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**ITK-233 Termodinamika Teknik Kimia I**

3 sks 2 - PVT Behavior of Fluid, Equation of State Dicky Dermawan

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**P – T Diagram P – v Diagram**

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T-v Diagram

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Equation of State For the regions of the diagram where a single phase exist: This means an equation of state exist relating P, V, T. An EOS may be solved for any one of the three quantities as a function of the other two, viz.: V = V(T,P) Volume expansivity: Isothermal compressibility:

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Example For liquid acetone at 20oC & 1 bar: Β = x 10-3 oC-1 κ = 62 x x 10-6 bar-1 V= cm3 g-1 For aceton, find: a. The value of b. The pressure generated by heating at constant V from 20oC & 1 bar to 30oC c. The change in volume for a change from 20oC & 1 bar to 0oC & 10 bar.

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Problem 3.1 Express the volume expansivity β and isothermal compressibility κ as functions of density ρ and its partial derivatives. The isothermal compressibility coefficient () of water at 50oC and 1 bar is x 10-6 bar-1. To what pressure must water be compressed at 50oC to change its density by 1%? Assume that is independent of P.

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Problem 3.2 & 3.3 Generally, volume expansivity β and isothermal compressibility κ depend on T and P. Prove that The Tait equation for liquids is written for an isotherm as: where V is specific or molar volume, Vo is the hypothetical molar or specific volume at P = 0 and A & B are positive constant. Find an expression for the isothermal compressibility consistent with this equation.

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Problem 3.4 For liquid water the isothermal compressibility is given by: where c & b are functions of temperature only. If 1 kg of water is compressed isothermally & reversibly from 1 bar to 500 bar at 60oC, how much work is required? At 60oC, b=2700 bar and c = cm3 g-1

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Problem 3.5 Calculate the reversible work done in compressing 1 ft3 of mercury at a constant temperature of 32oF from 1 atm to 3000 atm. The isothermal compressibility of mercury at 32oF is: κ/atm-1 = 3.9 x 10-6 – 0.1 x 10-9 P (atm)

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Problem 3.6 Five kilograms of liquid carbon tetrachloride undergo a mechanically reversible, isobaric change of state at 1 bar during which the temperature change from 0oC to 20oC. Determine ΔVt, W, Q, and ΔUt The properties for liquid carbon tetrachloride at 1 bar & ooC may be assumed independent of temperature: β = 1.2 x 10-3 K-1 Cp = 0.84 kJ kg-1 K-1 ρ = 1590 kg m-3

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Problem 3.7 A substance for which κ is a constant undergo a mechanically reversible process from initial state (P1,V1) to final state (P2,V2), where V is molar volume. Starting with the definition of κ, show that the path of the process is described by Determine an exact expression which gives the isothermal work done on 1 mol of this constant-κ substance

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P – v Diagram

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Virial EOS & Ideal Gas Virial expansion: Alternative form: Compressibility factor For ideal gas: Z = 1, thus

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The Ideal Gas The internal energy of a real gas is a function of pressure and temperature. This pressure dependency is the result of forces between the molecules. In an ideal gas, such forces does not exist. No energy would be required to alter the average intermolecular distance, and therefore no energy would be required to bring about volume & pressure changes in an ideal gas at constant temperature. In other word, the internal energy of an ideal gas is a function of temperature only.

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**Implied Property Relations for an Ideal Gas**

Thus H is also a funcion of temperature only

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**Isothermal Process Closed System, Ideal Gas, Mechanically Reversible**

PV = constant

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**Isobaric Process Closed System, Ideal Gas, Mechanically Reversible**

TV-1 = constant

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**Isochoric (Constant V) Process Closed System, Ideal Gas, Mechanically Reversible**

TP-1 = constant

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**Adiabatic Process Closed System, Ideal Gas, Mechanically Reversible**

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**Polytropic Process Closed System, Ideal Gas, Mechanically Reversible**

Polytropic process can be considered as general form of process. Isobaric process : δ = 0 Isothermal process : δ = 1 Adiabatic process : δ = γ Isochoric process : δ = ∞

