Anees A. Khadom, Aprael S. Yaro, and Abdul Amir H. Kadhum
Keywords: adsorption isotherms, corrosion inhibition, copper-nickel alloy, organic inhibitors
Abstract:
The inhibition of copper corrosion by Naphthylamine (NA), Ethylenediamine (EDA), Tetraethylenepentamine (TEPA), Diethylenetriamine (DETA), and Phenylenediamine (PDA) in 5% HCl have been investigated by weight loss technique at different temperatures. Langmuir adsorption isotherm, Freundlich Adsorption Isotherm and Kinetic-Thermodynamic Model were used to describe the adsorption process depending on values of surface converge. Maximum value of surface converge was 0.856 for NA at 35 oC and 15 g/l inhibitor concentration, while the lower value was 0.01 for PDA at 55 oC and 1 g/l inhibitor concentration. The films formed on the copper-nickel alloy surface of NA, EDA, TEPA, and DETA appear to obey the Freundlich Adsorption Isotherm more than Langmuir adsorption isotherm. In the other hand, the two-adsorption isotherms were unsuitable to represent the data of PDA. Results also showed that the Kinetic-Thermodynamic Model was suitable to fit the experimental data of the most inhibitors of the present study.
Because you are not logged-in to the journal, it is now our policy to display a 'text-only' version of the preprint. This version is obtained by extracting the text from the PDF or HTML file, and it is not guaranteed that the text will be a true image of the text of the paper. The text-only version is intended to act as a reference for search engines when they index the site, and it is not designed to be read by humans!
If you wish to view the human-readable version of the preprint, then please Register (if you have not already done so) and Login. Registration is completely free.
dISSN 1466-8858 Volume 12, Preprint 18 submitted 11 May 2009d ©dMTT9dUniversitydofdManchesterdanddthedauthorsFdThisdisdadpreprintdofdadpaperdthatdhasdbeendsubmitteddfordpublicationdindthedJournaldofd CorrosiondSciencedanddEngineeringFdItdwilldbedrevieweddandcdsubjectdtodthedreviewers"dcommentscdbedpublisheddonlinedatd http:DDwwwFjcseForgdindduedcourseFdUntildsuchdtimedasditdhasdbeendfullydpublishedditdshoulddnotdnormallydbedreferenceddindpublisheddworkFd 1 Adsorption MechanismAdsorption MechanismAdsorption MechanismAdsorption Mechanism of Some Chemical of Some Chemical of Some Chemical of Some Chemical Amines Amines Amines Amines Inhibitors Inhibitors Inhibitors Inhibitors forforforfor Corrosion Inhibition of CopperCorrosion Inhibition of CopperCorrosion Inhibition of CopperCorrosion Inhibition of Copper----Nickel Nickel Nickel Nickel Alloy AlloyAlloyAlloy in in in in Hydrochloric Hydrochloric Hydrochloric Hydrochloric Acid Acid Acid Acid Anees A. Khadom1,*, Aprael S. Yaro2, and Abdul Amir H. Kadhum1 1 Department of Chemical and Process Engineering , Faculty of Engineering and Built Environment, Universiti Kebangsaan Malaysia, Bangi, 43600, Selangor, Malaysia. 2 Chemical Engineering Department, College of Engineering, Baghdad University, Baghdad, Iraq. * * * * Corresponding for author: Corresponding for author: Corresponding for author: Corresponding for author: E-mail address: aneesdr@gmail.com Telephone: 0060 17 8769594, Fax no. : 603-89252546, 603-89216148 Abstract:Abstract:Abstract:Abstract: The inhibition of copper corrosion by Naphthylamine (NA), Ethylenediamine (EDA), Tetraethylenepentamine (TEPA), Diethylenetriamine (DETA), and Phenylenediamine (PDA) in 5% HCl have been investigated by weight loss technique at different temperatures. Langmuir adsorption isotherm, Freundlich Adsorption Isotherm and Kinetic-Thermodynamic Model were used to describe the adsorption process depending on values of surface converge. Maximum value of surface converge was 0.856 for NA at 35 oC and 15 g/l inhibitor concentration, while the lower value was 0.01 for PDA at 55 oC and 1 g/l inhibitor concentration. The films formed