(a) For propylene plot the residual enthalpy and residual entropy functions over the reduced pressure range of 0.5 ≤ Pr ≤ 20 for constant reduced temperatures of Tr = 0.5, 1.3, 2.1 and 2.9. Place all results on a single plot. Use (a.1) Redlich-Kwong equation (a.2) Soave-Redlich-Kwong equation (a.3) Peng-Robinson equation (b) Modify the output of part (a) to allow a direct comparison of your plots with generalized plot available in the literature

(a) For propylene plot the residual enthalpy and residual entropy functions over the reduced pressure range of 0.5 ≤ Pr ≤ 20 for constant reduced temperatures of Tr = 0.5, 1.3, 2.1 and 2.9. Place all results on a single plot. Use (a.1) Redlich-Kwong equation (a.2) Soave-Redlich-Kwong equation (a.3) Peng-Robinson equation (b) Modify the output of part (a) to allow a direct comparison of your plots with generalized plot available in the literature

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 2.46E: Define isobaric,isochoric, isenthalpic,and isothermal. Can achangein a gaseous system be isobaric,...

See similar textbooks

Similar questions

4.00 mol of perfect gas atoms with C p,m= 25 R is initially at 100.0 kPa, 100.0 dm3. It is heated to 150.0 dm3 at constant pressure and then heated to 150.0 kPa at constant volume. Calculate W, Q, ΔU and ΔH for this process.
12. Consider 0.1 mole of a monotomic ideal gas (system) which is initially equilibrated at a tem- perature of 500 K in a container with a volume 1 of 1 m³, and then undergoes a reversible norisothermal expansion to a volume of 2 m³. 200(a) What is the energy change of the gas (in J units)? Seemee axismo (b) How much work is exchanged in the above process (in J units)? emoldong slon Su for (c) What is the entropy change of the gas (in J/K units)? 36 or (d) What is the entropy change of the universe (in J/K units)? (319)
5. A sample consisting of 3 mol of ideal gas molecules with Cp.m = 20.8 J K-1 mol-1 is initially at 240 kPa and 325 K. It undergoes reversible adiabatic expansion until its pressure reaches 150 kPa. Calculate (i) the final volume and temperature, (ii) q, (iii) w, and (iv) AU.
gas are allowed to expand isothermally from 1.0 dm³ to 3.0 dm³ at 300 K. E3A.3(b) Calculate the change in entropy of the gas when 4.00 g of nitrogen is allowed to expand isothermally from 500 cm³ to 750 cm³ at 300 K. E3A.4(a) Calculate the change in the entropies of the system and the to though surroundings and the total chanc
A quantity of an ideal gas in an isolated system expanded V1 to V2 isothermally but irreversibly at 400 K and absorbed 100 J of heat. Calculate (a) the entropy change of the gas;(b) the entropy change of the reservoir, and(c) the entropy change of the whole system.Answer:a. 0.50b. -0.25c. 0
7:53 PM Mon Nov 21 8) A sample of 1 mol of perfect gas at 298 K and 1 bar with Cvm = 3/2 R and Cp.m= 5/2 R 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 bar. Calculate q, w, AU, and AH for each step, as well as any necessary variables (e.g. V₁, T, etc.) n=1 mol T= 298 K P= I bar Cum 3R - 2 Cp.m-2R T b) a) w=0 n=1 T= 298 K Cvm = 3R 2 AP= 1 bar 9,² AU= ΔΗ: PV = nRT V = nRT @87% 8
The Gibbs Function G is a thermodynamic property. If following relationship as Ꮩ . (ap)T = -(T)P p=-S and = V, prove the
For each system listed in the first column of the table below, decide (if possible) whether the change described in the second column will increase the entropy S of the system, decrease S, or leave S unchanged. If you don't have enough information to decide, check the "not enough information" button in the last column. Note for advanced students: you may assume ideal gas and ideal solution behaviour. System Change AS O AS 0 both at 2 atm and 7°C. not enough O Information AS 0 water and 250. mL of brine (very o not enough information salty water). O AS 0 not enough information 回因

For each system listed in the first column of the table below, decide (if possible) whether the change described in the second column will increase the entropy S of the system, decrease S, or leave S unchanged. If you don't have enough information to decide, check the "not enough information" button in the last column. Note for advanced students: you may assume ideal gas and ideal solution behaviour. System Change AS O AS 0 not enough information O As 0 at 19 °C. not enough information AS 0 carbon dioxide (CO,) gas at 3 atm pressure kept constant at 3 atm. and 16°C. not enough information Check Explanation O 2021 McGraw-Hill Education. All Rights Reserved. Terms of Use | Privacy Acc 60
One mole (1.0 mol) of an ideal gas is initially at T1 = 298 K and has volume V1 = 2.0 L. It is then reversibly expanded to final volume V2 = 3.0 L. Assume Cp = 5/2 R and Cv = 3/2R. a) Calculate the following if the expansion is isothermal: 1) ΔT 2) q 3) w 4) ΔU 5) ΔH b) Calculate ΔT–ΔU if the expansion is adiabatic instead of isothermal.c) Calculate the initial pressure and two final pressures for the process in a) & b).d) On a single set of axes, sketch a pressure–volume plot for each of the two processes in a) & b). Label the area that corresponds to the work for each process.
One mole of an ideal gas is reversibly compressed from 25 kPa to 105 kPa at aconstant temperature of 27 ℃. Calculate ?, ?, Δ?, Δ?, and Δ?.
1 THE SECOND LAW [6] Calculate the change in the entropies of the system and the surroundings, and the total change in entropy, when the volume of a sample of argon gas of mass 21 g at 298 K and 1.50 bar increases from 1.20 dm³ to 4.60 dm3 in (a) an isothermal reversible expansion (b) an isothermal irreversible expansion against pex = 0 (c) an adiabatic reversible expansion