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Department of Chemical Engineering, NITK Tutorial-VII

This document contains 11 problems related to chemical engineering thermodynamics. Problem 1 involves calculating thermodynamic properties of acetone such as the derivative of pressure with respect to temperature at a given state point and changes in pressure and volume between two state points. Problem 2 compares the ideal gas and van der Waals equations of state for CO2 at a given state point. Problem 3 involves calculating the acentric factor for ethanol using its vapor pressure equation.

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254 views2 pages

Department of Chemical Engineering, NITK Tutorial-VII

This document contains 11 problems related to chemical engineering thermodynamics. Problem 1 involves calculating thermodynamic properties of acetone such as the derivative of pressure with respect to temperature at a given state point and changes in pressure and volume between two state points. Problem 2 compares the ideal gas and van der Waals equations of state for CO2 at a given state point. Problem 3 involves calculating the acentric factor for ethanol using its vapor pressure equation.

Uploaded by

Nandita Chouhan
Copyright
© © All Rights Reserved
We take content rights seriously. If you suspect this is your content, claim it here.
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Download as PDF, TXT or read online on Scribd
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Department of Chemical Engineering, NITK

Tutorial-VII: Chemical Engineering Thermodynamics


Date: 07-10-20
(1) For a liquid acetone at 20°C and 1 bar, β = 1.487 * °C , K = 62 * -1 , V= 1.287

. For acetone , find the


 P 
(a) value of   at 20 C and 1 bar
o

 T v
(b) Pressure generated by heating at Constant volume from 20oC and 1 bar to 30oC
(c) Change in volume for a change from 20oC and 1 bar to 0oC and 10 bar

(2) One 1 kilo mole of CO2 occupies a volume of 0.381 m3 at 313 K. Compare pressure given by
(a) ideal gas equation
(b) Van der Waals equation
Take the Van der Waals constant to be a =0.365 Nm4/mol4, b=4.28 x10-5 m3/mol.

(3) Calculate the acentric factor for ethanol. The vapor pressure of ethanol can be estimated
from the following equation
1592.864
log10 P sat  8.1122 
t  226.184
where Psat is in mmHg and t is in oC. The critical constant for ethanol are TC =513.9 K & PC =61.48
bar.

(4) Determine the molar volume of methane at 600 bar and 27oC (300K) by using
(i) the ideal gas equation
(ii) the Van der Waals equation
The Van der Waals constants a and b are 0.2285 Nm4/mol2 and 4.27 x 10-5 m3/mol respectively.
(iii) the Redlich-Kwong equation. The critical temperature and pressure are 191.1K and
46.4 bar respectively

(5) A vessel of volume 0.03 m3 contains 0.5 kg gaseous ammonia at a constant temperature of
338K. The critical pressure and temperature are 112.8 bar and 405.5 K, respectively. Calculate
the pressure developed by this gas using the Redlich-Kwong equation

(6) Calculate the compressibility factor and molar volume for CH4 vapor at 500 K and 10 bar
using following equation. Experimental values of virial coefficients are B= -2.19 x 10-4 m3/mol;
C= -1.73 x 10-8 m6/mol2. The critical temperature and pressure of methanol are 512.6K and 81 bar.
(a) Virial equation (truncated form)
(b) Redlich –Kwong equation

(7) Determine the specific volume of refrigerant-134a at 1 MPa and 50°C, using (a) the ideal-gas
equation of state and (b) the generalized compressibility chart. Compare the values obtained to
the actual value of 0.021796 m3/kg and determine the error involved in each case
(8) A 40 kg block of iron casting at 625 K is dropped into a well-insulated vessel containing 160
kg of H2O at 276 K. Compute the amount of work lost in the process. Assume that the specific
heat of iron is 0.45 kJ/kg.K and that of water is 4.185 kJ/kg. K. (HW)

(9) Oil with a heat capacity of 3.2 kJ/kg.K is to be cooled from 495 K to 315 K at the rate of 5000
kg/hour. And unlimited supply of cooling water at a constant temperature of 303 K is available.
Determine the loss work in the process and the thermodynamic efficiency of the process. (HW)

(10) Predict the pressure of nitrogen gas at T= 175 K and v = 0.00375 m3/kg on the basis of
(a) the ideal-gas equation of state,
(b) the Van der Waals equation of state
(c) the Beattie-Bridgeman equation of state, and
(d)the Benedict-Webb-Rubin equation of state.
Compare the values obtained to the experimentally determined value of 10,000 kPa. (HW)

(11) Calculate the molar volume and compressibility factor of isopropanol vapor at 473 K
(200oC) and 10 bar using the virial equation
The virial coefficients are: B=-3.88 x 10-4 m3/mol and C=-2.6 x10-8 m6/mol2 (HW)

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