on the copper-nickel alloy surface of NA, EDA, TEPA, and DETA appear to obey the Freundlich Adsorption Isotherm more than Langmuir adsorption isotherm. In the other hand, the two-adsorption isotherms were unsuitable to represent the data of PDA. Results also showed that the Kinetic-Thermodynamic Model was suitable to fit the experimental data of the most inhibitors of the present study. Keywords: Keywords:Keywords:Keywords: adsorption isotherms, corrosion inhibition, copper-nickel alloy, organic inhibitors Introduction:Introduction:Introduction:Introduction: Copper and its alloys are commonly employed as a material in heating and cooling systems due to their good thermal conductivity and mechanical properties. Hydrochloric acid pickling is extensively used for the removal of rust and scale on heat transfer in several industrial processes. However, these systems should be regularly cleaned from carbonates and oxides that diminish dISSN 1466-8858 Volume 12, Preprint 18 submitted 11 May 2009d ©dMTT9dUniversitydofdManchesterdanddthedauthorsFdThisdisdadpreprintdofdadpaperdthatdhasdbeendsubmitteddfordpublicationdindthedJournaldofd CorrosiondSciencedanddEngineeringFdItdwilldbedrevieweddandcdsubjectdtodthedreviewers"dcommentscdbedpublisheddonlinedatd http:DDwwwFjcseForgdindduedcourseFdUntildsuchdtimedasditdhasdbeendfullydpublishedditdshoulddnotdnormallydbedreferenceddindpublisheddworkFd 2 their heating transmission. Diluted hydrochloric acid is used to clean these surfaces; a corrosion inhibitor is added to avoid the action of this acid on copper. Corrosion inhibitor is a chemical substance which when added in small concentration to environment effectively checks, decrease or prevent the reaction of metal with environment (1). It must be clearly understood that no universal corrosion inhibitor exists. Each inhibitor must be tailored to the specific corrosion problem that needs solution. While the use of inhibitors for some types of corrosion can be similar to other, this similarity must be treated as coincidence. Most inhibitors have been developed by empirical experimentation. Amines and triazoles derivatives have been reported to be very effective inhibitors for copper in acidic solutions [2-5]. The corrosion mechanism can vary considerably depending on the corrosive factors that are present. Similarly, the mechanism of inhibition will vary depending on the chemical nature of the inhibitor and the factor causing corrosion [6]. The most widely accepted postulated involves the formation of surface layers or films, which reduce the ease of access of the corrosive materials to the metal surface. Such scale can be formed naturally, or can be induced to form [7]. An equation relates the amount of substance attached to surface to its concentration in gas phase or in solution at fixed temperature, is known as an adsorption isotherms [8]. The simplest isotherm was first obtained in 1916 by Irvan Langmuir [8]. This isotherm can be represented as; KC KC += 1θ (1) Systems that obey this equation are often referred to ideal adsorption. Systems frequently deviate significantly from Langmuir equation. This may be because the surface is not uniform, and also there may be interaction between adsorbed molecules, a molecule attached to surface may make it more difficult, or less difficult, for another molecules to became attached to a neighboring site, and this will lead to deviation from the ideal adsorption equation. Non-ideal system can sometimes be fitted to an empirical adsorption isotherm of Freundlich [9] nKC=θ (2) K, is equilibrium constant, C is inhibitor concentration, n is positive generally not integer constant, and (θ) is surface coverage. The Freundlich isotherm theory says that the ratio of the amount of solute adsorbed onto a given mass of sorbent to the concentration of the solute in the solution is not constant at different concentrations [10]. dISSN 