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Example 3.2 Air is compressed from an initial condition of 1 bar & 25oC to a final state of 5 bar & 25oC by three different mechanically reversible processes in a closed system: Heating at constant volume followed by cooling at constant pressure Isothermal compression Adiabatic compression followed by cooling at constant volume. Assume air to be an ideal gas with the constant heat capacities: CV = 5/2 R, CP = 7/2 R. Sketch the process in a PV diagram & calculate the work required, heat transferred, and the changes in internal energy & entalphy of the air for each processes

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Example 3.3 An ideal gas undergoes the following sequence of mechanically reversible processes in a closed system: From an initial state of 70oC & 1 bar, it is compressed adiabatically to 150oC It is then cooled from 150oC to 70oC at constant pressure Finally, it is expanded isothermally to its original state Sketch the process in a PV diagram & calculate W, Q, DU, and DH for each of the three processes and for the entire cycle. Take CV = 3/2 R and CP = 5/2R

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**Problem 3.8 Constant volume Contant temperature Adiabatically**

One mole of an ideal gas with CV = 5/2 R, CP = 7/2 R expands from P1 = 8 bar & T1 = 600 K to P2 = 1 bar by each of the following path: Constant volume Contant temperature Adiabatically Assuming mechanical reversibility, calculate W, Q, DU, and DH for each of the three processes. Sketch each path in a single PV diagram

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Problem 3.9 An ideal gas initially at 600 K & 10 bar undergoes a four-step mechanically reversible cycle in a closed system. In step 1-2 pressure decreases isothermally to 3 bar; in step 2-3 pressure decreases at constant volume to 2 bar; in step 3-4 volume decreases at constant pressure; and in step 4-1 the gas returns adiabatically to its initial step. Sketch the cycle on a PV diagram Determine (where unknown) both T & P for states 1, 2, 3, and 4 Calculate W, Q, DU, and DH for each step of the cycle Data: CV = 5/2 R, CP = 7/2 R

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Problem 3.10 An ideal gas, CV = 3/2 R & CP = 5/2 R is changed from P1 = 1 bar & Vt1 = 12 m3 to P2 = 12 bar & Vt2 = 1 m3 by the following mechanically reversible processes: Isothermal compression Adiabatic compression followed by cooling at constant pressure Adiabatic compression followed by cooling at constant volume Heating at constant volume followed by cooling at constant pressure Cooling at constant pressure followed by heating at constant volume Calculate W, Q, DUt, and DHt for each of these processes, and sketch the paths of all processes on a single PV diagram

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Example 3.4 A 400 gram mass of nitrogen at 27oC is held in a vertical cylinder by a frictionless piston. The weight of the piston makes the pressure of the nitrogen 0.35 bar higher than that of the surroundings atmosphere, which is at 1 bar & 27oC. Thus the nitrogen is initially at a pressure of 1.35 bar, and is in mechanical & thermal equilibrium with its surroundings. Consider the following sequence of process: The apparatus is immersed in an ice/water bath and is allowed to come to equilibrium A variable force is slowly applied to the piston so that the nitrogen is compressed reversibly at the constant temperature of 0oC until the gas volume reaches one-half the value at the end of step a. At this point the piston is held in place by latches.

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Example 3.4 (cont’) The apparatus is removed from ice/water bath and comes to thermal equilibrium with the surrounding atmosphere at 27oC The latches are removed, and the apparatus is allowed to return to complete equilibrium with its surroundings Sketch the entire cycle on a PV diagram, and calculate Q, W, DU & DH for the nitrogen for each step of the cycle. Nitrogen may be considered an ideal gas for which CV = 5/2 R and CP = 7/2 R

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**Cubic Equation of State: van der Waals Equation (1873)**

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**Theorem of Corresponding State; Accentric Factor**

All fluids, when compared at the same reduced temperature & reduced pressure, have approximately the same compressibility factor, and all deviate from ideal gas behavior to about the sam degree Accentric Factor (Pitzer)

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**Critical Constants & Accentric Factors: Paraffins**

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**Critical Constants & Accentric Factors: Olefin & Miscellaneous Organics**

