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\title{Chemical and Electrochemical Study on the Effectively of Melilotus Officinalis Extract as Save Corrosion Inhibitor for Aluminium in 1 M Hydrochloric Acid Solutions}
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             \author[1]{  A.S.Fouda}

             \affil[1]{  Mansoura University}

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\date{\small \em Received: 11 April 2015 Accepted: 4 May 2015 Published: 15 May 2015}

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\begin{abstract}
        


Melilotus officinalis Extract (MOE), was investigated as a green corrosion inhibitor for aluminium in 1 M HCl solution using weight loss, hydrogen evolution, potentiodynamic polarization, electrochemical impedance spectroscopy (EIS) and electrochemical frequency modulation (EFM) techniques. Surface morphology was tested using scanning electron microscope (SEM). The effect of the temperature on corrosion behavior with addition of different concentrations was studied in the temperature range of 25-45 ºC by weight loss method. Polarization curves reveal that the investigated extract is a mixed type inhibitor. The inhibition efficiency was found to increase with increase in the investigated extract concentration and increase with increase in solution temperature. The adsorption of the inhibitor on aluminium surface was found to obey the Temkin?s adsorption isotherm. The activation and adsorption parameters were calculated and discussed. The results obtained from chemical and electrochemical techniques are in good agreement.

\end{abstract}


\keywords{acidic corrosion, aluminium, melilotus officinalis extract, EIS, EFM, SEM.}

