Part AConsider the adiabatic expansion of an ideal monatomic gas withCym = 3R/2. The initial state is described by P= 9.50 bar andт-303 К.Calculate the final temperature if the gas undergoes a reversible adiabatic expansion to a final pressure of P=1.00 bar.Express the temperature in kelvins to three significant figures.ανα ΑΣφ?T =KSubmitRequest AnswerPart BCalculate the final temperature if the same gas undergoes an adiabatic expansion against an external pressure of P=1.00 bar to a final pressure P=1.00 bar.Expresstemperature in kelvins to three significant figures.?T =KSubmitRequest AnswerPart C Complete previous part(s)

Answered: Image /qna-images/answer/8072f3df-0c3e-4090-8a0c-9da1c04313bd.jpg

Part A Consider the adiabatic expansion of an ideal monatomic gas with Cym - 3R/2 The initial state is described by P=9.50 bar and T= 303 K Calculate final temperature if the gas undergoes a reversible adiabatic expansion to a final pressure of P=1.00 bar Express the temperature in kelvins to three significant figures. ανα ΑΣφ K Submit Request Answer Part B Calculate the final temperature if the same gas undergoes an adiabatic expansion against an external pressure of P= 1.00 bar to a final pressure P=1.00 bar. Express the temperature in kelvins to three significant figures. K Submit Request Answer

Part A Consider the adiabatic expansion of an ideal monatomic gas with Cym - 3R/2 The initial state is described by P=9.50 bar and T= 303 K Calculate final temperature if the gas undergoes a reversible adiabatic expansion to a final pressure of P=1.00 bar Express the temperature in kelvins to three significant figures. ανα ΑΣφ K Submit Request Answer Part B Calculate the final temperature if the same gas undergoes an adiabatic expansion against an external pressure of P= 1.00 bar to a final pressure P=1.00 bar. Express the temperature in kelvins to three significant figures. K Submit Request Answer

University Physics Volume 2

18th Edition

ISBN:9781938168161

Author:OpenStax

Publisher:OpenStax

Chapter3: The First Law Of Thermodynamics

Section: Chapter Questions

Problem 93CP: An insulated vessel contains 1.5 moles of argon at 2 atm. The gas initially occupies a volume of 5...

See similar textbooks

Similar questions

An ideal gas initially at 300 K undergoes an isobaric expansion at 2.50 kPa. If the volume increases from 1.00 m3 to 3.00 m3 and 12.5 kJ is transferred to the gas by heat, what are (a) the change in its internal energy and (b) its final temperature?
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
A 2.00-mol sample of a diatomic ideal gas expands slowly and adiabatically from a pressure of 5.00 atm and a volume of 12.0 L to a final volume of 30.0 L. (a) What is the final pressure of the gas? (b) What are the initial and final temperatures? Find (c) Q, (d) Eint, and (e) W for the gas during this process.
Figure P21.45 shows a cyclic process ABCDA for 1.00 mol of an ideal gas. The gas is initially at Pi = 1.50 105 Pa, Vi = 1.00 103 m3 (point A in Fig. P21.45). a. What is the net work done on the gas during the cycle? b. What is the net amount of energy added by heat to this gas during the cycle? FIGURE P21.45
The arrow OA in the PV diagram shown in Figure OQ22.11 represents a reversible adiabatic expansion of an ideal gas. The same sample of gas, starting from the same state O. now undergoes an adiabatic free expansion to the same final volume. What point on the diagram could represent the final state of the gas? (a) the same point A as for the reversible expansion (b) point B (c) point C (d) any of those choices (e) none of those choices
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.
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?
One mole of an ideal gas does 3 000 J of work on its surroundings as it expands isothermally to a final pressure of 1.00 atm and volume of 25.0 L. Determine (a) the initial volume and (b) the temperature of the gas.
For a temperature increase of 10 at constant volume, what is the heat absorbed by (a) 3.0 mol of a dilute monatomic gas; (b) 0.50 mol of a dilute diatomic gas; and (c) 15 mol of a dilute polyatomic gas?
A gas in a cylindrical closed container is adiabatically and quasi-statically expanded from a state A (3 MPa, 2 L) to a state B with volume of 6 L along the path 1.8pV= constant. (a) Plot the path in the pV plane. (b) Find the amount of work done by the gas and the change in the internal energy of the gas during the process.