxygen gas is confined to a...Ch. 20 - Oxygen, modeled as an ideal gas, is in a container...Ch. 20 - A 5.00-L vessel contains nitrogen gas at 27.0C and...Ch. 20 - Prob. 6P
Ch. 20 - In a period of 1.00 s, 5.00 1023 nitrogen...Ch. 20 - A 7.00-L vessel contains 3.50 moles of gas at a...Ch. 20 - Calculate the change in internal energy of 3.00...Ch. 20 - Prob. 10PCh. 20 - In a constant-volume process, 209 J of energy is...Ch. 20 - A vertical cylinder with a heavy piston contains...Ch. 20 - A 1.00-L insulated bottle is full of tea at 90.0C....Ch. 20 - A certain molecule has f degrees of freedom. Show...Ch. 20 - You are working for an automobile tire company....Ch. 20 - Why is the following situation impossible? A team...Ch. 20 - You and your younger brother are designing an air...Ch. 20 - During the compression stroke of a certain...Ch. 20 - Air in a thundercloud expands as it rises. If its...Ch. 20 - Why is the following situation impossible? A new...Ch. 20 - Air (a diatomic ideal gas) at 27.0C and...Ch. 20 - Prob. 22PCh. 20 - Prob. 23PCh. 20 - Prob. 24PCh. 20 - Prob. 25PCh. 20 - The law of atmospheres states that the number...Ch. 20 - Prob. 27APCh. 20 - Prob. 28APCh. 20 - The dimensions of a classroom are 4.20 m 3.00 m ...Ch. 20 - Prob. 30APCh. 20 - The Earths atmosphere consists primarily of oxygen...Ch. 20 - Review. As a sound wave passes through a gas, the...Ch. 20 - Prob. 33APCh. 20 - In a cylinder, a sample of an ideal gas with...Ch. 20 - As a 1.00-mol sample of a monatomic ideal gas...Ch. 20 - A sample consists of an amount n in moles of a...Ch. 20 - The latent heat of vaporization for water at room...Ch. 20 - A vessel contains 1.00 104 oxygen molecules at...Ch. 20 - Prob. 39APCh. 20 - Prob. 40APCh. 20 - Prob. 41APCh. 20 - On the PV diagram for an ideal gas, one isothermal...Ch. 20 - Prob. 43APCh. 20 - Prob. 44APCh. 20 - Prob. 45CP
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- So each four dot shows four different states for an ideal gas. P is the pressure and the other one is the density of the gas. Is temperature of state 1 less or greater than the state 2? Can you please explain why?arrow_forwardIf one could somehow (pretend) get the temperature of an ideal gas to be absolute zero (i.e., 0 K) which of the following properties of the molecules of that gas would not be zero? (If you do not like pretending, for an ideal gas which of the following properties of the molecules does not have to be close to zero when the temperature is close to absolute zero?) Group of answer choices a) Average speed would not go to zero. b) Average momentum would not go to zero. c) Average kinetic energy would not go to zero. d) More than one of these would not go to zero. e) None of these (that is, they would all go to zero).arrow_forwardCylinder 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.arrow_forward
- Consider a gas filling two connected chambers that are separated by a removable barrier (Fig. P20.68). The gas molecules on the left (red) are initially at a higher temperature than the ones on the right (blue). When the barrier between the two chambers is removed, the molecules begin to mix and move from one chamber to the other. a. Describe what happens to the temperature in the left chamber and in the right chamber as time goes on, once the barrier is open. Discuss in terms of the mixing of the molecules from each gas. b. Describe what happens to the most probable speed and average speed in the left chamber and in the right chamber as time goes on, once the barrier is open. Do they increase or decrease by the same factor? Explain. FIGURE P20.68 Problems 68 and 69.arrow_forwardCan someone give me the full solution and detailed explanation?If a certain amount of ideal gas occupies a volume V at STP on earth, what would be its volume (in terms of V) on Venus, where the temperature is 1003°C and the pressure is 92 atm?arrow_forwardOne type of gas mixture used in anesthesiology is a 50%/50% mixture (by volume) of nitrous oxide (N2O) and oxygen (O2), which can be premixed and kept in a cylinder for later use. Because these two gases don't react chemically at or below 2000 psi, at typical room temperatures they form a homogeneous single gas phase, which can be considered an ideal gas. If the temperature drops below -6∘C, however, N2O may begin to condense out of the gas phase. Then any gas removed from the cylinder will initially be nearly pure O2; as the cylinder empties, the proportion of O2 will decrease until the gas coming from the cylinder is nearly pure N2O. In a test of the effects of low temperatures on the gas mixture, a cylinder filled at 27.0 ∘C to 2000 psi (gauge pressure) is cooled slowly and the pressure is monitored. What is the expected pressure at -5.00∘C if the gas remains a homogeneous mixture?arrow_forward
- One type of gas mixture used in anesthesiology is a 50% / 50% mixture (by volume) of nitrous oxide (N2O) and oxygen (O2), which can be premixed and kept in a cylinder for later use. Because these two gases don't react chemically at or below 2000 psi, at typical room temperatures they form a homogeneous single gas phase, which can be considered an ideal gas. If the temperature drops below -6°C, however, N2O may begin to condense out of the gas phase. Then any gas removed from the cylinder will initially be nearly pure O2; as the cylinder empties, the proportion of O2 will decrease until the gas coming from the cylinder is nearly pure N2O. In a test of the effects of low temperatures on the gas mixture, a cylinder filled at 25.0°C to 2000 psi (gauge pressure) is cooled slowly and the pressure is monitored.1. What is the expected pressure at -5.00∘C if the gas remains a homogeneous mixture?arrow_forwardConsider a sample of weakly interacting gas consisting of 1,000 atoms confined in a cubic container of side length 1 cm at a temperature of 300 K. The average distance between neighboring atoms is estimated to be 10 nm. Assume the gas behaves ideally and is described by the ideal gas equation of state. Calculate the average pressure exerted by the gas.arrow_forwardIn ideal gas, what happens to the pressure and temperature if the conainter of gas particles becomes small?arrow_forward
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