1466-8858 Volume 12, Preprint 18 submitted 11 May 2009d ©dMTT9dUniversitydofdManchesterdanddthedauthorsFdThisdisdadpreprintdofdadpaperdthatdhasdbeendsubmitteddfordpublicationdindthedJournaldofd CorrosiondSciencedanddEngineeringFdItdwilldbedrevieweddandcdsubjectdtodthedreviewers"dcommentscdbedpublisheddonlinedatd http:DDwwwFjcseForgdindduedcourseFdUntildsuchdtimedasditdhasdbeendfullydpublishedditdshoulddnotdnormallydbedreferenceddindpublisheddworkFd 3 Recent researches have looked in to the action of adsorptive inhibitors from purely mechanistic kinetic point of view [11, 12]. A kinetic-thermodynamic model for adsorption process at metal-solution interface has been suggested. This model has been tested on inhibition effect of number of open chain amines and one macrocyclic amine on the corrosion of steel in H 2SO4 [12] and aluminum in HCl [13]. In this model, (y) is the number of inhibitor molecules occupying one active site. This model can be given by the following equation; [ ]yCK`1=) ))( (( -θθ (3) Values of y>1 implies the formation of multilayers of inhibitor on the surface of metal. Values of y<1 mean a given inhibitor molecules will occupy more than one active site. K, corresponding to adsorption isotherm is given by; )) )) (( ((=yKK 1 ` (4) The present work is an attempt to evaluate some corrosion inhibitors for copper-nickel alloy in HCl. Some amines, which used in the past as corrosion inhibitors for another metals, such as Fe and Al, in another acids such as H 2SO4, H 3PO4 and HNO3 are tested here for the corrosion of copper in 5% HCl at different temperatures. ExperimentalExperimentalExperimentalExperimental WorkWorkWorkWork:::: The corrosion behavior of copper-nickel alloys, which used widely in many industrial equipments, was studied using weight loss in absence and presence of Naphthylamine (NA), Ethylenediamine (EDA), Tetraethylenepentamine (TEPA), Diethylenetriamine (DETA), and Phenylenediamine (PDA) in 5% HCl solution at different temperature (35, 45, and 55 C o), and different inhibitor concentrations (1, 5, 10, and 15 g/l). Ring shape specimen of Cu-Ni alloy with dimension (2.22 cm) outside diameter, (1.5 cm) width, and (0.13 cm) thickness, exposing a surface area of about (10 cm 2) to corrosive media. Specimens were cleaned by washing with detergent and flushed with tap water followed by distilled water, degreased by analar benzene and acetone, then annealed in vacuums to 600 C o for one hour and cooled under vacuum to room temperature. Before each run, specimens of Cu-Ni were abraded in sequence using emery paper of grade number 220,320, 400, and 600, then washed with running tap water followed by distilled water then dried with clean tissue, degreased with benzene, dried, degreased with acetone, dried, and finally left in desicater over silica gel. Weighing the specimen was carried out using 4 decimals digital balance and its dimensions were measured with dISSN 1466-8858 Volume 12, Preprint 18 submitted 11 May 2009d ©dMTT9dUniversitydofdManchesterdanddthedauthorsFdThisdisdadpreprintdofdadpaperdthatdhasdbeendsubmitteddfordpublicationdindthedJournaldofd CorrosiondSciencedanddEngineeringFdItdwilldbedrevieweddandcdsubjectdtodthedreviewers"dcommentscdbedpublisheddonlinedatd http:DDwwwFjcseForgdindduedcourseFdUntildsuchdtimedasditdhasdbeendfullydpublishedditdshoulddnotdnormallydbedreferenceddindpublisheddworkFd 4 vernier. The metal samples for weight loss runs were completely immersed in 250-cm 3 solution of corrodant contained in a conical flask. They were exposed for a period of three days at a desired temperature, acid concentration, and inhibitor concentration. Weight losses were determined in absence and presence of inhibitors. The data are expressed as mass loss per unit time per unit area; in present work the units of corrosion rate were g/m 2.day (gmd). The chemical compositions of Cu-Ni alloy were (0.148 %Sn, 