Assume that no heat flows from the gas to the tank or through the tank walls

2. Assume that the tank weighs 400 kg, is perfectly insulated, has an initial tem-perature of 25°C, has a specific heat of 0.46 kJ·kg⁻¹·K⁻¹, and is heated by the gas so as always to be at the temperature of the gas in the tank.

3.10. Problems 121

3.10 121

3.26. Develop equations that may be solved to give the final temperature of the gas remaining in a tank after the tank has been bled from an initial pressure P1 to a final pressure P2. Known quantities are initial temperature, tank volume, heat capacity of the gas, total heat capacity of the containing tank, P1, and P2. Assume the tank to be always at the temperature of the gas remaining in the tank and the tank to be perfectly insulated.

3.27. A rigid, nonconducting tank with a volume of 4 m³ is divided into two unequal parts by a thin membrane. One side of the membrane, representing 1/3 of the tank, contains nitrogen gas at 6 bar and 100°C, and the other side, representing 2/3 of the tank, is evacuated. The membrane ruptures and the gas fills the tank.

(a) What is the final temperature of the gas? How much work is done? Is the process reversible?

(b) Describe a reversible process by which the gas can be returned to its initial state.

How much work is done?

Assume nitrogen is an ideal gas for which CP = (7/2)R and CV = (5/2)R.

3.28. An ideal gas, initially at 30°C and 100 kPa, undergoes the following cyclic processes in a closed system:

(a) In mechanically reversible processes, it is first compressed adiabatically to 500  kPa, then cooled at a constant pressure of 500 kPa to 30°C, and finally expanded isothermally to its original state.

(b) The cycle traverses exactly the same changes of state, but each step is irreversible with an efficiency of 80% compared with the corresponding mechanically revers-ible process. Note: The initial step can no longer be adiabatic.

Calculate Q, W, ΔU, and ΔH for each step of the process and for the cycle. Take CP = (7/2)R and CV = (5/2)R.

3.29. One cubic meter of an ideal gas at 600 K and 1000 kPa expands to five times its initial volume as follows:

(a) By a mechanically reversible, isothermal process.

(b) By a mechanically reversible, adiabatic process.

(c) By an adiabatic, irreversible process in which expansion is against a restraining pressure of 100 kPa.

For each case calculate the final temperature, pressure, and the work done by the gas.

Take CP = 21 J·mol⁻¹·K⁻¹.

3.30. One mole of air, initially at 150°C and 8 bar, undergoes the following mechanically reversible changes. It expands isothermally to a pressure such that when it is cooled at constant volume to 50°C its final pressure is 3 bar. Assuming air is an ideal gas for which CP = (7/2)R and CV = (5/2)R, calculate W, Q, ΔU, and ΔH.

3.31. An ideal gas flows through a horizontal tube at steady state. No heat is added and no shaft work is done. The cross-sectional area of the tube changes with length, and this causes the velocity to change. Derive an equation relating the temperature to the velocity of the gas. If nitrogen at 150°C flows past one section of the tube at a velocity of 2.5 m·s⁻¹, what is its temperature at another section where its velocity is 50 m·s⁻¹? Assume CP = (7/2)R.

3.32. One mole of an ideal gas, initially at 30°C and 1 bar, is changed to 130°C and 10 bar by three different mechanically reversible processes:

∙ The gas is first heated at constant volume until its temperature is 130°C; then it is compressed isothermally until its pressure is 10 bar.

∙ The gas is first heated at constant pressure until its temperature is 130°C; then it is compressed isothermally to 10 bar.

∙ The gas is first compressed isothermally to 10 bar; then it is heated at constant pressure to 130°C.

Calculate Q, W, ΔU, and ΔH in each case. Take CP = (7/2)R and CV = (5/2)R. Alter-natively, take CP = (5/2)R and CV = (3/2)R.

3.33. One mole of an ideal gas, initially at 30°C and 1 bar, undergoes the following mechan-ically reversible changes. It is compressed isothermally to a point such that when it is heated at constant volume to 120°C its final pressure is 12 bar. Calculate Q, W, ΔU, and ΔH for the process.

3.34. One mole of an ideal gas in a closed system, initially at 25°C and 10 bar, is first expanded adiabatically, then heated isochorically to reach a final state of 25°C and 1 bar. Assuming these processes are mechanically reversible, compute T and P after the adiabatic expansion, and compute Q, W, ΔU, and ΔH for each step and for the overall process. Take CP = (7/2)R and CV = (5/2)R.

