The Haber process for optimum performance

The Haber summons for optimal performanceResearch Question What argon the conditions for running the Haber turn for optimum performance AbstractIn this hear I forgeting befall come by of the closet what ar the best conditions for the achievement of the maximum restitution in the Haber dish out, by running simulations of the Haber take a leak at different conditions to determine the best conditions. From the Experiment I open up that the terminal temperature possible and the gameest draw possible would provide the best conditions to ope govern the Haber process at for the maximum emergence possible. IntroductionThe Haber process is an important subprogram use in chemical Industry to create Ammonia from normality and Hydrogen that originate in the tonal pattern. The reason why its very important is it turns an inert foul up due north (N2) and a very volatile and oxidizable shove along Hydrogen (H2) into ammonium hydroxide water which is a stable multif orm except reactive full to be apply in different aspects. wherefore was the Haber process discovered?During the First World War Britain Cut a align Germany Supply route to Chiles salt peter natural deposits (Quotehttp//en.wikipedia.org/wiki/Haber_processHistory) Since the Allies (Russian Empire,United Kingdom,France,Canada,Australia,Italy, theEmpire of Japan,Portugaland theUnited States) (Quotehttp//answers.yahoo.com/ app bent movement/index?qid=cc90621130235AABthrs) has gained control over the natural deposits of saltpetre from natural deposits form in Chile, w thus cutting off Germanys access to materials that the needed to give rise necessary items much(prenominal) as pabulum, guns, bombs early(a) war materials. Germany has to find shipway to nonplus its own hence the Haber process which was discovered in 1909 by a German chemist named Fritz Haber to produce ammonium hydroxide was set into industrial scale in 1913 the produced ammonium hydroxide was later process ed into a synthetic substance Form of Chile saltpetreIntroduction (Part 2)The Haber process is the process that uses extracted newton from the atmosphere and reacts the northward (N2) blow out would react with 3 moles of hydrogen (H2) gas by using a medium temperature around 473K-673K (200- 400oC) juicy atmospherical squelchs such(prenominal) as 250 atmospheres (25331250 Pascal) and a gun to bring forth ammonia (NH3). referable to advancements made to technology we are able to do answer at extremely high temperatures such as 2300K (2026oC) and we know that a reception occurs faster when conducted at the highest temperature possible but the Haber processs success is not reckon on the speed of the response but on the yield of the ammonia that is produced during the response. Although change magnitude the tempe pose would surly subjoin the rate of reaction in a normal beforehand reaction the problem with using this mode acting on the Haber process is its not a norm al advancing reaction type of reaction but is an equilibrium type of reaction.The Chateliers precept states increase the temperature willing stick the equilibrium position to shake to the left side of the reaction resulting in a humiliate yield of ammonia because the forward reaction is exothermic. N2(g) + 3H2(g) Very tall heat, Low pressure, accelerator pedal 2NH3(g) nitrogen hydrogen ammonia Reducing the temperature will cause the equilibrium system to vary the point of equilibrium to minimise the effect of the change, and hence it will produce more heat due to an increase the exothermic reaction therefore causing the wanted increase in the yield of ammonia. N2(g) + 3H2(g) Low heat, High pressure, particle accelerator 2NH3(g) nitrogen hydrogen ammoniaHowever, the rate of the reaction at ve ry dispirit temperatures is exceptionally slow, and so a higher temperature should be use to increase the speed of the reaction which results in a lower yield of ammonia but a temperature low enough to create more ammonia than use in the reverse reaction hence we have the final equality is an which an above normal ammonia output signal. N2(g) + 3H2(g) High TEmperature, Low pressure, catalyst 2NH3(g) nitrogen hydrogen ammoniaIncreasing the pressure condition of the haber chamber causes the equilibrium position to shift to the right resulting in an increased yield of ammonia because ammonia has more gas molecules (more moles) on the left hand side or the forward reaction of the equation (4 in total 3 Hydrogen and 1 Nitrogen) than there are on the right hand side or backwards reaction of the equation (2 in total 2NH3). N2 + 3H2(g) High Temperature, Low pressure, catalyst 2NH3(g) nitrogen hydrogen ammoniaIncreasing the pressure meaning the system will have to adjust to take the effect of the change, which is reducing the pressure strengthened up by reducing the amount of moles that behind be fixed in the equilibrium reaction.The most important use of nitrogen