Original Article
Phys Chem Ind J, Volume: 12( 3)
Estimation of Energy to be Supplied from an External Source to Heat or to Compress Alcohols (C3C12) in Gas Phase
 *Correspondence:
 Franco Junior MR PPG Biofuels, Federal University of Uberlandia, Av. João Naves de Ávila, 2121Santa Mônica, UberlândiaMG, 38408100, Brazil
Tel: 5534997793009; Email: [email protected]
Received Date: October 07, 2017 Accepted Date: December 11, 2017 Published Date: December 14, 2017
Citation: Franco Junior MR, Lamounier KFR, Rocha NRAF, et al. Estimation of Energy to be Supplied from an External Source to Heat or to Compress Alcohols (C3C12) in Gas Phase. Phys Chem Ind J. 2017;12(3):116
Abstract
The spent of energy in process is a cuttingedge research in the general field of energy application. In this paper the amount of energy for heating or compressing a system in gas phase was estimated using the thermodynamic equations. Firstly, the systems were chosen and among the alcohols we used them from C3 to C12 to discuss the effect of number of carbons atoms in the chain. Secondly, the PengRobinson equation represented the pVT system behavior. Also, influences of the level in temperature and pressure were analyzed.
The results show that the spent energy for the isobaric heating was very similar in value regarding the range of pressures (1 atm15 atm). The number of carbons in the chain had considerable influence on the heating result of alcohols, as well as in the solution of integral of pdV. For isothermic compression, when the process occurred at low pressures (1 atm to 5 atm), the amount of spent energy was practically constant for all alcohols studied. Also, for the same range of pressure, as the temperature rises, the energy to compress increased. Because there is no influence of the pdV term, internal energy change could be considered as the same of spent energy in the process. The main conclusions drawn from this work will be helpful for future development of efficiency equipment’s such as combustion motors.
Keywords
Energy; Alcohols; Eos; Thermodynamic; Compression; Heating
Introduction
Compression and heating are required for a variety of purposes, some of which can be listed: to provide fluid of process for combustion, to transport process fluid through pipelines, to provide heated or compressed fluid for reaction and so on and to circulate process fluid within a process.
The design of the heat or compression engine can be better done when estimation purposes are concerned with the behavior of the fluids of the process. In the biofuel industry, alcohols are much employed [1] and normally have to be compressed or heated before used. Having estimative for the spent thermal energy would facilitate to estimate the costs of the process, which could easily be calculated.
Renewable energy such as solar [24], geothermal [5,6] and waste heat [79] could be used as important sources for heating or compressing systems in recent years. However, thermal energy has to be converted to electricity or work. If taking into account the thermaltoelectricity conversion efficiency, it is necessary to calculate the amount of thermal energy in the process.
This paper demonstrates that calculation or prediction of the spent energy to compress or to heat some gaseous alcohols (C_{3} C_{12}) without phase change can be obtained when the physical properties are available using simple equations from the thermodynamic. Recent studies related to compression, expansion and heating of materials have used the thirdorder Birch Murnaghan equation of state (BM EoS) [10,11] as the pVT relation, in this work we represented them by PengRobinson cubic equation of state [12,13], which no previous work proposed before.
Methodology
There are two different kinds of energy, which are heat and mechanical energy, respectively, so we selected the primarily energy to evaluate the system performance.
In this work, two estimative of amount of energy to change the thermodynamic properties of gaseous alcohols were done as follows:
Isobaric heating
When applied to closed systems in which only internal energy changes occur, the first law of thermodynamics [12] can be used to calculate the amount of energy in the process being expressed mathematically as
(1)
where ΔU is the finite change given by the difference between the final and initial values of U. In case of isobaric processes, it can be estimate using the following equation
(2)
The heat Q and work given by the integral of pdV are finite quantities of heat and work; they are not properties of the system. Values for derivatives, V_{2} and V_{1} will be found solving PengRobinson equation [12,13] in the conditions of (p,T_{2}) and (p,T_{1}) respectively. Also, C_{p} is the molar capacity at constant pressure is informed by DIPPR data bank or [14].
Isothermic compression
For isothermic compression, the heat is estimated equally as described above; however the integral of pdV and the term for ΔU will be calculated using the expressions as given:
(3)
(4)
Where, a and b are the parameters of PengRobinson (PR) equation and the derivatives for Eq. (3) will be obtained by solving PR equation numerically.
Experimental data or fitted equation for C_{p} is from the data bank of DIPPR or by [14].
Otherwise for the systems used, the choice was to examine a restricted class of alcohols fluids that differ in molecular structure and polarity. To compare the influence of molecular chain and the influence of the terms of the basic equation used, Tables 14 report also the results obtained for C_{3}C_{12} studied. Critical constants and acentric factor (ω) are from [14].

1 atm  5 atm  

400 K500 K  600 K700 K  400 K500 K  600 K700 K  
2Propanol  2701  3511  2667  3500 
2butanol  3445  4480  3392  4465 
2pentanol  4172  5492  4094  5473 
1hexanol  4913  6468  4718  6440 
1heptacanol  5249  8688  6233  7421 
1nonanol  7185  9439  7312  9371 
1decanol  7941  10429  8073  10336 
1undecanol  8702  11421  8836  11301 
ndodecanol  9450  12409  9543  12122 
Table 1. Energy (cal/mol) for isobaric heating of a pure alcohol at low pressures (1 atm and 5 atm).
10 atm  15 atm  