3.35. A process consists of two steps: (1) One mole of air at T = 800 K and P = 4 bar is cooled at constant volume to T = 350 K. (2) The air is then heated at constant pressure until its temperature reaches 800 K. If this two-step process is replaced by a single isothermal expansion of the air from 800 K and 4 bar to some final pressure P, what is the value of P that makes the work of the two processes the same? Assume mechanical reversibility and treat air as an ideal gas with CP = (7/2)R and CV = (5/2)R.

3.36. 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 Q, W, ΔU, and ΔH for each step and for the overall process. Assume mechanical reversibility and treat argon as an ideal gas with CP = (5/2)R and CV = (3/2)R.

(a) Isothermal compression followed by isobaric heating.

(b) Adiabatic compression followed by isobaric heating or cooling.

(c) Adiabatic compression followed by isochoric heating or cooling.

(d) Adiabatic compression followed by isothermal compression or expansion.

3.10. Problems 123

3.10 123

3.37. A scheme for finding the internal volume V B^t of a gas cylinder consists of the following steps. The cylinder is filled with a gas to a low pressure P1, and connected through a small line and valve to an evacuated reference tank of known volume V A^t . The valve is opened, and gas flows through the line into the reference tank. After the system returns to its initial temperature, a sensitive pressure transducer provides a value for the pressure change ΔP in the cylinder. Determine the cylinder volume V B^t from the following data:

∙ V A^t = 256  cm ³

∙ ΔP / P 1 = −0.0639

3.38. A closed, nonconducting, horizontal cylinder is fitted with a nonconducting, friction-less, floating piston that divides the cylinder into Sections A and B. The two sections contain equal masses of air, initially at the same conditions, T1 = 300 K and P1 = 1(atm). An electrical heating element in Section A is activated, and the air temper-atures slowly increase: TA in Section A because of heat transfer, and TB in Section B because of adiabatic compression by the slowly moving piston. Treat air as an ideal gas with C P = ^_7₂ R , and let nA be the number of moles of air in Section A. For the pro-cess as described, evaluate one of the following sets of quantities:

(a) TA, TB, and Q/nA, if P(final) = 1.25(atm) (b) TB, Q/nA, and P (final), if TA = 425 K (c) TA, Q/nA, and P (final), if TB = 325 K (d) TA, TB, and P (final), if Q/nA = 3 kJ·mol⁻¹

3.39. One mole of an ideal gas with constant heat capacities undergoes an arbitrary mechan-ically reversible process. Show that:

ΔU = _{___}1 γ − 1 Δ ⁽ PV ⁾

3.40. Derive an equation for the work of mechanically reversible, isothermal compression of 1 mol of a gas from an initial pressure P1 to a final pressure P2 when the equation of state is the virial expansion [Eq. (3.33)] truncated to:

Z = 1 + B′P

How does the result compare with the corresponding equation for an ideal gas?

3.41. A certain gas is described by the equation of state:

PV = RT + ₍ b − _{_}θ

RT ₎ P

Here, b is a constant and θ is a function of T only. For this gas, determine expressions for the isothermal compressibility κ and the thermal pressure coefficient ( ∂ P / ∂ T ) V . These expressions should contain only T, P, θ, dθ/dT, and constants.

3.42. For methyl chloride at 100°C the second and third virial coefficients are:

B = −242.5  cm ³ ·mol ⁻¹ C = 25,200  cm ⁶ ·mol ⁻²

Calculate the work of mechanically reversible, isothermal compression of 1 mol of methyl chloride from 1 bar to 55 bar at 100°C. Base calculations on the following forms of the virial equation:

(a) Z = 1 + _{__}B

V + _{___}C V ²

(b) Z = 1 + B′P + C′ P ²

where B′ = _{___}B

RT and C′= _{_____}C − B ² ( RT ) ² Why don’t both equations give exactly the same result?

3.43. Any equation of state valid for gases in the zero-pressure limit implies a full set of virial coefficients. Show that the second and third virial coefficients implied by the generic cubic equation of state, Eq. (3.41), are:

B = b − _{____}a ⁽ T ⁾

RT C = b ² + _{________} ⁽ ε + σ ⁾ ba ⁽ T ⁾ RT

Specialize the result for B to the Redlich/Kwong equation of state, express it in reduced form, and compare it numerically with the generalized correlation for B for simple flu-ids, Eq. (3.61). Discuss what you find.

