COLLEGE PHYSICS
2nd Edition
ISBN: 9781464196393
Author: Freedman
Publisher: MAC HIGHER
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Chapter 14, Problem 113QAP
To determine
The average kinetic energy for the ideal gas made up of diatomic molecules that can move in two dimensions.
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Suppose the volume of an ideal gas is doubled while the pressure is reduced by half. Does the thermal energy of the gas increase, decrease or remain the same? Explain.
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Chapter 14 Solutions
COLLEGE PHYSICS
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- 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 P20.29ANSarrow_forwardIf you add boiling water to a cup at room temperature, what would you expect the final equilibrium temperature of the unit to be? You will need to include 1he surroundings as pan of the system. Consider the zeroth law of thermodynamics.arrow_forwardWhat is the average mechanical energy of the atoms of an ideal monatomic gas at 300 K?arrow_forward
- Compare the charge in internal energy of an ideal gas for a quasi-static adiabatic expansion with that for a quasi-static isothermal expansion. What happens to the temperature of an ideal gas in an adiabatic expansion?arrow_forwardIf the translational speed of molecules in an ideal gas isdoubled, by what factor does the Kelvin temperature change?Explainarrow_forwardA certain volume of gas at atmospheric pressure is compressed adiabatically to (1/5)th of its original volume. Calculate the resulting pressure. Given y=1.4 .arrow_forward
- 2. For an ideal gas, when both the pressure and volume are each halved, then the (Kelvin) temperature is A. also halved B. quadrupled C. unchanged D. decreased by 4x E. doubledarrow_forwardExplain why the temperature of gas drops in an adiabatic expansion.arrow_forwardUse the Maxwell distribution to calculate the average value of v2 for the molecules in an ideal gas. Check that your answer agrees with equation 6.41 (Attached).arrow_forward
- Explain why the internal energy of the air increases as the tyre is inflated.arrow_forwardTwo moles of an ideal gas initially at 0∘C and 1.04 x 105 Pa expands isobarically to twice its original volume. Determine the work done by the gas in the process.arrow_forwardIs it possible to change both the pressure and the volume of anideal gas without changing the average kinetic energy of its molecules? If your answer is no, explain why not. If your answer is yes,give a specific examplearrow_forward
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