9. Derive the equation dH = TDS + VdP and show tha ASm = Cp.m In 2 - R In For the change of one mole of an ideal gas from Tu, P, to T2, P, assuming that Cp,m is independent of temperature. (Hint: Start from dU = Tds - pdV and consider what you need to add to both sides to get an expression for dH on the left side).
a) Show that for an ideal gas ΔŠ,-Ásv + R In b) The isochoric heat capacity of ethene gas can be expressed by 6085.929K 822826 K2 Су/R =16.4105-00 T2 over the temperature range from 300 K to 1000 K. Calculate ASv when 1 mole of ethene gas is heated from 300 K to 600 K at constant volume. c) Calculate ASp when 1 mole of ethene gas is heated from 300 K to 600 K at constant pressure. What is...
2. The enthalpy change dh of an incompressible substance is given by: (5 pts) a. du + pdv b. du + vdp d. du RdT 3. The temperature of an ideal gas undergoing an adiabatic expansion through a throttling valve (S a. increases c. remains constant b. decreases d. cannot be determined 4. A device which decreases the pressure and increases the velocity is a (5 pts) a. fan c. diffuser b. mixing heat exchanger d. nozzle
3 1. One mole of an ideal gas expands isothermally at T = 20°C from 1.2 m² to 1.8 m². The gas constant is given by R= 8.314 J/mol K). (a) Calculate the work done by the gas during the isothermal expansion. W= (b) Calculate the heat transfered during the expansion Q= (c) What is the change in entropy of the gas? AS аук (c) What is the entropy change of the thermal reservoir? AS reservar JK (d) What is...
5. (30 pts) In a steady-state flow process carried out at atmosphere pressure, 2 mol/s of air at 600K is continuously mixed with 3 mol/s of air at 450 K. The product stream is at 400 K and at 1 atm. Assume the ideal-gas state for air with Cp=7/2 R, and that kinetic and potential-energy changes of the streams are negligible, and the surroundings are at 300 K. a) What is the rate of heat transfer? b) What is the...
I thought when A has 2 mol and B has 1mol
mole fraction would be 2/3 for A and 1/3 for B
then the result is
delta S = -R (3N)*((2/3)ln(2/3) + (1/3)ln(1/3))
(and this was actually the answer of (4)!)
but the result is 3Rln(2).
Where am i wrong?
what is the difference between microstates in
2mol A 1mol B
and
2mol A 1mol A ?
1A rigid container is divided into two compartments of equal volume by a...
(1) A process has been proposed whereby an ideal gas is taken from P=10 bar and T=300 K to P=1 bar and T=500K in a closed system. During the process the system performs 1,000 [J] of work and receives 6,430 [j] of heat from the surroundings at a constant temperature of 300 K. The constant pressure heat capacity of the gas Cp=30 [J/(mol K)]. Gas constant R=8.314 [J/(mol K)]. (a) (7 pts.) What is the change of molar internal energy...
(1) A process has been proposed whereby an ideal gas is taken from P=10 bar and T=300 K to P=1 bar and T=500K in a closed system. During the process the system performs 1,000 [j] of work and receives 6,430 [J] of heat from the surroundings at a constant temperature of 300 K. The constant pressure heat capacity of the gas cp=30 [J/mol K)]. Gas constant. R=8.314 [J/(mol K)]. (a) (7 pts.) What is the change of molar internal energy...
10. Given the following table: Compound NO: (g) N:O (g) AHP (J mol) AGP (J mol) 51.84 33.85 9.66 98.29 For the reaction: N:Oa (g) eo 2NO: (g) (a) Use the information in the Table to calculate AG for the reaction (b) Use the information in the Table to calculate AH" for the reaction (c) Calculate K, at 25 C. (d) Calculate K, at 1600 °C. (Assume AH to be temperature independent) (e) Calculate the degree of dissociation, a, of...
Show all steps Chapter 3, Problem 36P ON (1 Bookmark Problem One cubic meter of argon is taken from 1 bar and 25°C to 10 bar and 300'C by each of the following two-step paths. For each path, compute o. w AU, and AH for each step and for the overall process Assume mechanical reversibility and treat argon as an ideal gas with Cp (5/2) Rand Cv (3/2)R (a) Isothermal compression followed by isobaric heating (b) Adiabatic compression followed by...