3.44. Calculate Z and V for ethylene at 25°C and 12 bar by the following equations:

(a) The truncated virial equation [Eq. (3.38)] with the following experimental values of virial coefficients:

B = −140  cm ³ ·mol ⁻¹ C = 7200  cm ⁶ ·mol ⁻²

(b) The truncated virial equation [Eq. (3.36)], with a value of B from the generalized Pitzer correlation [Eqs. (3.58)–(3.62)]

(c) The Redlich/Kwong equation (d) The Soave/Redlich/Kwong equation (e) The Peng/Robinson equation

3.45. Calculate Z and V for ethane at 50°C and 15 bar by the following equations:

(a) The truncated virial equation [Eq. (3.38)] with the following experimental values of virial coefficients:

B = −156.7   cm ³ ·mol ⁻¹ C = 9650   cm ⁶ ·mol ⁻²

(b) The truncated virial equation [Eq. (3.36)], with a value of B from the generalized Pitzer correlation [Eqs. (3.58)–(3.62)]

(c) The Redlich/Kwong equation

3.10. Problems 125

3.10 125

(d) The Soave/Redlich/Kwong equation (e) The Peng/Robinson equation

3.46. Calculate Z and V for sulfur hexafluoride at 75°C and 15 bar by the following equations:

(a) The truncated virial equation [Eq. (3.38)] with the following experimental values of virial coefficients:

B = −194  cm ³ ·mol ⁻¹ C = 15,300  cm ⁶ ·mol ⁻²

(b) The truncated virial equation [Eq. (3.36)], with a value of B from the generalized Pitzer correlation [Eqs. (3.58)–(3.62)]

(c) The Redlich/Kwong equation (d) The Soave/Redlich/Kwong equation (e) The Peng/Robinson equation

For sulfur hexafluoride, Tc = 318.7 K, Pc = 37.6 bar, Vc = 198 cm³·mol⁻¹, and ω = 0.286.

3.47. Calculate Z and V for ammonia at 320 K and 15 bar by the following equations:

(a) The truncated virial equation [Eq. (3.38)] with the following values of virial coefficients:

B = −208  cm ³ ·mol ⁻¹ C = 4378  cm ⁶ ·mol ⁻²

(b) The truncated virial equation [Eq. (3.36)], with a value of B from the generalized Pitzer correlation [Eqs. (3.58)–(3.62)]

(c) The Redlich/Kwong equation (d) The Soave/Redlich/Kwong equation (e) The Peng/Robinson equation

3.48. Calculate Z and V for boron trichloride at 300 K and 1.5 bar by the following equations:

(a) The truncated virial equation [Eq. (3.38)] with the following values of virial coefficients:

B = −724  cm ³ ·mol ⁻¹ C = −93,866  cm ⁶ ·mol ⁻²

(b) The truncated virial equation [Eq. (3.36)], with a value of B from the generalized Pitzer correlation [Eqs. (3.58)–(3.62)]

(c) The Redlich/Kwong equation (d) The Soave/Redlich/Kwong equation (e) The Peng/Robinson equation

For BCl3, Tc = 452 K, Pc = 38.7 bar, and ω = 0.086.

3.49. Calculate Z and V for nitrogen trifluoride at 300 K and 95 bar by the following equations:

(a) The truncated virial equation [Eq. (3.38)] with the following values of virial coefficients:

B = −83.5  cm ³ ·mol ⁻¹ C = −5592  cm ⁶ ·mol ⁻²

(b) The truncated virial equation [Eq. (3.36)], with a value of B from the generalized Pitzer correlation [Eqs. (3.58)–(3.62)]

(c) The Redlich/Kwong equation (d) The Soave/Redlich/Kwong equation (e) The Peng/Robinson equation

For NF3, Tc = 234 K, Pc = 44.6 bar, and ω = 0.126.

3.50. Determine Z and V for steam at 250°C and 1800 kPa by the following:

(a) The truncated virial equation [Eq. (3.38)] with the following experimental values of virial coefficients:

B = −152.5  cm ³ ·mol ⁻¹ C = −5800  cm ⁶ ·mol ⁻²

(b) The truncated virial equation [Eq. (3.36)], with a value of B from the generalized Pitzer correlation [Eqs. (3.58)–(3.62)].

(c) The steam tables (App. E).