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\let\tabcellsep& 	 	 		 
\section[{I. Introduction}]{I. Introduction}\par
orrosion is a fundamental process playing an important role in economics and safety? particularly for metals. The use of inhibitors is one of the most practical methods for protection against corrosion? especially in acidic media \hyperref[b0]{[1]}. Most wellknown acid inhibitor are organic compounds containing nitrogen ? sulfur? and oxygen atoms. Among them? organic inhibitors have many advantages such as high inhibition efficiency and easy production \hyperref[b1]{[2]}\hyperref[b2]{[3]}\hyperref[b3]{[4]}\hyperref[b4]{[5]}. Organic heterocyclic compounds have been used for the corrosion inhibition of iron \hyperref[b5]{[6]}\hyperref[b6]{[7]}\hyperref[b7]{[8]}\hyperref[b8]{[9]}, copper \hyperref[b10]{[10]}, aluminum \hyperref[b11]{[11]}\hyperref[b12]{[12]}\hyperref[b13]{[13]}, and other metals \hyperref[b14]{[14]}\hyperref[b15]{[15]} in different corroding media. Although many of these compounds have high inhibition efficiencies, several have undesirable side effects, even in very small concentrations, due to their toxicity to humans, deleterious environmental effects, and high-cost \hyperref[b16]{[16]}.\par
Plant extract is low-cost and environmental safe, so the main advantages of using plant extracts as corrosion inhibitor are economic and safe environment. Up till now, many plant extracts have been used as effective corrosion inhibitors for aluminium in acidic media, such as: Garlic \hyperref[b17]{[17]}, Black Mulberry \hyperref[b18]{[18]}, Piper Guineense seed \hyperref[b19]{[19]} Red onion skin \hyperref[b20]{[20]}. The inhibition performance of plant extract is normally ascribed to the presence of complex organic species, including tannins, alkaloids and nitrogen bases, carbohydrates and proteins as well as hydrolysis products in their composition. These organic compounds usually contain polar functions with nitrogen, sulfur, or oxygen atoms and have triple or conjugated double bonds with aromatic rings in their molecular structures, which are the major adsorption centers.\par
Melilotus officinalis extract (MOE), belongs to the family Leguminosae (Fabaceae). It exhibits several medicinal properties, this plant is mainly used for agricultural purposes. It is grown as hay despite its toxic properties when moldy. It is considered an excellent green manure. Sweet clover is a major source of nectar for domestic honey bees. Flowers and seeds can be used as flavoring Melilotus officinalis has been used as a phytoremediation-phytodegradation plant for treatment of soils contaminated with dioxins \hyperref[b21]{[21]}.\par
The present work was designed to study the inhibitory action of Melilotus officinalis for the corrosion of aluminium in 1 M HCl using Chemical and electrochemical techniques, and to study the effect of temperature on the rate of corrosion II. Experimental Methods 
\section[{a) Materials and Solutions}]{a) Materials and Solutions}\par
Aluminium used has the chemical composition (\% weight) 0.30 Si; 0.60 Fe; 0.10 Cu; 1.40 Mn; 0.05 Mg; 0.05 Cr; 0.05 Ti and the rest aluminium. The auxiliary electrode was a platinum wire (1 cm 2 ), while a saturated calomel electrode (SCE) connected to a conventional electrolytic cell of capacity 100 ml via a bridge with a Luggin capillary, the tip of which was very close to the surface of the working electrode to minimize the IR drop. The aggressive solution used was prepared by dilution of analytical reagent grade 37\% HCl with bidistilled water. The stock solution (1000 ppm) of Melilotus officinalis was used to prepare the desired concentrations by dilution with bidistilled water. The concentration range of MOE used was 50-300 ppm. 
\section[{b) Preparation of plant extracts}]{b) Preparation of plant extracts}\par
Fresh aerial parts of MOE sample were crushed to make fine powder. The powdered materials (250 g) were soaked in 500 ml of dichloromethane for 5 days and then subjected to repeated extraction with 5× 50 ml until exhaustion of plant materials. The extracts obtained were then concentrated under reduced pressure using rotary evaporator at temperature below 50°C. The dichloromethane evaporated to give solid extract that was prepared for application as corrosion inhibitor. Chemical studies have demonstrated that the main chemical constituents of Melilotus officinalis are the glycosides of coumaric acid, especially melitoside, which by hydrolysis of lactonises gives coumarin. Free coumarin, 3,4-dihydroxycoumarin (melilotin), scopoletin and umbelliferone are also present \hyperref[b22]{[22]}. 
\section[{c) Weight loss measurements}]{c) Weight loss measurements}\par
Seven parallel aluminium sheets of 2×2×0.2 cm were abraded with emery paper (grade 320-500-1200) and then washed with bidistilled water and acetone. After accurate weighing, the specimens were immersed in a 250 ml beaker, which contained 100 ml of HCl with and without addition of different concentrations of Melilotus officinalis. All the aggressive acid solutions were open to air. After 180 minutes, the specimens were taken out, washed, dried, and weighed accurately. The average weight loss of seven parallel aluminium sheets could be obtained. The inhibition efficiency (IE\%) and the degree of surface coverage, ? of MOE for the corrosion of Al were calculated as follows \hyperref[b23]{[23]}:????\% = ?? × 100 = ?1 ? ?? ?? °? × 100\textbf{(1)}\par
where Wº and W are the values of the average weight losses without and with addition of the inhibitor, respectively. 
\section[{d) Gasometric measurements}]{d) Gasometric measurements}\par
The gasometric method assembly used for the measurement of hydrogen gas evolution from the corrosion reaction was designed following the method described by Onuchukwu \hyperref[b24]{[24]}. The gasometric assembly measures the volume of hydrogen gas evolution from the reaction system. Sevenaluminium coupons of dimension 2 x 2 x 0.2cm were used in the experiments for test solutions containing 1 M HCl with the six different concentrations of MOE and the blank at 25 o C. A 50ml of each test solution was introduced into the reaction vessel connected to a burette through a delivery tube. The initial volume of air in the burette was recorded. Thereafter, one aluminium coupon was dropped into the corrodent and the reaction vessel quickly closed. Variation in the volume of hydrogen gas evolved with time was recorded every 1min. for 80 min. Each experiment was conducted on a fresh specimen of metal coupon. The hydrogen gas evolved displaced the paraffin water in the gasometric set-up and the displacement representing the volume of hydrogen evolved was read directly. The experiment was repeated in the presence of the six different concentrations of MOE, 50 to 300 ppm asused in the weight loss experiments. 
\section[{e) Electrochemical measurements}]{e) Electrochemical measurements}\par
Electrochemical measurements were performed using a typical three-compartments glass cell consisting of the aluminium specimen as working electrode (1 cm 2 ), saturated calomel electrode (SCE) as a reference electrode, and a platinum wire as a counter electrode. The reference electrode was connected to a Luggin capillary and the tip of the Luggin capillary is made very close to the surface of the working electrode to minimize IR drop. All the measurements were done in solutions open to atmosphere under unstirred conditions. All potential values were reported versus SCE. Prior to each experiment, the electrode was abraded with successive different grades of emery paper, degreased with acetone, also washed with bidistilled water, and finally dried. Tafel polarization curves were obtained by changing the electrode potential automatically from (-0.8 to 1 V vs. SCE) at open circuit potential with a scan rate of 1 mVs -1 . Stern-Geary method \hyperref[b25]{[25]}, used for the determination of corrosion current is performed by extrapolation of anodic and cathodic Tafel lines to a point which gives (log i corr ) and the corresponding corrosion potential (E corr ) for inhibitor free acid and for each concentration of inhibitor. Then (i corr ) was used for calculation of inhibition efficiency (IE \%) and surface coverage (?) as in equation 2:????\% = ? × 100 = ?1 ? ?? ???????? (???? ? ) i???????? (ð??"ð??"??ð??"ð??"ð??"ð??" ) ? × 100\textbf{(2)}\par
Where i corr(free) and i corr(inh) are the corrosion current densities in the absence and presence of inhibitor, respectively.\par
Impedance measurements were carried out in frequency range (2x10 4 Hz to 8x10 -2 Hz) with amplitude of 5 mV peak-to-peak using AC signals at open circuit potential. The experimental impedance was analyzed and interpreted based on the equivalent circuit. The main parameters deduced from the analysis of Nyquist diagram are the charge transfer resistance R ct (diameter of high-frequency loop) and the double layer capacity C dl . The inhibition efficiencies and the surface coverage (?) obtained from the impedance measurements are calculated from equation 3:\par
Where R o ct and R ct are the charge transfer resistance in the absence and presence of inhibitor, respectively.\par
Electrochemical frequency modulation, EFM, was carried out using two frequencies 2 and 5 Hz. The large peaks were used to calculate the corrosion current density (i corr ), the Tafel slopes (? a and ? c ) and the causality factors CF-2\&CF-3 \hyperref[b26]{[26]}. The electrode potential was allowed to stabilize 30 min before starting the measurements. All the experiments were conducted at 25°C.\par
All electrochemical measurements were performed using Gamry Instrument (PCI4/750) Potentiostat/ Galvanostat/ZRA. This includes a Gamry framework system based on the ESA 400. Gamry applications include DC105 software for potentiodynamic polarization, EIS 300 software for electrochemical impedance spectroscopy, and EFM 140 software for electrochemical frequency modulation measurements via computer for collecting data. Echem Analyst 6.03 software was used for plotting, graphing, and fitting data. To test the reliability and reproducibility of the measurements, duplicate experiments, which performed in each case at the same conditions. 
\section[{f) Surface morphology}]{f) Surface morphology}\par
For morphological study, surface features (2 x 2 x 0.2cm) of aluminium were examined before and after exposure to 1 M HCl solutions for 24 hour with and without extract. JEOL JSM-5500 scanning electron microscope was used for this investigation. 
\section[{III. Results and Discussion}]{III. Results and Discussion} 
\section[{a) Weight loss measurements}]{a) Weight loss measurements}\par
Weight loss measurements were carried out for aluminium in 1 M HCl in the absence and presence of different concentrations of Melilotus officinalis and are shown in Figure \hyperref[b0]{(1)}. The inhibition efficiency (IE\%) values calculated are listed in Table \hyperref[b0]{(1)}. From this table, it is noted that the IE\% increases steadily with increasing the concentration of Melilotus officinalis and with increasing temperature from 25-45ºC. The inhibition efficiency (IE\%) and surface coverage (?)were calculated by equation \hyperref[b0]{(1)}. The observed inhibition action of the MOE could be attributed to the adsorption of its components on aluminium surface. The formed layer, of the adsorbed molecules, isolates the metal surface from the aggressive medium which limits the dissolution of the latter by blocking of their corrosion sites and hence decreasing the corrosion rate, with increasing efficiency as their concentrations increase \hyperref[b27]{[27]}. as the incubation period. Further inspection of Figure \hyperref[fig_1]{2} reveals linear relationship between the time of reaction and the volume of hydrogen evolved, in all of the tested solutions. However, the presence of the extract decreases, markedly, the slope of the straight line. Since the slope of the line represents the corrosion reaction rate, it could be concluded that the Melilotus offecinalis extract has an excellent ability to inhibit the corrosion of aluminium in the acid solution. The values of inhibition efficiencies of different concentrations of the extract are given in \hyperref[tab_2]{Table 2}   Lee and Nobe \hyperref[b28]{[28]} reported the occurrence of a current peak between the apparent-Tafel and limitingcurrent regions during potential sweep experiments. The presence of MOE shifts both anodic and cathodic branches to the lower values of corrosion current densities and thus causes a remarkable decrease in the corrosion rate. The parameters derived from the polarization curves in Figure \hyperref[fig_2]{3} are given in Table \hyperref[tab_4]{3}. In 1 M HCl solution, the presence of MOE causes a remarkable decrease in the corrosion rate i.e., shifts both anodic and cathodic curves to lower current densities. In other words, both cathodic and anodic reactions of aluminium electrode are retarded by MOE in 1 M HCl solution. The Tafel slopes of ? a and ? c at 25ºCdo not change remarkably upon addition of MOE, which indicates that the presence of MOE does not change the mechanism of hydrogen evolution and the metal dissolution process. Generally, an inhibitor can be classified as cathodic type if the shift of corrosion potential in the presence of the inhibitor is more than 85 mV with respect to that in the absence of the inhibitor \hyperref[b29]{[29,}\hyperref[b30]{30]}. In the presence of MOE, E corr shifts to less negative but this shift is very small (about 20-30 mV), which indicates that MOE can be arranged as mixed inhibitor.    
\section[{d) Electrochemical impedance spectroscopy (EIS) measurements}]{d) Electrochemical impedance spectroscopy (EIS) measurements}\par
Figure  {\ref 4} shows impedance plots for aluminium in 1 M HClsolution without and with different concentrations of MOE. The impedance spectra consists of a Nyquist semicircle type without appearance of diffusive contribution to the total impedance (Z) indicating that the corrosion proceeds mainly under charge-transfer control and the presence of extract do not alter the mechanism of corrosion reaction.It is found that the obtained Nyquist plots are not perfect semicircle due to frequency dispersion and this behavior can be attributed to roughness and in homogeneities of the electrode surface \hyperref[b31]{[31,}\hyperref[b32]{32]}. When there is non-ideal frequency response, it is common practice to use distributed circuit elements in an equivalent circuit. The most widely employed is the constant phase element (CPE). In general a CPE is used in a model in place of a capacitor to compensate for inhomogeneity in the system \hyperref[b33]{[33]}. It was found that the diameters of the semicircle increases with increasing the concentration of the investigated extract. This indicates that the polarization resistance of the oxide layer increases with increasing the concentration of MOE and the depressed capacitive semicircle are often referred to the surface roughness and inhomogeneity, since this capacitive semicircle is correlated with dielectric properties and thickness of the barrier oxide film \hyperref[b34]{[34]}. The data revealed that, each impedance diagram consists of a large capacitive loop with low frequencies dispersion (inductive arc). This inductive arc is generally attributed to anodic adsorbed intermediates controlling the anodic process \hyperref[b35]{[35]}\hyperref[b36]{[36]}. By following this, inductive arc was disregarded. The electrical equivalent circuit model shown in Figure  {\ref 5}  solution resistance (R s ), the charge-transfer resistance of the interfacial corrosion reaction (R ct ) and the constant phase angle element (CPE). The value of frequency power (n) of CPE can be assumed to correspond to capacitive behavior. However, excellent fit with this model was obtained with our experimental data. The admittance of CPE is described as:?? ?????? = ?? ?? (????) n (\textbf{4})\par