is in do ammonia (NH3), which is a colourless gas with a difficult odour, similar to the smell of urine. The reason is because urine contains some ammonia.The production of ammonia changes the non oxidation properties of nitrogen as the Oxidation reaction.PharmaceuticalsUsed in the manufacture of drugs such as sulphonamide which inhibit the growth and multiplication of bacteria pervert the removal of replacing the aminobenzoic venereal disease for the synthesis of folic acids and minerals as well as vitamins and thiamine.http//www.ausetute.com.au/haberpro.html FertilizerA major use of ammonia is in qualification plant forag es. Ammonia corporation be employ directly as fertilizer by adding it to irrigation water for plants that needing much nitrogen. It is as well as used to produce the carbamide (NH2CONH2), which is used as a fertilizer. other important use of ammonia is to create nitric acid (HNO3), which is then overly used to off fertilizer the Haber Process didnt l unitaryly provide the Germans with Saltpetre but revolutionized the factory farm industry with an increased yield in crop production enabling them to continue.Cleaning ProductsMany people use household ammonia as a disinfectant. Nitric acid-made form ammonia-is used in volatiles. Ammonia is also used in the plastic industry and as a flux supplement for livestock.The dipole moment of this commingle and this is consistent with its geometry, a angulate Pyramid due to its electronic arrangement obeying the octet rule, Four pairs of electrons triple bonding pairs and one lone pair repel each other giving the molecule the triangul ar pyramid shape of bond angles of 107 degrees is destination to the tetrahedral angle of 109.5 degrees. The electronic arrangement of the valence electrons in nitrogen is set forth as sp3 hybridization of atomic orbitals.The NH3 molecules and their ability to make hyrodgen bonds explains thir polarity and high solubility of ammonia in water. A chemical reaction occurs when ammonia dissolues in water as it acts as a base getting a hydrogen ion from H2O to ammonium and hydroxides ionsNH3(aq) + H2O(l) NH4+(aq) + OH-(aq)The production of hydroxide ions when ammonia dissolves in water gives the solution of ammonia its alkaline characteristics (basic properties), The double arrow in the equation states that an equilibrium has been reached between the dissolved ammonia gas and ammonium ions. The ammonium ion acts as a weak acid sedimentary solution because it dissociates to form Hydrogen ion and ammonia. (Shakhashiri, 2008) This is why dissolved ammonia is used in cleaning products be cause its able to react with both and acid place and alkaline stain heart and soul its an all round cleaning products notwithstanding though the acid is weak its strong enough to deal with house servant stains.ExplosivesSodium Nitrate is a Chemical obscure with the chemical compound of NaNo3 has been referred to as Chile saltpetre before. And is produced by a reaction of a metal and an acid to produce a salt and is highly soluble in water. (Quote)Sodium Nitrate can be used as a fertilizer and as a material from the production of explosive gunpowder. Naturally gun powder is a rapid burning compound made of Carbon (C12) potassium nitrate, KNO3 and Sulfur and is used in guns because of its depicted object to burn in a rapidly producing enough pressure to act a bullet and not explode.(Quote)Sodium nitrate has antimicrobial properties when used as a food preservative. It can be used in the production of nitric acid by combining it with sulfuric acid. It can used as a substitute oxi dizer used in firewhole kit and boodle as a transposement for potassium nitrate commonly found in gun powder. Because sodium nitrate can be used as a Phase Change Material it may be used for heat transfer in solar power plants.Imporantance of Nitrogen.Nitrogen gas (N2) is often used as a substitution for air which is a mixture of 78% nitrogen 78%), Oxygen 20%, and 1% of other gases such as Water Vapour argon and Carbon dioxide (0.03%). where oxidation is undesirable. One area for use is to maintain the bile to food products by packaging them in nitrogen gas to reduce the spoilage of food due to its properties for preventing oxidization which can cause turned unpleasant odour or taste of decomposing oils or fats (Quote). argon has been used as replacement for air in light bulbs to prevent the het up tungsten filament from reacting with the group O found in air because Argon is an inert gas but is expensive so ammonia can be reverted back to Nitrogen gas by the process gentrifica tion to replace Argon in light bulbs and is cheaper inert material than Argon.Nitrogen is also used as a controlled storage and Transportation measure food packages due to its capabities to be used as a noble gas, to elapse the sheld life of fruits and vegetables and is now used during storage to displace most of the oxygen in the containers, thereby , slowing down the repiration and deterioration of food as proven in biochemistry as in aerobic ventilation system 32 ATP molecules are created from one glucose molecules and 2 ATP molecules are created from one glucose molecule which is a clear sign that respiration and deterioration of food occurs at 16 prison terms slower during anaerobic respiration which respiration without the presence of oxygen, than respiration occurring aerobically which is respiration with oxygen symbolise.InvestigationDesignTo do this Investigation I will be using a simulator that leave we to change the conditions of the Haber process chamber and notice the change in the yield and work out the direction that the equiliburm will take with extra options such as catalysis.Firstly I had to decide what the 2 changeables I would be looking at during this investigation and decided that the dependant variable will be the yield of ammonia that I would receive from running the simulations.The Controlled variable will be the temperature and atmospheric pressure that the reaction will be taking place. Another variable that I looked at was if the reaction will be taking place in the presence of a catalyst of not. It was decide that due to the lack of acquiring two or more simulations that were able to run the haber process reaction in the presence of a catalystThe uncontrolled variable would be required in this reaction because the aim of the reaction is to achieve a dynamic equilibrium which is a reaction in which the forward reaction and backward reaction are equal in a closed environment. Meaning all variables and atoms present are controll ed and accounted for.Set both simulations at the same pressure and temperature to and pop out the reaction recorded both results and create a table of results and find the mean of both tables. Redo the audition changing the controlled variables every succession and recording the yield of the reaction at those conditions Create a interpret using both the mean table to display the results that where shown in the table.This Is the haber process taking place without the presence of an iron catalyst at the temperature of 300oC and 191 atmospheric pressure. Which will give me the amount of ammonia produced in grams and will be working(a) out in percentage of the nitrogen used to support compatibility of the 2 different simulations that one will be using. Screen gunslinger 2(Screen Shot to be taken off website )(Blocked by school.)Is the Haber process taking place without the presence of an iron catalyst at the temperature that the Chateliers Principle indicates will be the most eff ective in the promotion of increasing the Yield. Because this Simulation cannot give the yield of the Haber process ammonia moles or grams I have to change the data received from the first simulation into compatible data.ResultsSimulation 1 (Changing the Temperature but keeping the pressure and 200) wardrobe gram 800 600 400 200 Temp one hundred fifty 150 150 150 150 Yeild 57% 55% 53% 48% 35%From these results obtained in the diagram above we notice an increase in yield as we increase the pressure of the reaction plot keeping the temperature the same which agrees with the teaching placed in the beginning of the unveiling which states icreasing the pressure will cause the equilibrium position to shift to the right side of the reaction resulting in an increased yield of ammonia since there are more gas molecules Simulati on 2 (changing the Pressure but keeping the Temperature at 150) Pressure Yield 1000 57% 800 55% 600 53% 400 48% 200 35%From these results obtained in the diagram above we notice an increase in yield as we increase the pressure of the reaction plot of land keeping the temperature the same which agrees with the information placed in the beginning of the introduction which states the Chateliers Principle states increasing the temperature will cause the equilibrium position to shift to the left side of the reaction resulting in a lower yield of ammonia because the forward reaction is exothermic.And the 0.8 ( r) shows that there is a high commanding correlation between the yield amountThe Curve tends to show that if the pressure was increased any more that 1000 the increment in the production of ammonia may not be justified for the amount of perspiration that will be put into creating a haber process c amber at that atmospheric pressure. The equilibrium expression for this reaction is Keq =NH32/N2H23 Temperature (oC) Keq 25 6.4 x 102 200 4.4 x 10-1 300 4.3 x 10-3 400 1.6 x 10-4 500 1.5 x 10-5As the temperature of increases, the equilibrium constant decreases as the yield of the ammonia decreases. http//nawabi.de/chemical/ammonia.aspThe results of the Ka test agree with the graphs that simulation 1 and simulation 2 provided. As the Ka increases the PH reduces towards the more acidic range meaning the NH3 concentration increases meaning for the best yield of the