One mole of an ideal gas initially at 300 K is expanded from 0.2 to 1.0 liter. Calculate AS for this change in state if it is carried out under the following conditions. Assume a constant volume heat capacity for the gas, CV, of 3 2 R. a. The expansion is reversible and isothermal. b. The expansion is irreversible and isothermal. c. The expansion is reversible and adiabatic (q = 0).

One mole of an ideal gas initially at 300 K is expanded from 0.2 to 1.0 liter. Calculate AS for this change in state if it is carried out under the following conditions. Assume a constant volume heat capacity for the gas, CV, of 3 2 R. a. The expansion is reversible and isothermal. b. The expansion is irreversible and isothermal. c. The expansion is reversible and adiabatic (q = 0).

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

4. A 1 mol sample of an ideal gas is expanded isothermally at 27 C from an initial pressure of 3 atm to a final pressure of 1 atm in 2 ways 1) reversibly and 2) against a constant external pressure of 1 atm. Calculate q, w, AU, AH, ASsys, ASsur and AStot in each case
The two processes that equivalent are for an ideal gas Isothermal reversible expansion and Adiabatic free expansion O Isothermal free expansion and Adiabatic free expansion O othermal reversible expansion and Adiabatic reversible expansion O Adiabatic free expansion and Adiabatic reversible expansion O
Suppose that one of water at its boiling point is kept in a cylinder that has frictionless piston. For equilibrium to be established, a pressure is maintained above the piston. If the piston sweeps out a volume of 0 dm3. Calculate the work done by the system for the following paths: Free expansion Reversible expansion against constant pressure of 4.0 atm Isothermal reversible expansion with initial volume = 0.80 dm3. When 2.0 mol of CO2 is heated at a constant pressure of 1.25 atm, its temperature increases from 280.00 K to 307.00 K. The heat (q) absorbed during this process is determined to be 2.0 kJ. Calculate (a) ΔH for this process (b) The molar heat capacity of CO2 at constant pressure (CP,m) (Hint: you can assume that CP,m is constant over this temperature range and that the CO2behaves ideally). (c) ΔU. Heat capacity of a material is temperature dependent. The T-dependence of the molar heat capacities of water (H2O(l)), H2(g) and O2(g) can be…
Suppose we're interested in studying ligaments. In class, we have focused on Problem 1 work done by changes in volume, but our initial framework presented accommodates other forms of work as well. When a ligament is stretched, we may represent the work done on the system as follows: dw fdl - pdV || Here, fis the restoring force of the ligament that opposes stretching, and /is the length. The differential expression for the Gibb's free energy can be written as follows: dG = Vdp – SdT + fdl differential expression. dA. a) Write all Maxwell relations from the Gibb's free energy energy, b) Derive the differential expression for Helmholtz free
3 moles of an ideal gas expand from 400 Kelvin and 4 bars to 1 bar final pressure.A) where the expansion is isothermal and reversibleb) explain why the work is larger by finding the work values for the situation where the expansion is Adiabatic and reversible. Cv,m = 3 / 2R
5. For an isothermal process, AS = а. q b. qrev/T С. Grev d. Tqrev e. q +w
A chemical reaction takes place in a container fitted with a piston of cross-sectional area 20cm2. As a result of the reaction, the gas undergoes a compression, the piston is displaced by 5cm (toward the bottom of the container), pushed by an external pressure of 105Pa. Calculate the work. a. +100 kJ b. -100 kJ c. -10 kJ d. +10 kJ
Each is false explain why
2.50 moles of an ideal gas with molar heat capacity at constant volume of 12.47 J/K-mol is expanded adiabatically against a constant external pressure of 1.00 atm. the initial temperature and pressure of the gas are 52 °C and 2.50 atm., respectively. The final pressure is 1.25 atm. For this expansion, calculate and enter answers below: a) Finals temperature (K) of the gas after the expansion b) q in joules c) w in joules d) AU in joules e) AH in joules
5 moles of monatomic ideal gas are conducted through the process shown in the PV diagram below. The system follows the path ABC. Curve BC represents an isothermal path.a) For the path ABC, determine whether the system absorbs or emits heat and calculate the magnitude of this heat.b) Calculate the change of internal energy and entropy of the gas in the path ABC.c) Calculate the entropy change of the gas in the process AB and BC. Explain in your own words wthat means the entropy change of the BC process using the definition of entropy in terms of the accessible microstates of the system.