where j is the imaginary root, ? the angular frequency, Y o the magnitude and n the exponential term \hyperref[b37]{[37]}. A long Warburg diffusion tail was observed at low frequency values. The tails are inclined at an angle of 45 o to the real-axis at the very low frequencies; A diffusion controlled process is therefore exists. Studies reported in the literature \hyperref[b38]{[38]} showed that the diffusion process is controlled by diffusion of dissolved oxygen from the bulk solution to the electrode surface and the Warburg impedance, which is observed in the low frequency regions, is ascribed to diffusion of oxygen to the alloy surface. This diffusion tail still appears, even in presence of high concentrations of the investigated extract. This means that the corrosion behavior of alloy in the absence as well as in the presence of MOE is influenced by mass transport. Also, Bode plots for the aluminium in 1 M HCl solution are shown in Figure 6. In which the high frequency limit corresponding to the electrolyte resistance (ohmic resistance) R ? , while the low frequency represents the sum of (R ? + R ct ), where R ct is in the first approximation determined by both electrolytic conductance of the oxide film and the polarization resistance of the dissolution and repassivation process. At both low and high frequency limits, the phase angle between the current and potential (?), assumes a value of about 0°, corresponding to the resistive behavior of R ? and (R ? + R ct ). The main parameters deduced from the analysis of Nyquist diagram are:\par
? The resistance of charge transfer R ct (diameter of high frequency loop)\par
? The capacity of double layer C dl which is defined as :C dl = 1 2???? ???? ð??"ð??" ??????\textbf{(5)}\par
Where f max is the maximum frequency at which the Z imag of the impedance is a maximum. Since the electrochemical theory assumed that (1/R ct ) is directly proportional to the capacity of double layer C dl , the inhibition efficiency (IE\%) of the inhibitor for aluminium in 1 M HCl solution was calculated from R ct values obtained from impedance data at different inhibitor concentration the following equation:????\% = ?1 ? ?? ???? °?????? ? × 100\textbf{(6)}\par
Where R o ct and R ct are the charge transfer resistance in the absence and Presence of investigated extract, respectively. From the impedance data given in Table \hyperref[tab_5]{4}, we can conclude that the value of R ct increases with the increase in the concentration of the investigated extract and this indicates the formation of a protective film on the Al surface by the adsorption and an increase in the corrosion inhibition efficiency in acidic solution. While the value of C dl decreases with increasing the concentrations of extract in comparison with that of blank solution (uninhibited), as a result from the replacement of water molecules by inhibitor molecules which lead to increase in local dielectric constant and/or an increase in the thickness of the electric double layer formed on the metal surface \hyperref[b39]{[39,}\hyperref[b40]{40]}.  
\section[{e) Electrochemical frequency modulation (EFM) measurements}]{e) Electrochemical frequency modulation (EFM) measurements}\par
EFM is a nondestructive corrosion measurement technique that can directly determine the corrosion current value without prior knowledge of Tafel slopes, and with only a small polarizing signal. These advantages of EFM technique make it an ideal candidate for online corrosion monitoring \hyperref[b41]{[41]}. The great strength of the EFM is the causality factors which serve as an internal check on the validity of EFM measurement. The causality factors CF-2 and CF-3 are e XV Issue III Version I ( ) C calculated from the frequency spectrum of the current responses. Figure 7 show the frequency spectrum of the current response of pure Aluminium in 1 M HCl solution, contains not only the input frequencies, but also contains frequency components which are the sum, difference, and multiples of the two input frequencies. The EFM intermodulation spectrums of Aluminium in 1 M HCl solution containing (50ppm-300ppm) of the MOE extract at 25 °C is shown in Figure 7. The harmonic and intermodulation peaks are clearly visible and are much larger than the background noise. The two large peaks, with amplitude of about 200 µA, are the response to the 40 and 100 mHz (2 and 5 Hz) excitation frequencies. It is important to note that between the peaks there is nearly no current response (<100 mA). The experimental EFM data were treated using two different models: complete diffusion control of the cathodic reaction and the "activation" model. For the latter, a set of three nonlinear equations had been solved, assuming that the corrosion potential does not change due to the polarization of the working electrode \hyperref[b42]{[42]}. The larger peaks were used to calculate the corrosion current density (i corr ), the Tafel slopes (? c and ? a ) and the causality factors (CF-2 and CF-3).These electrochemical parameters were simultaneously determined by Gamry EFM 140 software, and listed in Table \hyperref[tab_6]{5} indicating that this extract inhibit the corrosion of aluminium in 1 M HCl through adsorption. The causality factors obtained under different experimental conditions are approximately equal to the theoretical values (2 and 3) indicating that the measured data are verified and of good quality \hyperref[b43]{[43]}. The inhibition efficiencies IE EFM \% increase by increasing the studied extract concentrations and was calculated as follows:???? \% ??????= ?1? ?? ????????\par
?? ???????? °?×100 \hyperref[b6]{(7)} Where i o corr and i corr are corrosion current densities in the absence and presence of MOE extract, respectively.  The mode and interaction degree between an inhibitor and a metallic surface have been widely studied with the application of adsorption isotherms. The adsorption of an organic molecule occurs because the interaction energy between an inhibitor and a metallic surface is higher than that between water molecules and metallic surface \hyperref[b44]{[44,}\hyperref[b45]{45]}. To obtain the adsorption isotherms, the degree of surface coverage (?) obtained from weight loss method was determined as a function of inhibitor concentration. The values of ? were then plotted to fit the most suitable model of adsorption \hyperref[b46]{[46]}. Attempts were made to fit experimental data to various isotherms including Frumkin, Langmuir, Temkin, Freundlich, isotherms. By far the results were best fitted by Temkin adsorption isotherm as seen in Figure 7 \hyperref[b47]{[47]}. a/2.303?= logK ads + logC \hyperref[b8]{(9)} The equilibrium constant of adsorption K ads obtained from the intercepts of Temkin adsorption isotherm is related to the free energy of adsorption Î?"G° ads as follows:K ads =1/55.5 exp[(-Î?"G°a ds )/ RT]\textbf{(8)}\par
where 55.5 is the molar concentration of water in the solution in M -1 .The values obtained are given in Table \hyperref[tab_7]{6}.\par
The equilibrium constant of adsorption K ads obtained from the intercepts of Temkin adsorption   \hyperref[tab_7]{6} clearly shows a good dependence of Î?"G o ads on T, indicating the good correlation among thermodynamic parameters. The negative value of Î?"G o ads reflect that the adsorption of studied inhibitors on aluminium surface from 1 M HCl solution is spontaneous process and stability of the adsorbed layer on the aluminium surface. Generally, values of Î?"G o ads around -20 kJ mol -1 or lower are consistent with the electrostatic interaction between the charged molecules and the charged metal (physical adsorption); those around -40 kJ mol -1 or higher involves charge sharing or transfer from organic molecules to the metal surface to form a coordinate type of bond (chemisorption) \hyperref[b48]{[48]}.\par
From the obtained values of Î?"G°a ds it was found the existence of chemical adsorption). The values of thermodynamic parameter for the adsorption of inhibitors Table \hyperref[tab_7]{6} can provide valuable information about the mechanism of corrosion inhibition. Endothermic adsorption process (Î?"H o ads > 0) is attributed unequivocally to chemisorption \hyperref[b49]{[49]}, an exothermic adsorption process (Î?"H o ads < 0) may involve either physisorption or chemisorption or mixture of both processes. In the presented case, the calculated values of Î?"H o ads for the adsorption of extract in 1 M HCl indicating that this extract may be chemically adsorbed. The values of Î?"S°a ds in the presence of extract is large and positive that is accompanied with endothermic adsorption process. This indicates that decrease in disorder takes places on going from reactants to the metal-adsorbed reaction complex \hyperref[b50]{[50]}.  g) Kinetic-thermodynamic corrosion parameters Weight loss method was carried out at different temperature (25 °C-45 °C) in the presence of different concentration of MOE. It has been found that he corrosion rate decreases with the increase in temperature for MOE (Table \hyperref[tab_1]{1}). The corrosion rate of aluminium in the absence of MOE increased steeply from 25 to 45 °Cwhereas; in the presence of MOE the corrosion rate decreased slowly. The inhibition efficiency was found to increase with temperature. The corrosion parameter in the absence and presence of extract in the temperature range 25-45 °C has been summarized in (Table \hyperref[tab_1]{1}).The apparent activation energy (E * a ) for dissolution of aluminium in 1 M HCl was calculated from the slope of plots by using Arrhenius equation:log ?? = ??? ?? * 2.303 ?? ?? + log ??\textbf{(9)}\par
where k is rate of corrosion, E * a is the apparent activation energy, R is the universal gas constant, T is absolute temperature and A is the Arrhenius preexponential factor.\par
By plotting log k against 1/T the values of activation energy (E * a ) has been calculated (E * a = (slope) 2.303 x R) (Figure  {\ref 9}). Activation energy for the reaction of aluminium in 1M HCl decreases in the presence of extract (Table \hyperref[tab_8]{7}). This decreas indicates the formation of chemical bonds were strengthen by increasing the temperature. However, the extent of the rate increment in the inhibited solution is lower than that in the free acid solution. Therefore, the inhibition efficiency of the MOE increases markedly with increasing temperature. This result supports the idea that the adsorption of extract components on the aluminium surface may be chemical in nature. Thus, as the temperature increases the number of adsorbed molecules increases leading to an increase in the inhibition efficiency. This could be done by adsorption on the aluminium surface making a barrier for mass and charge transfer. However, such types of inhibitors perform a good inhibition at high temperature with considerable increase in inhibition efficiency at elevated temperatures \hyperref[b51]{[51]}. Moreover, the relatively high value of activation energy in presence of MOE suggests a chemical adsorption process.\par
The values of change of entropy (Î?"S * ) and change of enthalpy (Î?"H * ) can be calculated by using the formula:?? = ? ???? ??? ? ð??"ð??"???? ? ??? * ?? ? ð??"ð??"???? ? ??? * ???? ? (\textbf{10})\par
where k is rate of corrosion, h is Planck's constant, N is Avogadro number, Î?"S * is the entropy of activation, and Î?"H * is the enthalpy of activation. A plot of log (k/T) vs. 1/T (Figure \hyperref[fig_0]{10}) should give a straight line, with a slope of (Î?"H * /2.303R) and an intercept of [log (R/Nh)+Î?"S * / 2.303R], from which the values of Î?"S * and Î?"H * can be calculated (Table \hyperref[tab_8]{7}). The positive value of Î?"S * for the extract indicates that activated complex in the rate determining step represents a dissociation rather than an association step, meaning that an increase in disorder takes place during the course of transition from reactant to the activated complex \hyperref[b52]{[52]} The positive sign of Î?"H * indicates that the adsorption of extract molecules is an endothermic process. Generally, an endothermic process signifieschemisorption process.   11b. The faceting seen in this figures was a result of pits formed due to the exposure of aluminium to the acid. The influence of the inhibitor addition 300 ppm on the aluminium in 1 M HCl solution is shown in Figure 11c. The morphology in Figure 11c shows a rough surface, characteristic of uniform corrosion of aluminium in acid, as previously reported \hyperref[b52]{[52]}, that corrosion does not occur in presence of inhibitor and hence corrosion was inhibited strongly when the inhibitor was present in the hydrochloric acid, and the surface layer is very rough. In contrast, in the presence of 300 ppm of MOE, there is much less damage on the aluminium surface, which further confirm the inhibition action. Also, there is an adsorbed film adsorbed on aluminium surface (Figure 11c). In accordance, it might be concluded that the adsorption film can efficiently inhibits the corrosion of aluminium.  
\section[{i) Mechanism of the corrosion inhibition}]{i) Mechanism of the corrosion inhibition}\par
The adsorption of organic compounds can be described by two main types of interactions: physical and chemisorptions adsorption. In general, physical adsorption requires the presence of both the electrically charged surface of the metal and charged species in solution. The surface charge of the metal is due to the electric field existing at the metal/solution interface. A chemisorption process, on the other hand, involves charge sharing or charge transfer from the inhibitor molecules to the metal surface to form a coordinate type of a bond. This is possible in case of a positive as well as a negative charge of the surface. The presence of a transition metal, having vacant, low-energy electron orbitals and an inhibitor with molecules having relatively loosely bound electrons or heteroatoms with a lone pair of electrons is necessary for the inhibiting action \hyperref[b53]{[53]}. Generally, two types of mechanisms of inhibition were proposed. One was the formation of polymeric complexes with aluminium ions (Al 3+ ) depending on the applied conditions \hyperref[b54]{[54,}\hyperref[b55]{55]}. The other was the chemical adsorption of MOE components on aluminium surface e XV Issue III Version I ( ) C \hyperref[b56]{[56,}\hyperref[b57]{57]}. The inhibition action of MOE does not occur by the simple blocking at the surface of aluminium, especially at high temperature. This might be attributed to the different adsorption capacities of the MOE extract on the aluminium surface at different temperatures. It has been studied that with the increase in temperature, the desorption effect of MOE on aluminium surface increased. Some of the hydrophilic groups with positively charged atoms (O + ) desorbed from the surface of aluminium and did more work to prevent the H + from getting nearer to the metal surface. Therefore, MOE preferentially inhibited both cathodic and anodic corrosion processes at high temperature. 
\section[{IV. Conclusions}]{IV. Conclusions}\par
From the overall experimental results the following conclusions can be deduced:\par
1. The MOE shows good performance as corrosion inhibitor in 1 M HCl. 2. The results obtained from weight loss showed that the inhibiting action increases with the MOE concentration and also increase with the increasing in temperature. 3. Double layer capacitances decrease with respect to blank solution when the plant extract is added. This fact confirms the adsorption of plant extract molecules on the aluminium surface. \begin{figure}[htbp]
\noindent\textbf{1}\includegraphics[]{image-2.png}
\caption{\label{fig_0}Figure 1 :}\end{figure}
 \begin{figure}[htbp]
\noindent\textbf{2}\includegraphics[]{image-3.png}
\caption{\label{fig_1}Figure 2 :}\end{figure}
 \begin{figure}[htbp]
\noindent\textbf{3}\includegraphics[]{image-4.png}
\caption{\label{fig_2}Figure 3 :}\end{figure}
 \begin{figure}[htbp]
\noindent\textbf{}\includegraphics[]{image-5.png}
\caption{\label{fig_3}}\end{figure}
 \begin{figure}[htbp]
\noindent\textbf{45}\includegraphics[]{image-6.png}
\caption{\label{fig_4}Figure 4 :Figure 5 :}\end{figure}
 \begin{figure}[htbp]
\noindent\textbf{}\includegraphics[]{image-7.png}
\caption{\label{fig_5}}\end{figure}
        \begin{figure}[htbp]
\noindent\textbf{} \par 
\begin{longtable}{P{0.85\textwidth}}
III Version I\\
e XV Issue\\
( )\end{longtable} \par
 