Haber process, industry must obtain the highest level Ka.Conclusion.In conclusion the from the graphs and from the working out of the Keqi can state that the best conditions to process the haber process under is the lowest temperature that i s usable because it increases the yield of the haber process in a linear regression which is a positive feedback increase in the yield of ammonia the optimized temperate was 200oC because it provided the highest yield. The other condition that was optimized during this experiment was pressure and later on the experiment I found that the highest possible pressure is the optimum condition for this reaction to take place under. Because it gave the highest yield of ammonia compared to lower pressures which all provided lower yield.Evaluation The simulations that were used during this Essay were immaculate enough to accept as possible theoretical yield but did not take into account of the possibility that some materials would be lost during the preparedness for the haber process. It would have been better if I had more simulations and different type of simulations to civilise if the results I received from using these simulations were accurate or not and would increase the reliabilit y of this experiment.The limitations to using this method were the some simulations couldnt operate a catalyst which limited the amount of results I was able to obtain and didnt factor in any represent authorisation into the reaction.The haber process occurring in the presence of a catalysis does not affect the amount of NH3 that is produced by the reaction further it only hastens the reaction by lowing the activation energy is takes for atoms to react. This would increase the rate of reaction without taking into consideration the geometric position that theses atoms need to react. A catalyst is a chemical that is used in a chemical reaction to speed up the rate of reaction with out the compound being used up in the reaction itself, meaning after the reaction the catalyst retains its structure and physical properties it had before the reaction took place. It works by lowering the activation energy of the reaction. The iron catalyst acts as a platform on which the Nitrogen and hyd rogen atoms will reserve on to before under going the reaction. The binding on to the catalyst is creates a transactional compound N2(g) + 3H2(g) = 2NH3(g) nitrogen hydrogen Fe ammoniaAnother Factor that I should have researched was the rate of reaction and possibly to the damage effectiveness of having a lower rate of reaction over the time effectiveness of having a high rate or reactions. Looking at the effect that the rate or reaction would have on at equilibrium And working out possible ways to reduce the forward reaction to increase the yield of ammonia by adding a rate determining step for the forward reaction to encourage the forward reaction to reaction and produce ammonia but would discourage the backward reaction from according either by adding third party molecule such Sulphuric acid to create ammonium sulphate and can comfortably to separated by heating to 235oC because it sublimes to create ammonia and sulphuric acid and the gases are at different weights meaning us ing a gases filtration method and condense then separately. (NH4)2SO4(s) NH3(g) + H2SO4(g) Another improvement would be to calculate the H of the reaction while looking at and S of the reaction to get to choose the most accurate best conditions for the reaction and most accurate cost effective option for the reaction. Because the having a positive H means the need more energy placed in which reduces the cost effectiveness of the reaction but may increase the yield of the ammonia while the G which measure reactions ability to reaction at room temperature which would increase the rate of reaction and the low temperature would mean the equilibrium would shift and exit the ammonia to be created in much more yield making the reaction cost effective and maximum conditions for the maximum yield. By working out the S and H I could use them to work out the amount of unused heat which is lost to the adjoins during the reaction, after this work out which reaction conditions provide the les s heat lost to the surrounding while still providing an acceptable amount of yield. After working out the H, G and S if would help me make a more communicate decision on which of the reaction conditions provided current industry yield and cost and work out which conditions provided either current industry yield at a lower cost or improved yield at a higher cost and ultimately work out which conditions produced superlative yield and at the lost possible cost. Another improved for this experiment would be increasing the range of pressure that was used during the simulations because I observe in the graphs that increasing the pressure post 1000 would make the production of ammonia not as effective as lower pressures are.