(d) A quantity of n = 2.0 mol of an ideal gas with Cv,m = 20.8 J K¹ mol¹ is initially atp = 330 kPa and T = 310 K. It undergoes reversible adiabatic expansion until thepressure reaches 250 kPa. Calculate (i) the final volume, (ii) the final temperatureand (iii) the work done in the process.

Answered: Image /qna-images/answer/086e0e94-e9b2-4685-8088-07f3e5dc04db.jpg

Answered: (d) A quantity of n = 2.0 mol of an…

Physical Chemistry

2nd Edition

ISBN:9781133958437

Author:Ball, David W. (david Warren), BAER, Tomas

Publisher:Ball, David W. (david Warren), BAER, Tomas

Chapter2: The First Law Of Thermodynamics

Section: Chapter Questions

Problem 2.58E: What is the finaltemperature of0.122 mole ofmonatomic ideal gas that performs 75J of work...

See similar textbooks

Similar questions

What are the numerical values of the heat capacities c-v and c-p of a monatomic ideal gas,in units of cal/mol.K and L.atm/mol.K?
The Dieterici equation of state for one mole of gas is p=RTe-aVRTV-b Where a and b are constants determined experimentally. For NH3g, a = 10.91 atm. L2 and b = 0.0401 L. Plot the pressure of the gas as the volume of 1.00 mol of NH3g expands from 22.4 L to 50.0 L at 273 K, and numerically determine the work done by the gas by measuring the area under the curve.
Calculate the work for the isothermal, reversible compressionof 0.245 moleof an idealgas going from 1.000L to 1.00 mL if the temperature were 95.0C.
A 220-ft3 sample of gas at standard temperature and pressure is compressed into a cylinder, where it exerts pressure of 2000 psi. Calculate the work (in J) performed when this gas expands isothermally against an opposing pressure of 1.0 atm. (The amount of work that can be done is equivalent to the destructive force of about 1/4 lb of dynamite, giving you an idea of how potentially destructive compressed gas cylinders can be if improperly handled!)
Benzoic acid, C6H5COOH, is a common standard used in bomb calorimeters, which maintain a constant volume. If 1.20 g of benzoic acid gives off 31, 723 J of energy when burned in the presence of excess oxygen and in a water bath having a temperature of 24.6 C, calculate q, w, H, and U for the reaction.
Determine an expression for V/T p, n in terms of and . Does the sign on the expression make sense in terms of what you know happens to volume as temperature changes?
Many compressed gases come in large,heavy metal cylindersthat are so heavy that they need a special cart to move them around. An80.0-Ltank ofnitrogen gas pressurized to 172 atm is left in the sun and heats from its normal temperature of 20.0C to 140.0C. Determine a the final pressureinsidethe tank and b the work, heat, and U of the process. Assume that behavior is ideal and the heatcapacity of diatomic nitrogenis 21.0J/mol.K.
A 1.00 mol sample of H2 is carefully warmed from 22 K to 40 K at constant volume. a What is the expected heat capacity of the hydrogen? b What is q for the process?
A 1.65 mole sample of an ideal gas for which Cv, m = 3/2 R undergoes the following two-step process: (a) From an initial state of the gas described by T = 14.5 oC and P = 2x104 Pa, the gas undergoes isothermal expansion against a constant external pressure of 1.0x104 Pa until the volume has doubled. (b) Then the gas is cooled to constant volume. The temperature drops to -35.6 oC. Calculate q, w, ΔH, ΔU for each step and for the overall process.
A sample consisting of 0.10 mol of perfect gas molecules is held by a piston inside a cylinder such that the volume is 1.25 dm3; the external pressure is constant at 1.00 bar and the temperature is maintained at 300 K by a thermostat. The piston is released so that the gas can expand. Calculate (a) the volume of the gas when the expansion is complete; (b) the work done when the gas expands; (c) the heat absorbed by the system. Hence calculate ΔStot.
Suppose 2.00 mol of an ideal, monatomic gas is initially at a pressure of 3.00 atm and a temperature T = 350 K. It is expanded irreversibly and adiabatically (q = 0) against a constant external pressure of 1.00 atm until the volume has doubled. (a) Calculate the final volume. (b) Calculate w, q, and AU for this process, in joules. (c) Calculate the final temperature of the gas.
(c) An ideal monoatomic gas at 1 bar and 300 K is expanded adiabatically against a constant pressure of 0.5 bar until the final pressure is 0.5 bar. Given that the Cy is 1.5R, calculate (i) (ii) heat per mole. work per mole.

SEE MORE QUESTIONS

Recommended textbooks for you

Physical Chemistry

Chemistry

ISBN:

9781133958437

Author:

Ball, David W. (david Warren), BAER, Tomas

Publisher:

Wadsworth Cengage Learning,

Principles of Modern Chemistry

Chemistry

ISBN:

9781305079113

Author:

David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:

Cengage Learning

Chemistry: Principles and Practice

Chemistry

ISBN:

9780534420123

Author:

Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:

Cengage Learning

Physical Chemistry

Chemistry

ISBN:

9781133958437

Author:

Ball, David W. (david Warren), BAER, Tomas

Publisher:

Wadsworth Cengage Learning,

Principles of Modern Chemistry

Chemistry

ISBN:

9781305079113

Author:

David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:

Cengage Learning

Chemistry: Principles and Practice

Chemistry

ISBN:

9780534420123

Author:

Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:

Cengage Learning

Living By Chemistry: First Edition Textbook

Chemistry

ISBN:

9781559539418

Author:

Angelica Stacy

Publisher:

MAC HIGHER

SEE MORE TEXTBOOKS

(d) A quantity of n = 2.0 mol of an ideal gas with Cv,m = 20.8 J K¹ mol¹ is initially at p = 330 kPa and T = 310 K. It undergoes reversible adiabatic expansion until the pressure reaches 250 kPa. Calculate (i) the final volume, (ii) the final temperature and (iii) the work done in the process.