\caption{\label{tab_0}C}\end{figure}
 \begin{figure}[htbp]
\noindent\textbf{1} \par 
\begin{longtable}{P{0.009491315136476426\textwidth}P{0.12233250620347394\textwidth}P{0.17295285359801488\textwidth}P{0.20880893300248138\textwidth}P{0.1708436724565757\textwidth}P{0.009491315136476426\textwidth}P{0.003163771712158809\textwidth}P{0.1444789081885856\textwidth}P{0.008436724565756823\textwidth}}
Temp. o C\tabcellsep {}[Inh] ppm\tabcellsep Weight loss, mg cm -2\tabcellsep k corr, mg cm -2 min -1\tabcellsep \tabcellsep \multicolumn{2}{l}{?}\\
\tabcellsep Blank\tabcellsep 3.24\tabcellsep 0.027\tabcellsep -\tabcellsep \multicolumn{2}{l}{----}\tabcellsep -\tabcellsep ----\\
\tabcellsep 50\tabcellsep 1.48\tabcellsep 0.012\tabcellsep \multicolumn{3}{l}{0.544}\tabcellsep 54.4\\
\tabcellsep 100\tabcellsep 1.46\tabcellsep 0.012\tabcellsep \multicolumn{3}{l}{0.546}\tabcellsep 54.6\\
\tabcellsep 150\tabcellsep 1.41\tabcellsep 0.011\tabcellsep \multicolumn{3}{l}{0.560}\tabcellsep 56.0\\
\tabcellsep 200\tabcellsep 1.31\tabcellsep 0.011\tabcellsep \multicolumn{3}{l}{0.599}\tabcellsep 59.9\\
\tabcellsep 250\tabcellsep 1.30\tabcellsep 0.011\tabcellsep \multicolumn{3}{l}{0.595}\tabcellsep 59.5\\
\tabcellsep 300\tabcellsep 1.20\tabcellsep 0.010\tabcellsep \multicolumn{3}{l}{0.623}\tabcellsep 62.3\\
\tabcellsep Blank\tabcellsep 7.44\tabcellsep 0.062\tabcellsep \multicolumn{3}{l}{----}\tabcellsep -----\\
\tabcellsep 50\tabcellsep 2.55\tabcellsep 0.021\tabcellsep \multicolumn{3}{l}{0.657}\tabcellsep 65.7\\
\tabcellsep 100\tabcellsep 2.41\tabcellsep 0.020\tabcellsep \multicolumn{3}{l}{0.674}\tabcellsep 67.4\\
\tabcellsep 150\tabcellsep 2.22\tabcellsep 0.020\tabcellsep \multicolumn{3}{l}{0.701}\tabcellsep 70.1\\
\tabcellsep 200\tabcellsep 1.81\tabcellsep 0.018\tabcellsep \multicolumn{3}{l}{0.757}\tabcellsep 75.7\\
\tabcellsep 250\tabcellsep 1.73\tabcellsep 0.014\tabcellsep \multicolumn{3}{l}{0.767}\tabcellsep 76.7\\
\tabcellsep 300\tabcellsep 1.66\tabcellsep 0.013\tabcellsep \multicolumn{3}{l}{0.776}\tabcellsep 77.6\\
\tabcellsep Blank\tabcellsep 23.67\tabcellsep 0.198\tabcellsep \multicolumn{2}{l}{-}\tabcellsep ---\tabcellsep -\tabcellsep ----\\
\tabcellsep 50\tabcellsep 6.70\tabcellsep 0.055\tabcellsep \multicolumn{3}{l}{0.717}\tabcellsep 71.7\\
\tabcellsep 100\tabcellsep 6.49\tabcellsep 0.054\tabcellsep \multicolumn{3}{l}{0.726}\tabcellsep 72.6\\
\tabcellsep 150\tabcellsep 6.10\tabcellsep 0.050\tabcellsep \multicolumn{3}{l}{0.744}\tabcellsep 74.4\\
\tabcellsep 200\tabcellsep 5.24\tabcellsep 0.043\tabcellsep \multicolumn{3}{l}{0.778}\tabcellsep 77.8\\
\tabcellsep 250\tabcellsep 4.87\tabcellsep 0.040\tabcellsep \multicolumn{3}{l}{0.794}\tabcellsep 79.4\\
\tabcellsep 300\tabcellsep 4.39\tabcellsep 0.036\tabcellsep \multicolumn{3}{l}{0.814}\tabcellsep 81.4\\
\tabcellsep Blank\tabcellsep 34.92\tabcellsep 0.291\tabcellsep \multicolumn{3}{l}{-----}\tabcellsep -----\\
\tabcellsep 50\tabcellsep 5.82\tabcellsep 0.049\tabcellsep \multicolumn{3}{l}{0.834}\tabcellsep 83.4\\
\tabcellsep 100\tabcellsep 5.39\tabcellsep 0.044\tabcellsep \multicolumn{3}{l}{0.845}\tabcellsep 84.5\\
\tabcellsep 150\tabcellsep 4.55\tabcellsep 0.037\tabcellsep \multicolumn{3}{l}{0.869}\tabcellsep 86.9\\
\tabcellsep 200\tabcellsep 4.10\tabcellsep 0.034\tabcellsep \multicolumn{3}{l}{0.883}\tabcellsep 88.3\\
\tabcellsep 250\tabcellsep 3.65\tabcellsep 0.030\tabcellsep \multicolumn{3}{l}{0.895}\tabcellsep 89.5\\
\tabcellsep 300\tabcellsep 3.25\tabcellsep 0.027\tabcellsep \multicolumn{3}{l}{0.907}\tabcellsep 90.7\\
\tabcellsep Blank\tabcellsep 51.96\tabcellsep 0.433\tabcellsep -\tabcellsep \multicolumn{2}{l}{----}\tabcellsep -----\\
\tabcellsep 50\tabcellsep 8.10\tabcellsep 0.068\tabcellsep \multicolumn{3}{l}{0.845}\tabcellsep 84.5\\
\tabcellsep 100\tabcellsep 7.35\tabcellsep 0.061\tabcellsep \multicolumn{3}{l}{0.858}\tabcellsep 85.8\\
\tabcellsep 150\tabcellsep 6.50\tabcellsep 0.054\tabcellsep \multicolumn{3}{l}{0.874}\tabcellsep 87.4\\
\tabcellsep 200\tabcellsep 5.57\tabcellsep 0.046\tabcellsep \multicolumn{3}{l}{0.893}\tabcellsep 89.3\\
\tabcellsep 250\tabcellsep 4.75\tabcellsep 0.039\tabcellsep \multicolumn{3}{l}{0.908}\tabcellsep 90.8\\
\tabcellsep \tabcellsep 3.80\tabcellsep 0.032\tabcellsep \multicolumn{3}{l}{0.926}\tabcellsep 92.6\end{longtable} \par
 