3.51. With respect to the virial expansions, Eqs. (3.33) and (3.34), show that:

B′ = ( _{___}∂ Z

∂ P ) _T,P=0 and B = ( ∂ Z_{___}

∂ ρ ) _T,ρ=0 where ρ ≡ 1/V.

3.52. Equation (3.34) when truncated to four terms accurately represents the volumetric data for methane gas at 0°C with:

B = −53.4  cm ³ ·mol ⁻¹ C = 2620  cm ⁶ ·mol ⁻² D = 5000  cm ⁹ ·mol ⁻³

(a) Use these data to prepare a plot of Z vs. P for methane at 0°C from 0 to 200 bar.

(b) To what pressures do Eqs. (3.36) and (3.37) provide good approximations?

3.53. Calculate the molar volume of saturated liquid and the molar volume of saturated vapor by the Redlich/Kwong equation for one of the following and compare results with values found by suitable generalized correlations.

(a) Propane at 40°C where P^sat = 13.71 bar (b) Propane at 50°C where P^sat = 17.16 bar (c) Propane at 60°C where P^sat = 21.22 bar (d) Propane at 70°C where P^sat = 25.94 bar

3.10. Problems 127

3.10 127

(e) n-Butane at 100°C where P^sat = 15.41 bar (f ) n-Butane at 110°C where P^sat = 18.66 bar (g) n-Butane at 120°C where P^sat = 22.38 bar (h) n-Butane at 130°C where P^sat = 26.59 bar (i) Isobutane at 90°C where P^sat = 16.54 bar (j) Isobutane at 100°C where P^sat = 20.03 bar (k) Isobutane at 110°C where P^sat = 24.01 bar (l) Isobutane at 120°C where P^sat = 28.53 bar (m) Chlorine at 60°C where P^sat = 18.21 bar (n) Chlorine at 70°C where P^sat = 22.49 bar (o) Chlorine at 80°C where P^sat = 27.43 bar (p) Chlorine at 90°C where P^sat = 33.08 bar (q) Sulfur dioxide at 80°C where P^sat = 18.66 bar (r) Sulfur dioxide at 90°C where P^sat = 23.31 bar (s) Sulfur dioxide at 100°C where P^sat = 28.74 bar (t) Sulfur dioxide at 110°C where P^sat = 35.01 bar (u) Boron trichloride at 400 K where P^sat = 17.19 bar

For BCl3, Tc = 452 K, Pc = 38.7 bar, and ω = 0.086.

(v) Boron trichloride at 420 K where P^sat = 23.97 bar (w) Boron trichloride at 440 K where P^sat = 32.64 bar (x) Trimethylgallium at 430 K where P^sat = 13.09 bar

For Ga(CH3)3, Tc = 510 K, Pc = 40.4 bar, and ω = 0.205.

(y) Trimethylgallium at 450 K where P^sat = 18.27 bar (z) Trimethylgallium at 470 K where P^sat = 24.55 bar

3.54. Use the Soave/Redlich/Kwong equation to calculate the molar volumes of saturated liquid and saturated vapor for the substance and conditions given by one of the parts of Prob. 3.53 and compare results with values found by suitable generalized correlations.

3.55. Use the Peng/Robinson equation to calculate the molar volumes of saturated liquid and saturated vapor for the substance and conditions given by one of the parts of Prob. 3.53 and compare results with values found by suitable generalized correlations.

3.56. Estimate the following:

(a) The volume occupied by 18 kg of ethylene at 55°C and 35 bar.

(b) The mass of ethylene contained in a 0.25 m³ cylinder at 50°C and 115 bar.

3.57. The vapor-phase molar volume of a particular compound is reported as 23,000 cm³·mol^–1 at 300 K and 1 bar. No other data are available. Without assuming ideal-gas behavior, determine a reasonable estimate of the molar volume of the vapor at 300 K and 5 bar.

3.58. To a good approximation, what is the molar volume of ethanol vapor at 480°C and 6000 kPa? How does this result compare with the ideal-gas value?

3.59. A 0.35 m³ vessel is used to store liquid propane at its vapor pressure. Safety considerations dictate that at a temperature of 320 K the liquid must occupy no more than 80% of the total volume of the vessel. For these conditions, determine the mass of vapor and the mass of liquid in the vessel. At 320 K the vapor pressure of propane is 16.0 bar.

