20.17 In the figure V23 = 3V₁; n moles of a diatomic ideal gas are taken through the cycle with the molecules rotating but not oscillating. What are: (a) P₂/P₁, (b) p3/p₁ and (c) T3/T₁; For 1-2 find (d) W/nRT₁, (e) Q/nRT₁, (f) AEint/nRT₁, (g) AS/nR. For 2-3 find (h) W/nRT₁, (i) Q/nRT₁, (j) AEint/nRT₁, (k) AS/nR, For 3-1 find (1) W/nRT₁, (m) Q/nRT₁, (n)AEint/nRT₁, (o) AS/nR? (p) What is the efficiency of this cycle? Pressure Adiabatic Isothermal Volume MAR

20.17 In the figure V23 = 3V₁; n moles of a diatomic ideal gas are taken through the cycle with the molecules rotating but not oscillating. What are: (a) P₂/P₁, (b) p3/p₁ and (c) T3/T₁; For 1-2 find (d) W/nRT₁, (e) Q/nRT₁, (f) AEint/nRT₁, (g) AS/nR. For 2-3 find (h) W/nRT₁, (i) Q/nRT₁, (j) AEint/nRT₁, (k) AS/nR, For 3-1 find (1) W/nRT₁, (m) Q/nRT₁, (n)AEint/nRT₁, (o) AS/nR? (p) What is the efficiency of this cycle? Pressure Adiabatic Isothermal Volume MAR

University Physics Volume 2

18th Edition

ISBN:9781938168161

Author:OpenStax

Publisher:OpenStax

Chapter3: The First Law Of Thermodynamics

Section: Chapter Questions

Problem 35P: Two monatomic ideal gases A and B are at the same temperature. If 1.0 g of gas A has the same...

See similar textbooks

Similar questions

Suppose a tank contains 809 m3 of neon (Ne) at an absolute pressure of 1.02 x 105 Pa. The temperature is changed from 293.2 to 294.7 K. What is the increase in the internal energy of the neon?
A 1.00 mol sample of an ideal diatomic gas, originally at 1.00 atm and 20 oC, expands adiabatically to 1.75 times its initial volume. What are the final pressure and temperature for the gas? ( Assume no molecular vibration)
A sample of a monatomic ideal gas occupies 5.00 L at atmospheric pressure and 300 K (point A in Fig. P17.68). It is warmed at constant volume to 3.00 atm (point B). Then it is allowed to expand isothermally to 1.00 atm (point C) and at last compressed isobarically to its original state. (a) Find the number of moles in the sample. Find (b) the temperature at point B, (c) the temperature at point C, and (d) the volume at point C. (e) Now consider the processes A B, B C, and C A. Describe how to carry out each process experimentally. (f) Find Q, W, and Eint for each of the processes. (g) For the whole cycle A B C A, find Q, W, and Eint. Figure P17.68
One process for decaffeinating coffee uses carbon dioxide ( M=44.0 g/mol) at a molar density of about 14,0 mol/m3 and a temperature of about 60 . (a) Is CO2 a solid, liquid, gas, or supercritical fluid under those conditions? (b) The van der Waals constants for carbon dioxide are a=0.3658 Pa m6/mol2 and b=4.286105 m3/mol. Using the van der Waals equation, estimate pressure of CO2 at that temperature and density. `
An ideal gas has a pressure of 0.50 atm and a volume of 10 L. It is compressed adiabatically and quasi-statically until its pressure is 3.0 atm and its volume is 2.8 L. Is the monatomic, diatomic, or polyatomic?
A sample of a monatomic ideal gas occupies 5.00 L at atmospheric pressure and 300 K (point A in Fig. P21.65). It is warmed at constant volume to 3.00 atm (point B). Then it is allowed to expand isothermally to 1.00 atm (point C) and at last compressed isobarically to its original state, (a) Find the number of moles in the sample. Find (b) the temperature at point B, (c) the temperature at point C, and (d) the volume at point C. (e) Now consider the processes A B, B C, and C A. Describe how to carry out each process experimentally, (f) Find Q, W, and Eint for each of the processes, (g) For the whole cycle A B C A, find Q, W, and Eint.
Two monatomic ideal gases A and B are at the same temperature. If 1.0 g of gas A has the same internal energy as 0.10 g of gas B, what are (a) the ratio of the number of moles of each gas and (b) the ration of the atomic masses of the two gases?
Find (a) the most probable speed, (b) the average speed, and (c) the rms speed for nitrogen molecules at 295 K.
Expand 1.00 mol of an monatomic gas initially at 5.00 kPaand 600 K from initial volume Vi = 1.00 m3 to final volume Vf =2.00 m3. At any instant during the expansion, the pressure p and volumeV of the gas are related by p = 5.00 exp[(Vi - V)/a], with p inkilopascals, Vi and V in cubic meters, and a = 1.00 m3.What are thefinal (a) pressure and (b) temperature of the gas? (c) How muchwork is done by the gas during the expansion? (d) What is S for theexpansion? (Hint: Use two simple reversible processes to find S.)
Under constant pressure, the temperature of 2.00 mol of an ideal monatomic gas is raised 15.0 K. What are (a) the work W done by the gas, (b) the energy transferred as heat Q, (c) the change Eint in the internal energy of the gas, and (d) the change K in the average kinetic energy per atom?
Only answer letters (d) and (e) a) Using the Maxwell-Boltzmann function, calculate the fraction of argon gas molecules with a speed of 305 m/s at 500 K. (ans: 0.0014) b) If the system in (a) has 0.46 moles of argon gas, how many molecules have the speed of 305 m/s? (ans: 6.44 x 10-4) c) Calculate the values of vmp, vavg, and vrms for xenon gas at 298 K. (ans: Vmp=194.2 m/s , Vavg=219.2 m/s , Vrms=237.8 m/s) d) From the values calculated in (c), label the Boltzmann distribution plot with the approximate locations of vmp, v avg, and vrms e) What will have a larger speed distribution, helium at 500 K or argon at 300 K? Helium at 300 K or argon at 500 K? Argon at 400 K or argon at 1000 K?
Suppose 4.00 mol of an ideal diatomic gas, with molecular rotation but not oscillation, experienced a temperature increase of 60.0 K under constant-pressure conditions. What are (a) the energy transferred as heat Q, (b) the change Eint in internal energy of the gas, (c) the work W done by the gas, and (d) the change K in the total translational kinetic energy of the gas?