\caption{\label{tab_1}Table 1 :}\end{figure}
 \begin{figure}[htbp]
\noindent\textbf{2} \par 
\begin{longtable}{P{0.23114035087719298\textwidth}P{0.39517543859649124\textwidth}P{0.22368421052631576\textwidth}}
{}[Inh] Ppm\tabcellsep Volume of hydrogen gas evolvedml\tabcellsep IE \%\\
Blank\tabcellsep 6.3\tabcellsep -\\
50\tabcellsep 2.7\tabcellsep 56.8\\
100\tabcellsep 2.4\tabcellsep 61.9\\
150\tabcellsep 2.1\tabcellsep 66.6\\
200\tabcellsep 1.8\tabcellsep 72.2\\
250\tabcellsep 1.4\tabcellsep 77.7\\
300\tabcellsep 1.1\tabcellsep 83.3\end{longtable} \par
 
\caption{\label{tab_2}Table 2 :}\end{figure}
 \begin{figure}[htbp]
\noindent\textbf{} \par 
\begin{longtable}{P{0.04662447257383966\textwidth}P{0.17573839662447258\textwidth}P{0.014345991561181434\textwidth}P{0.2187763713080169\textwidth}P{0.06814345991561181\textwidth}P{0.010759493670886076\textwidth}P{0.31561181434599156\textwidth}}
\tabcellsep 0.4\tabcellsep \tabcellsep \multicolumn{2}{l}{Blank (1M HCl) 50 ppm}\tabcellsep \\
\tabcellsep 0.2\tabcellsep \tabcellsep 100 ppm\tabcellsep \tabcellsep \\
\tabcellsep 0.0\tabcellsep \tabcellsep 150 ppm 200 ppm\tabcellsep \tabcellsep \\
\tabcellsep -0.2\tabcellsep \tabcellsep 250 ppm\tabcellsep \tabcellsep \\
E. mV(Vs SCE)\tabcellsep -1.2 -1.0 -0.8 -0.6 -0.4\tabcellsep \tabcellsep 300 ppm\tabcellsep \tabcellsep \tabcellsep Year 2015\\
\tabcellsep -1.4\tabcellsep \tabcellsep \tabcellsep \tabcellsep \\
\tabcellsep -1.6\tabcellsep \tabcellsep \tabcellsep \tabcellsep \tabcellsep 13\\
\tabcellsep -1.8\tabcellsep 1E-4\tabcellsep 1E-3\tabcellsep 0.01 logi, mA cm -2\tabcellsep 0.1\tabcellsep Issue III Version I\\
\tabcellsep \tabcellsep \tabcellsep \tabcellsep \tabcellsep \tabcellsep of Researches in Engineering ( ) Volume XV C\\
\tabcellsep \tabcellsep \tabcellsep \tabcellsep \tabcellsep \tabcellsep Global Journal\end{longtable} \par
 