0.2%Fe, 0.134%Zn, 0.015%Al, 0.0003%P, 0.5%Sb, 0.0583%Pb, 0.0202%Si, 0.017%S, 0.0056%As, 10%Ni, and the reminder is Cu). Results and Discussions:Results and Discussions:Results and Discussions:Results and Discussions: The corrosion rates of Cu-Ni alloy in 5% HCl acid solution as a function of temperature in absence and presence of different inhibitors concentrations are summarized in Table (1) through 64 runs using weight loss technique. The following equation was used to calculate the inhibitor efficiency: 100%×-= uninhibitinhibituninibitWWWIE (5) Where W uninhibit and Winhibit are the corrosion rates in absence and presence of inhibitor respectively. Table Table Table Table 1111 Effect of Temperature and Inhibitor Concentration on the Corrosion of Cu-Ni alloy in 5% HCl Acid Solution. Run Inhibitors C (g/l) T (oC) Rate (gmd) IE (%) 1 NilNilNilNil Nil 35 12.5 2 45 15.87 3 55 20.83 4 NA NANANA 1 35 10.5 16 5 5 6.875 45 6 10 4 68 7 15 1.8 85.6 8 1 45 14.01 11 9 5 10.313 35 10 10 6.341 60 11 15 3.65 77 12 1 55 19.021 8.8 13 5 14.032 32.3 14 10 9.374 55 15 15 6.249 70 16 EDAEDAEDAEDA 1 10.312 17.5 dISSN 1466-8858 Volume 12, Preprint 18 submitted 11 May 2009d ©dMTT9dUniversitydofdManchesterdanddthedauthorsFdThisdisdadpreprintdofdadpaperdthatdhasdbeendsubmitteddfordpublicationdindthedJournaldofd CorrosiondSciencedanddEngineeringFdItdwilldbedrevieweddandcdsubjectdtodthedreviewers"dcommentscdbedpublisheddonlinedatd http:DDwwwFjcseForgdindduedcourseFdUntildsuchdtimedasditdhasdbeendfullydpublishedditdshoulddnotdnormallydbedreferenceddindpublisheddworkFd 5 17 5 35 7.843 37.25 18 10 5.274 57.8 19 15 3.125 75 20 1 45 12.692 20.03 22 5 9.744 38.6 23 10 6.874 56.68 24 15 4.741 70.126 25 1 55 17.741 14.83 26 5 13.324 36.03 27 10 10.554 49.33 28 15 55 7.875 62.193 29 TEPA TEPATEPATEPA 1 35 10.8 13.6 30 5 9.375 25 31 10 8 36 32 15 6.5 48 33 1 45 13.5 14.9 34 5 10.932 31.1 35 10 9.52 40 36 15 7.457 53 37 1 55 16.8 19.3 38 5 13.96 32.9 39 10 11.66 44 40 15 9.373 55 41 DETADETADETADETA 1 35 12.375 4 42 5 12 8 43 10 11.51 10.9 44 15 10.625 15 45 1 45 14.985 5.6 46 5 13.71 13.6 47 10 13 15 48 15 11.265 29 49 1 55 19.44 6.7 50 5 16.987 18.5 51 10 14.58 30 52 15 12.05 42.4 53 PDA PDAPDAPDA 1 35 12.3 1.6 54 5 11.625 7 55 10 10.95 8.5 dISSN 1466-8858 Volume 12, Preprint 18 submitted 11 May 2009d ©dMTT9dUniversitydofdManchesterdanddthedauthorsFdThisdisdadpreprintdofdadpaperdthatdhasdbeendsubmitteddfordpublicationdindthedJournaldofd CorrosiondSciencedanddEngineeringFdItdwilldbedrevieweddandcdsubjectdtodthedreviewers"dcommentscdbedpublisheddonlinedatd http:DDwwwFjcseForgdindduedcourseFdUntildsuchdtimedasditdhasdbeendfullydpublishedditdshoulddnotdnormallydbedreferenceddindpublisheddworkFd 6 56 15 9.2 10 57 1 45 15.39 3 58 5 14.28 10 59 10 11.437 31 60 15 11.25 42 61 1 55 20.622 1 62 5 18.54 11 63 10 17.91 14 64 15 14.587 30 The primary step in the action of inhibitors in acid solution is generally agreed to be adsorption on the metal surface. This involves the assumption that the corrosion reactions are prevented from occurring over the area (or active sites) of the metal surface covered by adsorbed inhibitor species, whereas these corrosion reaction occurred normally on the inhibitor-free area [14]. Accordingly, the fraction of surface covered with inhibitor species ( 100 %IE=θ) can followed as a function of inhibitor concentration and solution temperature. The surface coverage (θ) data are very useful while discussing the adsorption characteristics. When the fraction of surface covered is determined as a function of the concentration at constant temperature, adsorption isotherm could be evaluated at equilibrium condition. The corrosion rate increases with temperature increasing, generally, the addition of inhibitors reduces the corrosion rate, and the reductions depend on the type of inhibitors. All tested inhibitors, approximately, give the same behavior; the corrosion