400 K500 K  600 K700 K  400 K500 K  600 K700 K  
2Propanol  2539  3484  2508  3938 
2butanol  3287  4441  3548  4405 
2pentanol  4127  5439  4277  5366 
1hexanol  5024  6373  5022  6238 
1heptacanol  5987  7283  5987  7400 
1nonanol  7310  9316  7308  9539 
1decanol  8072  10534  8070  10531 
1undecanol  8834  11527  8832  11524 
ndodecanol  9597  12518  9594  12515 
Table 2. Energy (cal/mol) for isobaric heating of a pure alcohol at moderate pressures (10 atm and 15 atm).
400 K  700 K  

2propanol  4219711  12870813 
2butanol  4238073  12871334 
2pentanol  4270368  12874343 
1hexanol  4423293  12879974 
1heptacanol  4347819  12885974 
1nonanol  4160889  12910944 
1decanol  4056524  12931636 
1undecanol  4001850  12956371 
ndodecanol  3796365  12991044 
Table 3. Energy (cal/mol) for isothermic compression of a pure alcohol at two distinct temperatures from 1 atm to 5 atm.
400 K  600 K  800 K  

5 atm10 atm  10 atm20 atm  5 atm10 atm  10 atm20 atm  5 atm10 atm  10 atm20 atm  
2Propanol  0.8433  0.4441  1.4830  1.5180  2.628  2.636 
2butanol  0.7221  0.3282  1.4900  1.5970  2.630  2.647 
2pentanol  0.6278  0.3283  1.5030  1.6970  2.634  2.670 
1hexanol  0.3282  0.3283  1.5410  1.4460  2.640  2.722 
1heptanol  0.3283  0.3283  1.6340  1.0910  2.649  2.837 
1nonanol  0.3282  0.3283  1.5840  0.7389  2.685  2.901 
1decanol  0.3283  0.3283  1.4250  0.7386  2.724  2.646 
1undecanol  0.3283  0.3283  1.2670  0.7386  2.792  2.322 
ndodecanol  0.3283  0.3283  0.7386  0.7386  2.889  1.979 
Table 4. Energy (Q.10^{6}, cal/mol) for isothermic compression of a pure alcohol at three distinct temperatures at two limits.
Results and Discussion
Apparently, the calculation for energy spent for compressing and heating fluids is a common and classic process. Hence, the key point is to acquire the accuracy and reliable results of for the alcohols systems. Calculations were performed for nine alcohols systems such as: 2propanol, 2butanol, 2pentanol, 1hexanol, 1heptanol, 1nonanol, 1decanol, 1undecanol and ndodecanol (C_{3}C_{12}). For that, the experimental molar heat capacity, critical properties, acentric factor as well as the saturation pressure equation to decide the limits and intervals would be adopted are found in DIPPR data bank, together with the relevant literature values available so far [DDB]. Based on the theoretical model and operation conditions, a simulation examples of the compression and heating process is conducted, which is shown in Tables 14. In Tables 12, the calculated amount of energy for heating at low and moderate pressures of the alcohols are shown as a function of pressure and the number of carbon atoms n in their chains. Comparison is made with the different pressures used and for two intervals of temperatures. As expected, related to the energy spent for heating values are higher as the carbon number increases.
Moreover, it did not change with rising pressure, otherwise for interval of heating near critical temperature, values are a little higher.
To analysis the performance of the alcohols systems and make a comparison with long chain ones, the key operation parameters on the system are discussed in this section, and the variation ranges of pressures (1 atm15 atm) and temperatures (400 K800 K) are also presented in the Tables 3 and 4 for the compression process. For the same range of pressure, as the temperature rises, the amount of thermal energy to compress increased. In general, for 50% of temperature increased, the amount of spent thermal energy triplicate. At low and moderate temperatures, the spent energy for compressing decreased as the length of the carbon chain increased.
The molar internal energy and the correspondent term pdV are reported in Figure 1. As can be seen, molar internal energies are really much higher than the integral of pdV. Therefore, the second one can be neglected in the future calculations if amount of energy has to be quantified for. Our results can also be usefully presented as plots of the molar internal energies (DU) and integral of pdV as a function of number of carbons atoms (n), pressure and temperatures [Figure 25].
Figure 2 illustrates the effect of pressure (P) on the DU (or ?U) term for each system that is heated in the variation of temperature of 400 K500 K. The chosen pressures of the system can be adjusted according to the need due to the pVT behavior of the group of compounds tested. Observing this figure, it is obvious that, for this range of pressure, the calculated results were not influenced by the pressure; otherwise they were hardly affected by the number of carbons in the chain.
For both process, the integral of pdV was affected by the level of pressure. Figure 3 depicts results for the heating process and apart from 1 atm all data were influenced by the number of carbon atoms. Despite being an important term, when compared with the internal energy, the value is too small, and then negligible.
In Figure 4, in low pressures, on increasing n (number of C atoms) is observed that the amount of thermal energy stays invariable. Otherwise for moderate pressures and higher temperatures the amount of thermal energy decreases when n increases. This is attributable to a progressive prevalence of the dispersive interactions contribution to the stability of higher terms and is manifested by an almost constant decrease per methylene unit.
The influence of temperature in the DU term is shown in Figure 5. It can be seen that the average increase of calculated DU of alcohols is due to the progressively increased dimension of the molecules and corresponding increase of dispersive interaction.
Conclusion
The amount of thermal energy for heating or compressing alcohols in gaseous phase was evaluated for low and moderate pressures in low and high temperatures.
The influence of the integral of pdV is not pronounced nor for isobaric heating neither for the isothermic compression, then the calculation of the spent energy is reasonable even if the one is neglected. Summing up, internal energy change could be considered as the same of thermal energy spent in all processes.
Depending on the range of pressure and the level of temperature, the amount of spent energy can be affected or not by the number of carbon atoms of the system.
Acknowledgements
This work has been supported by the UniRVUniversity of Rio Verde which provided scholarship (Grant No. 30Public Notice 01/2016 PRPPG/UniRV).
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