An ideal gas sample containing 2.50 mol for which Cv,m =3/2R undergoes the followin reversible cyclical process from an initial state characterized by T = 450 K and P = 1.00 bar: a) It is expanded reversibly and adiabatically until the volume doubles. b) It is reversibly heated at constant volume until T increases to 450 K. c) The pressure is increased in an isothermal reversible compression until P = 1.00 bar. Calculate q, w, AU, AH, AS, ASsurroundings, and AStotal for each step in the cycle, and for the total cycle. The temperature of the surroundings is 300 K.

An ideal gas sample containing 2.50 mol for which Cv,m =3/2R undergoes the followin reversible cyclical process from an initial state characterized by T = 450 K and P = 1.00 bar: a) It is expanded reversibly and adiabatically until the volume doubles. b) It is reversibly heated at constant volume until T increases to 450 K. c) The pressure is increased in an isothermal reversible compression until P = 1.00 bar. Calculate q, w, AU, AH, AS, ASsurroundings, and AStotal for each step in the cycle, and for the total cycle. The temperature of the surroundings is 300 K.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

One mole of a perfect monatomic gas, initially at 300 K and a pressure 15.0 atm, expands to afinal pressure of 1.00 atm. Consider the expansion via each of the following paths: (a)isothermal and reversible, (b) isothermal and irreversible, (c) adiabatic and reversible, (d)adiabatic and irreversible. In these irreversible processes, the expansion occurs against anexternal pressure of 1.00 atm. For each case, calculate the values of q, w, ΔU and ΔH.
Calculate the change in the entropies of the system and the surroundings, when 1 mole of an ideal gas at 298 K and 1.00 bar is compressed against Pex = 2 bar isothermally until it reaches equilibrium. And Prove this process is irreversible.
A sample of 1.00 mol perfect gas molecules with Cp,m = 7/2R and at 298 K and 1.00 atm is put through the following cycle: (a) Constant volume heating to twice its initial pressure, (b) Reversible, adiabatic expansion back to its initial temperature, (c) reversible isothermal compression back to 1.00 atm. Calculate q, w, ΔU, and ΔH for each step and overall (assume the initial temp is 298 K). Please answer very soon will give rating surely All questions answers needed Please answer complete questions
1 mole of an ideal gas with CV,m = 5/2 R undergoes transformation either (I) or (II) from aninitial temperature (Ti) = 250 K and initial pressure (Pi) = 1.00 bar. CV,m denotes molar heatcapacity at constant volume.(I) 1 mol of gas undergoes a reversible adiabatic expansion until the final pressure (Pf) ishalf of its initial value. The surroundings are at 250 K and 0.500 bar.(II) 1 mol of gas undergoes an adiabatic expansion against a constant external pressure(Pex) of 0.500 bar until the final pressure (Pf) is equal to half of its initial value. Thesurroundings are at 300 K and 0.500 bar.a) Calculate the change in entropy of the system (ΔSsys) (in unit J K-1 ) for each (I) and (II). b) Calculate the change in entropy of the surroundings (ΔSsur) (in unit J K-1 ) for each (I) and (II). c) Calculate the total change in entropy (ΔStot) (in unit J K-1 ) for each (I) and (II). d) State which of the process [(I) or (II)] is a spontaneous process.
. A 2.50 mole sample of a perfect gas for which Cv,m = 3R/2 (assume constant over T-range) undergoes the following two-step process: (1) from an initial state of the gas described by T = 13 ºC and P = 1.75 x 105 Pa, the gas undergoes an isothermal expansion against a constant pressure of 3.75 x 104 Pa until the volume has doubled. (2) subsequently, the gas is cooled at constant volume. The temperature falls to -24ºC. Calculate q, w, ∆U, and ∆H for each step and for the overall process.
3 m of an ideal gas expands from 400K and 4 bar to 1 bar final pressure. a) The situation where the expansion is isothermal and reversible b) Explain which work is bigger and why by finding the work values for the case where the expansion is adiabatic and reversible. Cv, m = 3 / 2R
2.00-mol NH3 (g) was initially at 298 K, and is now under reversible adiabatic expansion from 1.00 dm3 to 4.00 dm3. Assume ideal gas behavior and the molar heat capacity of NH3 (g) at constant volume CV,m = 3R where R is the gas constant. (a)Calculate the final temperature (in K) (b)Determine the amount of work done including the correct sign for this process (in Joule or kJ).
3 m of an ideal gas expands from 400K and 4 bar to 1 bar final pressure. a) The situation where the expansion is isothermal and reversible b) Explain which job is bigger and why by finding the job values for the case where the enlargement is adiabatic and reversible. Cv, m = 3 / 2R
The soft container contains 5.00 moles of gaseous Ar having the temperature 0.00° C and pressure of 2.00 atm has been placed into thermal contact with the environment having temperature 25.00°C and pressure 1atm. What is the change of the Gibbs free energy (final minus initial) after equilibration. Express the answer in kJ. Consider Ar as an ideal gas and use a classical expression for its specific heat...
Determine the work involved when one mole of an ideal gas is compressed isothermally from 1.00 bar to 5.00 bar at a constant pressure of 300K
A 2.50 mol sample of ideal gas with CV, m = 3 / 2R, T = 450 K and P = 1.00 bar startpasses the following reversible cycle process from the state:a) Reversibly doubling its volume adiabaticallyb) Reversibly fixed volume T temperature is heated up to 450 K.c) By increasing the pressure, it is isothermally compressed reversibly until P = 1.00 bar.Calculate the sum of q, w, ΔU, ΔH, ΔS, ΔSphere, and ΔS for each stage and total cycle.calculate. Consider the environmental temperature as 300 K.
A mole of a diatomic gas at 0.1 m³ is expanded isothermally at 298 Kelvins to 1.0 m³ bar against a constant external pressure of 0.5 bar. Which of the following statements is true? A. q=w B. q= -w C. ∆H= ∆U D. ∆H> ∆U