rate decreases with increasing the inhibitors concentrations, and increases with temperature increasing. The order of inhibition of inhibitors evaluated by weight loss technique was as follows: - NA > EDA > TEPA > DETA > PDA The corrosion rate data can be used to analyze the adsorption mechanism, by using the value of θas a function of inhibitor concentration. Rearranging Langmuir isotherm equation will gives: CK C+=1 θ (6) dISSN 1466-8858 Volume 12, Preprint 18 submitted 11 May 2009d ©dMTT9dUniversitydofdManchesterdanddthedauthorsFdThisdisdadpreprintdofdadpaperdthatdhasdbeendsubmitteddfordpublicationdindthedJournaldofd CorrosiondSciencedanddEngineeringFdItdwilldbedrevieweddandcdsubjectdtodthedreviewers"dcommentscdbedpublisheddonlinedatd http:DDwwwFjcseForgdindduedcourseFdUntildsuchdtimedasditdhasdbeendfullydpublishedditdshoulddnotdnormallydbedreferenceddindpublisheddworkFd 7 Equation (6) can be plotted as ) ))( ((θ C vs. C. The higher value of K indicates that the inhibitor is strongly adsorbed on the metal surface. From Table (2), and figure 1 the Langmuir lines deviate from linearity in the case of NA, the relation between surface coverage and the concentration of NA becomes linear when Freundlich adsorption isotherm is applied. This suggest that the corrosion rate data for NA is follow Freundlich adsorption isotherm (figure 2), with K values of 0.1614, 0.1099, and 0.0895 l/g at 35, 45 and 55 oC respectively, which in the same order and gives the same behavior as in Langmuir adsorption isotherm. The average value of (n) was 0.703 at different temperature, which is in agree with typical value of n= 0.6 [15]. Figure 3 shows the kinetic thermodynamic model for the adsorption of NA on Cu-Ni surface. Generally, values of K obtained from the two-adsorption isotherms were in a good agreed with the values obtained from kinetic-thermodynamic models (0.22, 0.151, and 0.123 l/g) at 35,45and 55 C o, respectively. The values of y at different temperatures were near unity (1.19 to 1.154), which indicates that NA molecules were attached to one active site of Cu-Ni alloy. For EDA, there is a good agreement between the adsorption isotherms and kinetic-thermodynamic model, as it is shown from the values of K obtained from different models. The best fit was obtained by Freundlich adsorption isotherm (figure 4), the values of K approximately constant with increasing of temperature. As shown in figure (5), for TEPA, the best fit to the data was by using Freundlich adsorption isotherm with an average value of correlation coefficient of 0.995. The values of equilibrium constant were increased slightly with temperature, which indicate, that there is some improvement in surface coverage with increasing in temperature. Values of K obtained from kinetic-thermodynamic model are differing from that obtained from adsorption isotherm, which indicate that this model did not represent the corrosion rate data of TEPA. In the case of DETA, figure (6) shows that Freundlich adsorption isotherm fit the corrosion rate data with an average correlation coefficient of 0.9854, which is more than the average correlation coefficient of Langmuir adsorption isotherm, (i.e., 0.8948). Also, there is some increasing in the values of K with increasing in temperature. The values of K obtained from the two-adsorption isotherm were in the same order, while the values that obtained from kinetic-thermodynamic model were lower, and y<1. Non of the adsorption isotherm used in present work are represent the corrosion rate data of PDA, this may be due to a low surface coverage of this dISSN 1466-8858 Volume 12, Preprint 18 submitted 11 May 2009d ©dMTT9dUniversitydofdManchesterdanddthedauthorsFdThisdisdadpreprintdofdadpaperdthatdhasdbeendsubmitteddfordpublicationdindthedJournaldofd CorrosiondSciencedanddEngineeringFdItdwilldbedrevieweddandcdsubjectdtodthedreviewers"dcommentscdbedpublisheddonlinedatd