\caption{\label{tab_3}}\end{figure}
 \begin{figure}[htbp]
\noindent\textbf{3} \par 
\begin{longtable}{P{0.09071146245059288\textwidth}P{0.1276679841897233\textwidth}P{0.1108695652173913\textwidth}P{0.0974308300395257\textwidth}P{0.1041501976284585\textwidth}P{0.10079051383399208\textwidth}P{0.1142292490118577\textwidth}P{0.1041501976284585\textwidth}}
{}[Inh] ppm\tabcellsep -E corr mV vs SCE\tabcellsep i corr m A cm -2\tabcellsep ? a mV dec -1\tabcellsep ? c mV dec -1\tabcellsep C.Rx10 -3 mpy\tabcellsep ?\tabcellsep IE\%\\
0\tabcellsep 725\tabcellsep 275\tabcellsep 250\tabcellsep 420\tabcellsep 164\tabcellsep ---\tabcellsep ---\\
50\tabcellsep 760\tabcellsep 136\tabcellsep 150\tabcellsep 170\tabcellsep 58\tabcellsep 0.505\tabcellsep 50.5\\
100\tabcellsep 730\tabcellsep 127\tabcellsep 80\tabcellsep 100\tabcellsep 57\tabcellsep 0.538\tabcellsep 53.8\\
150\tabcellsep 732\tabcellsep 82\tabcellsep 60\tabcellsep 100\tabcellsep 37\tabcellsep 0.700\tabcellsep 70.0\\
200\tabcellsep 743\tabcellsep 62\tabcellsep 30\tabcellsep 90\tabcellsep 10\tabcellsep 0.773\tabcellsep 77.3\\
250\tabcellsep 742\tabcellsep 56\tabcellsep 20\tabcellsep 90\tabcellsep 5.3\tabcellsep 0.796\tabcellsep 79.6\\
300\tabcellsep 744\tabcellsep 30\tabcellsep 30\tabcellsep 90\tabcellsep 5.0\tabcellsep 0.889\tabcellsep 88.9\end{longtable} \par
  {\small\itshape [Note: corr ), corrosion current density (i corr ), Tafel slopes (? c ,? a ), degree of surface coverage (?), and inhibition efficiency (IE\%) of Al in 1M HCl at 25°C]} 
\caption{\label{tab_4}Table 3 :}\end{figure}
 \begin{figure}[htbp]
\noindent\textbf{4} \par 
\begin{longtable}{P{0.13993902439024392\textwidth}P{0.16585365853658537\textwidth}P{0.2073170731707317\textwidth}P{0.17621951219512194\textwidth}P{0.16067073170731708\textwidth}}
{}[Inh] ppm\tabcellsep R p ? Cm 2\tabcellsep C dl x10 -6 µF Cm -2\tabcellsep ?\tabcellsep IE\%\\
0\tabcellsep 1.7\tabcellsep 21\tabcellsep ---\tabcellsep ---\\
50\tabcellsep 2.9\tabcellsep 5.9\tabcellsep 0.468\tabcellsep 46.8\\
100\tabcellsep 3.2\tabcellsep 4.4\tabcellsep 0.595\tabcellsep 59.5\\
150\tabcellsep 4.2\tabcellsep 3.2\tabcellsep 0.730\tabcellsep 73.0\\
200\tabcellsep 6.3\tabcellsep 3.0\tabcellsep 0.760\tabcellsep 76.0\\
250\tabcellsep 7.1\tabcellsep 2.5\tabcellsep 0.840\tabcellsep 84.0\\
300\tabcellsep 10.9\tabcellsep 2.3\tabcellsep 0.844\tabcellsep 84.4\end{longtable} \par
 