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**Critical Constants & Accentric Factors: Miscellaneous Organic Compounds**

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**Critical Constants & Accentric Factors: Elementary Gases**

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**Critical Constants & Accentric Factors: Miscellaneous Inorganic Compounds**

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**Cubic Equation of State: Redlich/Kwong Equation (1949)**

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**Cubic Equation of State: Soave/Redlich/Kwong Equation (1972)**

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**Cubic Equation of State: Peng - Robinson Equation (1976)**

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Example 3.8 Given that the vapor pressure of n-butane at 350 K & bar, find the molar volumes of saturated vapor and saturated liquid n-butane at these conditions as given by: Van der Waals Redlich/Kwong Soave/Redlich/Kwong Peng-Robinson

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**Application of The Virial Equations**

At low to moderate pressure, it is common to use truncated virial equation: At pressure above the range of applicability of the above eqn, the appropriate form is: Benedict/Webb/Rubin equation: and its modifications are inspired by volume expansion virial eqn and are used in the petroleum & natural gas industries for light hydrocarbons.

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Example 3.7 Reported values for the virial coefficients of isopropanol vapor at 200oC are: B = -388 cm3 mol C = cm6 mol-2 Calculate V and Z for isopropanol at 200oC & 10 bar by: The ideal gas equation Two term truncated pressure expansion virial equation Three term truncated volume expansion virial equation

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**Pitzer Correlation for the Second Virial Coefficient**

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**Generalized Correlations 4 Gases: Pitzer type: Lee -Kessler**

Tr Z0 Pr

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**Generalized Correlations 4 Gases: Pitzer type: Lee -Kessler**

Tr Z0 Pr

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**Generalized Correlations 4 Gases: Pitzer type: Lee -Kessler**

Tr Z1 Pr

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**Generalized Correlations 4 Gases: Pitzer type: Lee -Kessler**

Tr Z1 Pr

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Real Gas, EOS Calculate Z and V for steam at 250oC and 1,800 kPa by the following: a. Ideal gas equation b. Truncated virial equation with the following experimental values of virial coefficient: B = cm3 mol-1 C = -5,800 cm6 mol-2 c. Pitzer correlation for virial equation d. Pitzer-type correlation of Lee – Kessler e. Steam table f. van der Waals equation g. Redlich/Kwong equation h. Soave/Redlich/Kwong equation i. Peng-Robinson Equation

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**Correlation for Liquids: Rackett Equation**

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**Correlation for Liquids: Lydersen, Greenkorn & Hougen**

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Problem 3.45 A 30 m3 tank contains 14 m3 of liquid n-butane in equilibrium with its vapor at 25oC. Estimate the total mass of n-butane in the tank. The vapor pressure if n-butane at the given temperature is 2.43 bar.

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Ideal Gas A cylinder pressure vessel having an inside diameter of 50 cm and height of 1.25 cm. Amount of the ammonia gas is confined in that a pressure vessel. Measured pressure and temperature of gas are 30 bars and 200oC. What are the specific volume and amount of the ammonia gas in pressure vessel (in SI unit), assuming ammonia is an ideal gas?

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Real Gas, EOS Calculate Z and for steam at 250oC and 1,800 kPa by the following: The ideal gas equation The truncated virial equation with the following experimental values of virial coefficient: B = cm3 mol-1 C = -5,800 cm6mol-2 The van der Waals equation The Redlich/Kwong equation The steam table Data: critical point of steam, TC = K; PC = bar; = 55.9 cm3mol-1

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1st law after diagram 1 kmole of ideal gas (Cv = 3R/2) undergoes a three-step mechanically reversible cycle in a closed system. Gas in initial state at 500 kPa and 27 oC is heated at constant pressure Followed by adiabatic expansion until the its pressure become 120 kPa Finally step, gas is isothermally compressed to initial condition From that process description: Illustrate the cycle process at P-V diagram in T parameter! b. Calculate H, U, Q and W for each step of process and total!

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Thermodynamics Internal energy of a system can be increased either by adding energy to the system or by doing work on the system Remember internal energy.

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