http:DDwwwFjcseForgdindduedcourseFdUntildsuchdtimedasditdhasdbeendfullydpublishedditdshoulddnotdnormallydbedreferenceddindpublisheddworkFd 8 inhibitor and low ability to form a layer on the metal surface. Kinetic- thermodynamic model slightly fit the corrosion rate data with K values in the same order as the values obtained from the adsorption isotherms. Generally, the values of K are approximately constant with an average value of 0.021 l/g. From the values of equilibrium constants, which obtained from different isotherms, the values of heat of adsorption, ΔG ads, can be obtained using the following equation [16] ) ))( (( Δ-) ))( ((=RTGK adsexp55.551 (7) The value of (55.5) is the water concentration in solution expressed in M, (i.e., ~1000 g/l). R and T are the gas constant and absolute temperature respectively. The values of ΔG ads, heat of adsorption were given in tables (2), (3), and (4). The values of ΔG ads for the five inhibitors were in the range of (-3.418 to - 14.28 kJ/mol.), which indicate the weak adsorption of these inhibitors to the metal surface. The negative value of o adsGΔ ensure the spontaneity of the adsorption process and stability of the adsorbed layer on the metal surface. Generally, value of o adsGΔ up to -20 kJ.mol-1 is consistent with electrostatic interaction between the charged molecules and the charged metal (physisorption) while those around -40 kJ.mol -1 or higher are associated with chemisorptions as a result of sharing or transfer of electrons from the organic molecules to the metal surface to form a coordinate type of bond [17,18]. While other researchers suggested that the range of o adsGΔ of chemical adsorption processes for organic inhibitor in aqueous media lies between -21 to -42 kJ.mol -1 [19]. Therefore, for present work the value of o adsGΔ has been considered within the range of physical adsorption. Table TableTableTable 2222 Adsorption Constants, and heats of adsorption from Langmuir Isotherm Models. Inhibit or T (oC) K (l/g) ΔGads (kJ/mol.) R BTABTABTABTA 35 5.586 -22.093 0.99993 45 4.762 -22.389 0.99992 3 55 4.762 -23.093 0.99989 NA NANANA 35 0.1603 -13 0.9851 45 0.106 -12.329 0.9725 dISSN 1466-8858 Volume 12, Preprint 18 submitted 11 May 2009d ©dMTT9dUniversitydofdManchesterdanddthedauthorsFdThisdisdadpreprintdofdadpaperdthatdhasdbeendsubmitteddfordpublicationdindthedJournaldofd CorrosiondSciencedanddEngineeringFdItdwilldbedrevieweddandcdsubjectdtodthedreviewers"dcommentscdbedpublisheddonlinedatd http:DDwwwFjcseForgdindduedcourseFdUntildsuchdtimedasditdhasdbeendfullydpublishedditdshoulddnotdnormallydbedreferenceddindpublisheddworkFd 9 55 0.089 -12.24 0.99109 TEPA TEPATEPATEPA 35 0.115 -12.15 0.95489 45 0.143 -13.121 0.9727 55 0.18 -14.161 0.97755 PDA PDAPDAPDA 35 0.02 -7.671 0.98296 45 0.025 -8.510 0.2068 55 0.0116 -6.683 0.6095 Table TableTableTable 3333 Adsorption Constants, Heats of Adsorption, and n From Freundlich Isotherm Models. Inhibit or T (oC) K (l/g) n ΔGads (kJ/mol.) R BTABTABTABTA 35 0.883 0.048 -17.37 0.974 2 45 0.87 0.049 -17.894 0.990 17 55 0.879 0.043 -18.485 0.998 5 EDA EDAEDAEDA 35 0.1698 0.532 -13.15 0.996 7 45 0.1954 0.460 -13.95 0.997 1 55 0.1496 0.526 -13.66 0.999 4 TEPA TEPATEPATEPA 35 0.131 0.452 -12.484 0.991 82 45 0.148 0.455 -13.211 0.997 24 55 0.188 0.378 -14.279 0.995 16 DETA DETADETADETA 35 0.039 0.471 -9.381 0.994 47 45 0.054 0.546 -10.546 0.963 12 55 0.0656 0.672 -11.408 0.998 61 dISSN 1466-8858 Volume 12, Preprint 18 submitted 11 May 2009d ©dMTT9dUniversitydofdManchesterdanddthedauthorsFdThisdisdadpreprintdofdadpaperdthatdhasdbeendsubmitteddfordpublicationdindthedJournaldofd CorrosiondSciencedanddEngineeringFdItdwilldbedrevieweddandcdsubjectdtodthedreviewers"dcommentscdbedpublisheddonlinedatd http:DDwwwFjcseForgdindduedcourseFdUntildsuchdtimedasditdhasdbeendfullydpublishedditdshoulddnotdnormallydbedreferenceddindpublisheddworkFd 10 Table TableTableTable 4444 