\caption{\label{tab_5}Table 4 :}\end{figure}
 \begin{figure}[htbp]
\noindent\textbf{5} \par 
\begin{longtable}{P{0.06875\textwidth}P{0.11666666666666667\textwidth}P{0.07083333333333333\textwidth}P{0.07291666666666667\textwidth}P{0.06458333333333333\textwidth}P{0.06458333333333333\textwidth}P{0.08124999999999999\textwidth}P{0.08124999999999999\textwidth}P{0.075\textwidth}P{0.15416666666666665\textwidth}}
{}[Inh] ppm\tabcellsep i corr m A cm -2\tabcellsep ? a mV dec -1\tabcellsep ? c mV dec -1\tabcellsep CF-2\tabcellsep CF-3\tabcellsep CRx10 -3 mpy\tabcellsep ?\tabcellsep IE\%\tabcellsep Issue III Version I\\
0 50 100 150 200 250 300\tabcellsep 1100 400.9 348.8 345.7 342.8 235.5 214.3\tabcellsep 182 32 31 34 24 19 18\tabcellsep 195 102 66 55 36 33 25\tabcellsep 1.1 2.0 1.1 1.7 1.8 1.2 2.0\tabcellsep 2.3 2.7 2.9 2.2 2.5 2.3 2.3\tabcellsep 667 238 207 204 146 140 127\tabcellsep ---0.642 0.688 0.691 0.694 0.789 0.809\tabcellsep ---64.2 68.8 69.1 69.4 78.9 80.9\tabcellsep ( ) Volume XV\\
\tabcellsep \tabcellsep \tabcellsep \tabcellsep \tabcellsep \tabcellsep \tabcellsep \tabcellsep \tabcellsep of Researches in Engineering\\
\tabcellsep \tabcellsep \tabcellsep \tabcellsep \tabcellsep \tabcellsep \tabcellsep \tabcellsep \tabcellsep Global Journal\end{longtable} \par
 