3.60. A 30 m³ tank contains 14 m³ of liquid n-butane in equilibrium with its vapor at 25°C.

Estimate the mass of n-butane vapor in the tank. The vapor pressure of n-butane at the given temperature is 2.43 bar.

3.61. Estimate:

(a) The mass of ethane contained in a 0.15 m³ vessel at 60°C and 14,000 kPa.

(b) The temperature at which 40 kg of ethane stored in a 0.15 m³ vessel exerts a pres-sure 20,000 kPa.

3.62. A size D compressed gas cylinder has an internal volume of 2.40 liters. Estimate the pressure in a size D cylinder if it contains 454 g of one of the following semiconductor process gases at 20°C:

(a) Phosphine, PH3, for which Tc = 324.8 K, Pc = 65.4 bar, and ω = 0.045 (b) Boron trifluoride, BF3, for which Tc = 260.9 K, Pc = 49.9 bar, and ω = 0.434 (c) Silane, SiH4, for which Tc = 269.7 K, Pc = 48.4 bar, and ω = 0.094

(d) Germane, GeH4, for which Tc = 312.2 K, Pc = 49.5 bar, and ω = 0.151 (e) Arsine, AsH3, for which Tc = 373 K, Pc = 65.5 bar, and ω = 0.011

(f) Nitrogen trifluoride, NF3, for which Tc = 234 K, Pc = 44.6 bar, and ω = 0.120 3.63. For one of the substances in Prob. 3.62, estimate the mass of the substance contained

in the size D cylinder at 20°C and 25 bar.

3.64. Recreational scuba diving using air is limited to depths of 40 m. Technical divers use different gas mixes at different depths, allowing them to go much deeper. Assuming a lung volume of 6 liters, estimate the mass of air in the lungs of:

(a) A person at atmospheric conditions.

(b) A recreational diver breathing air at a depth of 40 m below the ocean surface.

(c) A near-world-record technical diver at a depth of 300 m below the ocean surface, breathing 10 mol% oxygen, 20 mol% nitrogen, 70 mol% helium.

3.65. To what pressure does one fill a 0.15 m³ vessel at 25°C in order to store 40 kg of ethylene in it?

3.66. If 15 kg of H2O in a 0.4 m³ container is heated to 400°C, what pressure is developed?

3.67. A 0.35 m³ vessel holds ethane vapor at 25°C and 2200 kPa. If it is heated to 220°C, what pressure is developed?

3.68. What is the pressure in a 0.5 m³ vessel when it is charged with 10 kg of carbon dioxide at 30°C?

3.10. Problems 129

3.10 129

3.69. A rigid vessel, filled to one-half its volume with liquid nitrogen at its normal boiling point, is allowed to warm to 25°C. What pressure is developed? The molar volume of liquid nitrogen at its normal boiling point is 34.7 cm³·mol^–1.

3.70. The specific volume of isobutane liquid at 300 K and 4 bar is 1.824 cm³·g^–1. Estimate the specific volume at 415 K and 75 bar.

3.71. The density of liquid n-pentane is 0.630 g·cm^–3 at 18°C and 1 bar. Estimate its density at 140°C and 120 bar.

3.72. Estimate the density of liquid ethanol at 180°C and 200 bar.

3.73. Estimate the volume change of vaporization for ammonia at 20°C. At this temperature the vapor pressure of ammonia is 857 kPa.

3.74. PVT data may be taken by the following procedure: A mass m of a substance of molar mass ℳ is introduced into a thermostated vessel of known total volume V^t. The sys-tem is allowed to equilibrate, and the sys-temperature T and pressure P are measured.

(a) Approximately what percentage errors are allowable in the measured variables (m, ℳ, V^t, T, and P) if the maximum allowable error in the calculated compressibility factor Z is ±1%?

(b) Approximately what percentage errors are allowable in the measured variables if the maximum allowable error in calculated values of the second virial coefficient B is ±1%? Assume that Z ≃ 0.9 and that values of B are calculated by Eq. (3.37).

3.75. For a gas described by the Redlich/Kwong equation and for a temperature greater than T_c, develop expressions for the two limiting slopes,

lim

P→0 ( _{___}∂ Z

∂ P ) _T lim _P→∞ ( _{___}∂ Z

∂ P ) _T

Note that in the limit as P → 0, V → ∞, and that in the limit as P → ∞, V → b.