Adsorption Constants, heats of adsorption, and y from Kinetic- Thermodynamic Models. Inhibit or T (oC) K (l/g) y ΔGads (kJ/mol.) R BTABTABTABTA 35 3.67 1.31 -21.018 0.89 45 5.53 1.003 -22.784 0.940 6 55 8.803 0.813 -24.768 0.955 29 NA NANANA 35 0.22 1.199 -13.811 0.977 6 45 0.151 1.176 -13.265 0.986 1 55 0.123 1.154 -13.122 0.994 8 EDA EDAEDAEDA 35 0.160 0.925 -12.996 0.971 5 45 0.152 0.793 -13.282 0.978 9 55 0.107 0.802 -12.742 0.995 0 TEPA TEPATEPATEPA 35 0.0447 0.621 -9.73 0.992 5 45 0.065 0.652 -11.036 0.952 52 55 0.074 0.575 -11.737 0.992 8 ETA ETAETAETA 35 0.002 0.512 -1.775 0.992 48 45 0.0106 0.631 -6.241 0.952 52 55 0.0393 0.833 -10.011 0.992 84 dISSN 1466-8858 Volume 12, Preprint 18 submitted 11 May 2009d ©dMTT9dUniversitydofdManchesterdanddthedauthorsFdThisdisdadpreprintdofdadpaperdthatdhasdbeendsubmitteddfordpublicationdindthedJournaldofd CorrosiondSciencedanddEngineeringFdItdwilldbedrevieweddandcdsubjectdtodthedreviewers"dcommentscdbedpublisheddonlinedatd http:DDwwwFjcseForgdindduedcourseFdUntildsuchdtimedasditdhasdbeendfullydpublishedditdshoulddnotdnormallydbedreferenceddindpublisheddworkFd 11 PDAPDAPDAPDA 35 0.0038 0.722 -3.418 0.978 02 45 0.0444 1.168 -10.028 0.978 38 55 0.0325 1.319 -9.493 0.985 51 dISSN 1466-8858 Volume 12, Preprint 18 submitted 11 May 2009d ©dMTT9dUniversitydofdManchesterdanddthedauthorsFdThisdisdadpreprintdofdadpaperdthatdhasdbeendsubmitteddfordpublicationdindthedJournaldofd CorrosiondSciencedanddEngineeringFdItdwilldbedrevieweddandcdsubjectdtodthedreviewers"dcommentscdbedpublisheddonlinedatd http:DDwwwFjcseForgdindduedcourseFdUntildsuchdtimedasditdhasdbeendfullydpublishedditdshoulddnotdnormallydbedreferenceddindpublisheddworkFd 12 0 2 4 6 8 10 12 14 16 C (g/l) Fig. 1 Langmuir Adsorption Isotherm for Cu-Ni Alloy in 5% HCl in Presence of NA 4681012141618202224 C/θ (g/l) 35 oC 45 55 -0.2 0.0 0.2 0.4 0.6 0.8 1.0 1.2 1.4 Log C Fig. 2 Freundlich Adsorption Isotherm of NA on Cu-Ni Alloy in 5% HCl Acid at Different Temperatures. -1.2-1.0-0.8-0.6-0.4-0.20.0 log θ 35oC 45 55 dISSN 1466-8858 Volume 12, Preprint 18 submitted 11 May 2009d ©dMTT9dUniversitydofdManchesterdanddthedauthorsFdThisdisdadpreprintdofdadpaperdthatdhasdbeendsubmitteddfordpublicationdindthedJournaldofd CorrosiondSciencedanddEngineeringFdItdwilldbedrevieweddandcdsubjectdtodthedreviewers"dcommentscdbedpublisheddonlinedatd http:DDwwwFjcseForgdindduedcourseFdUntildsuchdtimedasditdhasdbeendfullydpublishedditdshoulddnotdnormallydbedreferenceddindpublisheddworkFd 13 -0.2 0.0 0.2 0.4 0.6 0.8 1.0 1.2 1.4 Log C Fig. 3 Kinetic-Thermodynamic Model of NA on Cu-Ni Alloy in 5% HCl Acid at Different Temperatures. -1.2-1.0-0.8-0.6-0.4-0.20.00.20.40.60.81.0 log (θ/1-θ) 35oC 45 55 -0.2 0.0 0.2 0.4 0.6 0.8 1.0 1.2 1.4 Log C Fig. 4 Freundlich Adsorption Isotherm of EDA on Cu-Ni Alloy in 5% HCl Acid at Different Temperatures. -0.9-0.8-0.7-0.6-0.5-0.4-0.3-0.2-0.10.0 log θ 35oC 45 55 dISSN 1466-8858 Volume 12, Preprint 18 submitted 11 May 2009d ©dMTT9dUniversitydofdManchesterdanddthedauthorsFdThisdisdadpreprintdofdadpaperdthatdhasdbeendsubmitteddfordpublicationdindthedJournaldofd CorrosiondSciencedanddEngineeringFdItdwilldbedrevieweddandcdsubjectdtodthedreviewers"dcommentscdbedpublisheddonlinedatd http:DDwwwFjcseForgdindduedcourseFdUntildsuchdtimedasditdhasdbeendfullydpublishedditdshoulddnotdnormallydbedreferenceddindpublisheddworkFd 14 -0.2 0.0 0.2 0.4 0.6 0.8 1.0 1.2 1.4 Log C Fig. 5 Freundlich Adsorption Isotherm of TEPA on Cu-Ni Alloy in 5% HCl Acid at Different Temperatures. -0.9-0.8-0.7-0.6-0.5-0.4-0.3-0.2 log θ 35oC 45 55 -0.2 0.0 0.2 0.4 0.6 0.8 1.0 1.2 1.4 Log C Fig. 6 Kinetic-Thermodynamic Model of DETA on Cu-Ni Alloy in 5% HCl Acid at Different Temperatures. -1.6-1.4-1.2-1.0-0.8-0.6-0.4-0.20.0 log (θ/1-θ) 35oC 45 55 dISSN 1466-8858 Volume 12, Preprint 18 submitted 11 May 2009d ©dMTT9dUniversitydofdManchesterdanddthedauthorsFdThisdisdadpreprintdofdadpaperdthatdhasdbeendsubmitteddfordpublicationdindthedJournaldofd