\caption{\label{tab_6}Table 5 :}\end{figure}
 \begin{figure}[htbp]
\noindent\textbf{6} \par 
\begin{longtable}{P{0.0908805031446541\textwidth}P{0.19245283018867926\textwidth}P{0.18710691823899372\textwidth}P{0.016037735849056604\textwidth}P{0.12295597484276728\textwidth}P{0.22452830188679243\textwidth}P{0.016037735849056604\textwidth}}
Temp.\tabcellsep K ads x10 -6\tabcellsep -?G o\tabcellsep ads\tabcellsep -?H o ads\tabcellsep ?S o\tabcellsep ads\\
?C\tabcellsep M -1\tabcellsep \multicolumn{2}{l}{k J mol -1}\tabcellsep k J mol -1\tabcellsep \multicolumn{2}{l}{J mol -1 k -1}\\
25\tabcellsep 12.2\tabcellsep \multicolumn{2}{l}{50.4}\tabcellsep \tabcellsep 226.7\tabcellsep \\
30\tabcellsep 15.6\tabcellsep \multicolumn{2}{l}{51.8}\tabcellsep \tabcellsep 227.8\tabcellsep \\
35\tabcellsep 20.6\tabcellsep \multicolumn{2}{l}{53.4}\tabcellsep 17.2\tabcellsep 229.2\tabcellsep \\
40\tabcellsep 26.9\tabcellsep \multicolumn{2}{l}{54.9}\tabcellsep \tabcellsep 230.5\tabcellsep \\
45\tabcellsep 33.9\tabcellsep \multicolumn{2}{l}{56.5}\tabcellsep \tabcellsep 231.6\tabcellsep \end{longtable} \par
 
\caption{\label{tab_7}Table 6 :}\end{figure}
 \begin{figure}[htbp]
\noindent\textbf{7} \par 
\begin{longtable}{P{0.85\textwidth}}
III Version I\\
e XV Issue\\
( ) C\end{longtable} \par
 
\caption{\label{tab_8}Table 7 :}\end{figure}
 			\footnote{© 2015 Global Journals Inc. (US)} 		 		\backmatter  			  				\begin{bibitemlist}{1}
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\end{document}
