An ideal diatomic gas has an initial pressure of 1.00×10°Pa , an initial volume of 2.00m', andan initial temperature of 300K. (This is point 1 on the pV-diagram.) The gas has an isochoricincrease in pressure to 2.00×10°P. . (This is point 2 on the pV-diagram.) The gas then has anisothermal expansion to a volume of 3.00m'. (This is point 3 on the pV-diagram.) The pressureis then reduced adiabatically back down to its original pressure of 1.00×10°P.. (This is point 4on the pV-diagram.) Finally, the gas has an isobaric decrease in volume to its original volume of2.00m. (The gas is back to point 1 on the pV-diagram.)а.Fill in the missing values on the following table.PointVolume,Pressure,Temperature,v (m²)p(10ʻPA)T(K)12.001.0030022.0033.0041.00b. Fill in the values for each of the processes in the following table. (These valuescorrespond to the First Law of Thermodynamics written as: AE, =W +Q.)ProcessChange in internalWork done to gas,Heat added to gas,energy, AE, (J)W (3)Q(1)'th1→ 22 → 33 → 44 →1Full Cycle

Iso choric process is the process where the system volume remain constant during the process. Iso…

Answered: An ideal diatomic gas has an initial…

Principles of Physics: A Calculus-Based Text

5th Edition

ISBN:9781133104261

Author:Raymond A. Serway, John W. Jewett

Publisher:Raymond A. Serway, John W. Jewett

Chapter17: Energy In Thermal Processes: The First Law Of Thermodynamics

Section: Chapter Questions

Problem 47P

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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?
Two moles of a monatomic ideal gas at (5 MPa, 5 L) is expanded isothermally until the volume is doubled (step 1). Then it is cooled isochorically until the pressure is 1 MPa (step 2). The temperature drops in this process. The gas is now compressed isothermally until its volume is back to 5 L, but its pressure is now 2 MPa (step 3). Finally, the gas is heated isochorically to return to the initial state (step 4). (a) Draw the four pi-cresses in the pV plane. (b) Find the total work done by the gas.
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
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?
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?
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. `
As shown below, calculate the work done by the gas in the quasi-static processes represented by the paths (a) AB; (b) ADB; (c) ACB; and (d) ADCB. `
One of a dilute diatomic gas occupying a volume of 10.00 L expands against a constant pressure of 2.000 atm when it is slowly heated. If the temperature of the gas rises by 10.00 K and 400.0 J of heat are added in the process, what is its final volume?
A monatomic ideal gas undergoes a quasi-static adiabatic expansion in which its volume is doubled. How is the pressure of the gas changed?
What is the internal energy of 6.00 mol of an ideal monatomic gas at 200 ?
Two moles of a monatomic ideal gas such as oxygen is compressed adiabatically and reversibly from a state (3 atm, 5 L) to a state with a pressure of 4 atm. (a) Find the volume and temperature of the final state. (b) Find the temperature of the initial state. (c) Find work done by the gas in the process. (d) Find the change in internal energy in the process. Assume Cv=5R and Cp=Cv+R for the diatomic ideal gas in the conditions given.
Suppose 1.00x10^2 moles of monatomic ideal gas undergoes an isothermal expansion as shown (vertical: Pressure, kPa and horizontal: Volume, m^3). The horizontal axis is marked in increments of 30m^3 and the vertical axis is marked in increments of 100kPa. How much work is down by the gas from A to B?

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