CorrosiondSciencedanddEngineeringFdItdwilldbedrevieweddandcdsubjectdtodthedreviewers"dcommentscdbedpublisheddonlinedatd http:DDwwwFjcseForgdindduedcourseFdUntildsuchdtimedasditdhasdbeendfullydpublishedditdshoulddnotdnormallydbedreferenceddindpublisheddworkFd 15 Conclusion:Conclusion:Conclusion:Conclusion: The corrosion rate of Cu-Ni alloy in 5% HCl acid solution, increased with increasing of temperature, and decreased with increasing of inhibitor concentration. NA was the relatively the most effective inhibitor than the other. Other chemicals (i.e. EDA, TEPA, DETA, and PDA) were ineffective inhibitors even at high level of inhibitor concentration (i.e. 15 g/l). NA, EDA, TEPA, and DETA appear to obey the Freundlich adsorption isotherm more than Langmuir adsorption isotherm. In the other hand, the two-adsorption isotherms were unsuitable to represent the data of PDA. Results also showed that the Kinetic- Thermodynamic Model was suitable to fit the experimental data of the most inhibitors of the present study. The values of y (i.e. the number of inhibitor molecules occupying one active site on the metal surface) obtained from the present work were near unity, which indicate the formation of monolayer on the metal surface. Values of heat of adsorption ()adsGΔwere lower in the cases, which indicate the weak binding of inhibitors to the metal surface. The order of inhibition of inhibitors evaluated by weight loss technique were as follows; NA > EDA > TEPA > DETA > PDA Acknowledgment:Acknowledgment:Acknowledgment:Acknowledgment: This work was supported by Universiti Kebangsaan Malaysia (Grant number: UKM-OUP-NBT-26-120/2008) which is gratefully acknowledged. ReferencesReferencesReferencesReferences [1] Da-Quan Zhang, Qi-Rui Cai, Li-Xin Gao, Kang Yong Lee (2008) Corros Sci 50505050: 3615- 3621. [2] Sherif E, Erasmus R M, Comins J D (2007 ) J. Colloid Interface Sci. 311311311311: 144. [3] Sherif E, Erasmus R M, Comins J D (2007) J. Colloid Interface Sci. 306306306306: 96. [4] Sherif E, Park S M (2006) J. Electrochim. Acta 51515151: 6556. [5] Sherif E, Park S M (2006) J. Electrochim. Acta 51515151: 4665. [6] Sastri V. S., 2001. Corrosion Inhibitors principles and applications, Johan Wiley & Sons publisher. [7] Fiala A, Chibani A, Darchen A, Boulkamh A., Djebbar K (2007) Appl. Surf. Sci. 253253253253:9347- 9356 [8] El-Egamy S S (2008) Corro. Sci. 50505050: 928-937 [9] Nageh K. Allam (2007) Appl. Surf. Sci. 253253253253: 4570-4577 [10] Unuabonah E I, Olu-Owolabi B I, Adebowale K O, Ofomaja A E (2007) Colloids and Surfaces A: Physicochem Eng Aspects 292292292292: 202-211 [11] Fouda A S, Al-Sarawy A A,Ahmed F Sh, El-Abbasy H M (2009) Corro. Sci .51515151: 485-492 [12] El-Awady A A, Abd-El-Nabey B A, Aziz S G (1992) J. Electochem.... Soc. 139139139139: 153. dISSN 1466-8858 Volume 12, Preprint 18 submitted 11 May 2009d ©dMTT9dUniversitydofdManchesterdanddthedauthorsFdThisdisdadpreprintdofdadpaperdthatdhasdbeendsubmitteddfordpublicationdindthedJournaldofd CorrosiondSciencedanddEngineeringFdItdwilldbedrevieweddandcdsubjectdtodthedreviewers"dcommentscdbedpublisheddonlinedatd http:DDwwwFjcseForgdindduedcourseFdUntildsuchdtimedasditdhasdbeendfullydpublishedditdshoulddnotdnormallydbedreferenceddindpublisheddworkFd 16 [13] El-Awady A A, Abd-El-Nabey B A, Aziz S G (1993) J. Chem. Soc. Faraday Trans. 89 898989:795. [14] Shereir, L. L., Corrosion, vol. 2, 2 nd edition, Newnes-Butterworths, London, 1977. [15] Clark, A., The Theory of Adsorption and Catalyst, Academic Press, New York (1970). [16] Scendo M (2007) Corros. Sci. 49494949:3953-3968. [17] Umoren S A, Ebenso E E (2007) Mate.r Chem. Phys. 106106106106: 393. [18] Umoren S A, Obot I B, Ebenso E E (2008) E-journal Chem. 5555:355. [19] Damaskin, W.W., Pietrij, O.A. & Batrakow, W.W, "Adsorption of Organic Compounds on Electrode", Plenum Press, New York (1971).