3.76. If 140(ft)³ of methane gas at 60(°F) and 1(atm) is equivalent to 1(gal) of gasoline as fuel for an automobile engine, what would be the volume of the tank required to hold methane at 3000(psia) and 60(°F) in an amount equivalent to 10(gal) of gasoline?

3.77. Determine a good estimate for the compressibility factor Z of saturated hydrogen vapor at 25 K and 3.213 bar. For comparison, an experimental value is Z = 0.7757.

3.78. The Boyle temperature is the temperature for which:

lim _P→0 ( _{___}∂ Z

∂ P ) _T = 0

(a) Show that the second virial coefficient B is zero at the Boyle temperature.

(b) Use the generalized correlation for B, Eqs. (3.58)–(3.62), to estimate the reduced Boyle temperature for simple fluids.

3.79. Natural gas (assume pure methane) is delivered to a city via pipeline at a volumetric rate of 150 million standard cubic feet per day. Average delivery conditions are 50(°F) and 300(psia). Determine:

(a) The volumetric delivery rate in actual cubic feet per day.

(b) The molar delivery rate in kmol per hour.

(c) The gas velocity at delivery conditions in m·s^–1.

The pipe is 24(in) schedule-40 steel with an inside diameter of 22.624(in). Standard conditions are 60(°F) and 1(atm).

3.80. Some corresponding-states correlations use the critical compressibility factor Zc, rather than the acentric factor ω, as a third parameter. The two types of correlation (one based on Tc, Pc, and Zc, the other on Tc, Pc, and ω) would be equivalent were there a one-to-one correspondence between Zc and ω. The data of App. B allow a test of this correspondence. Prepare a plot of Zc vs. ω to see how well Zc correlates with ω.

Develop a linear correlation (Zc= a + bω) for nonpolar substances.

3.81. Figure 3.3 suggests that the isochores (paths of constant volume) are approximately straight lines on a P-T diagram. Show that the following models imply linear isochores.

(a) Constant-β, κ equation for liquids (b) Ideal-gas equation

(c) Van der Waals equation

3.82. An ideal gas, initially at 25°C and 1 bar, undergoes the following cyclic processes in a closed system:

(a) In mechanically reversible processes, it is first compressed adiabatically to 5 bar, then cooled at a constant pressure of 5 bar to 25°C, and finally expanded isother-mally to its original pressure.

(b) The cycle is irreversible, and each step has an efficiency of 80% compared with the corresponding mechanically reversible process. The cycle still consists of an adiabatic compression step, an isobaric cooling step, and an isothermal expansion.

Calculate Q, W, ΔU, and ΔH for each step of the process and for the cycle. Take CP = (7/2)R and CV = (5/2)R.

3.83. Show that the density-series second virial coefficients can be derived from isothermal volumetric data via the expression:

B = lim _ρ→0 ( Z − 1 ) / ρ ρ(molar density)≡ 1 / V

3.84. Use the equation of the preceding problem and data from Table E.2 of App. E to obtain a value of B for water at one of the following temperatures:

(a) 300°C (b) 350°C

3.10. Problems 131

3.10 131

3.85. Derive the values of Ω, Ψ, and Zc given in Table 3.1 for:

(a) The Redlich/Kwong equation of state.

(b) The Soave/Redlich/Kwong equation of state.

(c) The Peng/Robinson equation of state.

3.86. Suppose Z vs. Pr data are available at constant Tr . Show that the reduced density-series second virial coefficient can be derived from such data via the expression:

B ˆ = lim _P

r →0 ( Z − 1 ) Z T r / P r

Suggestion: Base the development on the full virial expansion in density, Eq. (3.34) 3.87. Use the result of the preceding problem and data from Table D.1 of App. D to obtain a value

of B ˆ for simple fluids at Tr = 1. Compare the result with the value implied by Eq. (3.61).

3.88. The following conversation was overheard in the corridors of a large engineering firm.

New engineer: “Hi, boss. Why the big smile?”

Old-timer: “I finally won a wager with Harry Carey, from Research. He bet me that I couldn’t come up with a quick but accurate estimate for the molar volume of argon at 30°C and 300 bar. Nothing to it; I used the ideal-gas equation, and got about

Old-timer: “I finally won a wager with Harry Carey, from Research. He bet me that I couldn’t come up with a quick but accurate estimate for the molar volume of argon at 30°C and 300 bar. Nothing to it; I used the ideal-gas equation, and got about

In document INTRODUCTION TO CHEMICAL ENGINEERING (pagina 139-152)