One mole of an ideal, monoatomic gas initially at 300 K and 15.0 bar, expands to a final pressure of 1.00 bar. The expansion can occur via any of the following four paths: (a) isothermal and reversible (b) isothermal and irreversible (c) adiabatic and reversible (d) adiabatic and irreversible For irreversible processes, the expansion occurs against a constant external pressure of 1.00 bar. For each case calculate the values of q, w, AU, and AH.

One mole of an ideal, monoatomic gas initially at 300 K and 15.0 bar, expands to a final pressure of 1.00 bar. The expansion can occur via any of the following four paths: (a) isothermal and reversible (b) isothermal and irreversible (c) adiabatic and reversible (d) adiabatic and irreversible For irreversible processes, the expansion occurs against a constant external pressure of 1.00 bar. For each case calculate the values of q, w, AU, and AH.

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

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

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

Chapter12: Thermodynamic Processes And Thermochemistry

Section: Chapter Questions

Problem 18P

See similar textbooks

Similar questions

Show that = T/p for an ideal gas.
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.
It has been experimentally determined that the heat of combustion of benzene at constant volume is: ΔU ° rxn = -3265.6 kj, at 298K and the heat of combustion at constant pressure is: ΔH ° rxn = -3261.9 kj. C6H6 (l) + 15/2 O2 (g) → 6 CO2 (g) + 3 H2O (l) If we consider that substances in the gas phase behave as ideal gases, responding as appropriate: i) Does the system experience expansion or compression? justify mathematically.
Carbon dioxide gas with a mass of 88 g is isothermally compressed at a fixed external pressure of 15 bar, with a speed of 298 K and a final pressure of 10 bar from 1 bar. Interpret the results by finding the quantities Δu, Δh, w, Q, Δs, Δa, g and Δsaverage, Δssystem in the event.
It transmits 3 m of an ideal gas 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 expansion is adiabatic and reversible. Cv, m = 3 / 2R
One mole sample of an ideal, monoatomic gas initially has a molar volume of 24.45 L/mole at 1 bar and 298.2 K. It was expanded adiabatically and reversibly to 187.8K where the molar volume increased to 48.90 L/mole. How many KJ of work is involved in the process? Express answer in three significant figures
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...
One mole sample of an ideal, monoatomic as initially has a molar volume of 24.45 liters per mole at 1 bar and 298.2 Kelvins, It was expanded adiabatically and reversibly to 187.8 Kelvins where the molar volume increased to 48.90 liters per mole. How many KiloJoules of work is involved in the process. Express answer in three sig figs.
One mole of a monatomic ideal gas begins in a state withP 5 1.00 atm and T 5 300 K. It is expanded reversiblyand adiabatically until the volume has doubled; then it isexpanded irreversibly and isothermally into a vacuumuntil the volume has doubled again; and then it is heatedreversibly at constant volume to 400 K. Finally, it is compressed reversibly and isothermally until a inal state withP 5 1.00 atm and T 5 400 K is reached. Calculate DSsysfor this process. (Hint: There are two ways to solve thisproblem—an easy way and a hard way.)
How would an ideal gas (where dU=Cv(dt) is always true) undergoing isothermal reversible expansion be represented by the equation for the First Law? Think about what is changing in order to do work. Which term(s) is/are now zero?
Calculate ∆U and ∆H in heating 55.4 g of Xe from 300 K to 450 K. Assume the heat capacities atconstant volume and constant pressure to be independent of temperature and ideal gas behavior
What would be the final volume occupied by 1.0 mol of an ideal gas initially at 0°C and 1.0 bar if Q = 1000J during a reversible isothermal expansion?