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Explains key ideas behind nitrogen fertiliser production using the Haber process, including equilibrium, balanced reversible reactions, and uses of ammonia. Covers catalyst function, dynamic equilibrium characteristics, and Le Chatelier’s principle through how increased and decreased pressure affect crowding, reaction rates, product amounts, and the equilibrium constant Kc, concluding with selecting an optimal safe and economical pressure.",{"@graph":69,"@context":120},[70,84,99],{"@type":71,"itemListElement":72},"BreadcrumbList",[73,77,79,82],{"item":74,"name":75,"@type":76,"position":8},"https://docshare.wps.com","Home","ListItem",{"item":78,"name":9,"@type":76,"position":14},"https://docshare.wps.com/document/",{"item":80,"name":35,"@type":76,"position":81},"https://docshare.wps.com/document/healthcare/",3,{"item":83,"name":65,"@type":76,"position":19},"https://docshare.wps.com/document/fertilisers-memo-haber-process-and-le-chateliers-effect-of-pressure/573747/",{"url":83,"name":65,"@type":85,"author":86,"headline":65,"publisher":89,"fileFormat":92,"inLanguage":63,"description":67,"dateModified":93,"datePublished":93,"encodingFormat":92,"isAccessibleForFree":94,"interactionStatistic":95},"DigitalDocument",{"name":87,"@type":88},"LangkahRina","Person",{"url":74,"name":90,"@type":91},"DocShare","Organization","application/pdf","2026-10-14",true,{"@type":96,"interactionType":97,"userInteractionCount":4},"InteractionCounter",{"@type":98},"ViewAction",{"@type":100,"mainEntity":101},"FAQPage",[102,108,112,116],{"name":103,"@type":104,"acceptedAnswer":105},"Why is nitrogen important to plants, and in what forms can they absorb it?","Question",{"text":106,"@type":107},"Nitrogen is found in all proteins, making it an essential nutrient. Plants can absorb dissolved urea, nitrate, nitrite, and ammonium ions.","Answer",{"name":109,"@type":104,"acceptedAnswer":110},"What is the purpose of the Haber Process and what is the balanced reversible equation?",{"text":111,"@type":107},"The Haber Process produces ammonia (NH3) from nitrogen (N2) and hydrogen (H2). The reversible balanced equation is N2 + 3H2 ⇌ 2NH3.",{"name":113,"@type":104,"acceptedAnswer":114},"How does an iron oxide catalyst (and ruthenium) affect the Haber Process?",{"text":115,"@type":107},"A catalyst speeds up the reaction by lowering its activation energy, acting as a binding site where the reaction can occur.",{"name":117,"@type":104,"acceptedAnswer":118},"How do increased and decreased pressure affect the Haber Process equilibrium and ammonia production?",{"text":119,"@type":107},"Increased pressure increases gaseous crowding and temporarily shifts equilibrium toward the reaction that forms fewer gas molecules, producing more ammonia at equilibrium; Kc changes accordingly. Decreased pressure decreases crowding and shifts equilibrium toward the reaction that forms more gas molecules, resulting in less ammonia at equilibrium, with Kc changing as well.","https://schema.org",{"og:url":83,"og:type":122,"og:title":65,"og:site_name":90,"og:description":67},"article",{"robots":124,"canonical":83},"index,follow",{"doc_id":126,"site_id":62},573747,1791944888,{"code":4,"msg":5,"data":129},{"doc_id":126,"user_id":130,"nickname":87,"user_avatar":131,"doc_module":4,"category_id":34,"category_name":35,"doc_title":65,"doc_description":67,"doc_content":132,"file_id":133,"file_url":134,"file_type":135,"file_size":136,"view_count":4,"is_deleted":4,"is_public":8,"is_downloadable":8,"audit_status":8,"page_count":19,"language":137,"language_code":63,"site_id":62,"html_lang":63,"table_of_contents":138,"faqs":139,"seo_title":140,"seo_description":67,"update_tm":127,"read_time":52},962090893776,"https://ap-avatar.wpscdn.com/davatar_155a257f0dc6eb9ab79c44ca47cae57d","FERTILISERS MEMO  \nOverview  \n1 Why is nitrogen important to plants? Nitrogen is found in all proteins, and so it is an essential nutrient.  \n2. In what forms can plants absorb nitrogen?  \nDissolved urea, nitrate, nitrite and ammonium ions.  \n3 Complete to summarise the industrial processes.  \n| Process | Reactants | Products\u003Cbr>of step 1 | Products\u003Cbr>of step 2 | Final products |\n| --- | --- | --- | --- | --- |\n| Haber | N2 + H2 | not applicable |  | NH3 |\n| Ostwald | NH3 + O2 | NO | NO2 | HNO3 |\n| Contact | S + O2 | SO2 | SO3 | H2SO4 |\n\nHaber Process  \n4 What is the purpose of the Haber Process?  \nTo produce ammonia (NH3) from nitrogen (N2) and hydrogen (H2) .  \n5 Write a balanced equation for the Haber Process's reversible reaction. N2 + 3H2  2NH3  \n6 Name some uses of ammonia. As a cleaning agent. As a coolant in some air conditioners. To manufacture nitrogen fertilisers.  \n7 Name two conditions which must be met for a reaction to reach equilibrium.  \n- reversible reaction - closed system  \n8 Name two characteristics of equilibrium.  \n- rates of forward and reverse reactions are equal to one another  \n-the concentrations of reactants and products remain constant  \n9 In the Haber Process an iron oxide catalyst is usually used. Ruthenium can also be used. What does a catalyst do to a reaction, and how does it do this? It speeds up a reaction by lowering its activation energy. It does this by serving as a binding site on which thereaction can occur.  \n10 Circle the correct option (True / False) for each of the following.  \ni A catalyst speeds up the Haber Process's forward reaction more than the reverse. [True / False] ii A catalyst will cause more product to be formed. [True / False]  \niii A catalyst will decrease the time it takes to reach equilibrium because it speeds up both forward and reverse reactions. [True / False]  \niv A catalyst speeds both forward and reverse reactions equally [True / False]  \n11 Link each element from Column A with its corresponding element in Column B. Write the letter from A next to each item in B in the last column.  \nColumn A Column B A  \na dynamic equilibrium absorbs heat b  \nb endothermic a measure of the average kinetic energy of particles i  \nc exothermic disturbs equilibrium, favours increased crowding, more e  \nmolecules  \nd Le Chatelier's principle 273 K and 101,3 kPa k  \ne decrease in pressure disturbs equilibrium, favours exothermic reaction g  \nf increase in pressure releases heat c  \ng removing heat a state in which forward and reverse reactions occur at a  \nequal rates  \nh adding heat force per area, in gases related to rate of particle j  \ncollisions  \ni temperature disturbs equilibrium, favours decreased crowding, fewer f  \nmolecules  \nj pressure disturbs equilibrium, favours endothermic reaction h  \nk STP when a system which is in equilibrium is disturbed, it d  \nwill respond in such a way as to counteract the disturbance  \n􀂈 Creative Commons BY-NC-SA CHEMICAL INDUSTRIES RESOURCE PACK 􀀔􀀓  \nLe Chatelier: Effect of pressure  \n12 Complete the explanation by filling the gaps or choosing from the options. Do this before, or after, but not during, watching the animations. Mark during re-watching.  \nIncreased pressure  \nAccording to Le Chatelier's principle, when a system which is in equilibrium is disturbed, it will respond in such a way as to counteract the disturbance. An increase in pressure [de/in]creases the crowding of gaseous molecules. The system will respond by [de/in]creasing their crowding. Crowding is decreased in gases when [fewer/more] molecules are formed. In the Haber Process the [forward/reverse] reaction makes fewer molecules than the [forward/reverse] reaction. In the forward reaction 2 molecules of ammonia are made from every 4 molecules  \nof reactants (1 N2 and 3 H2 molecules) . Consequently, an increase in  \npressure disturbs equilibrium for a while by making the [forward/reverse] reaction occur at a higher rate than the [forward/reverse] reaction. This causes [","cbCaiuMZRnAWt6te","https://ap.wps.com/l/cbCaiuMZRnAWt6te","pdf",555039,"English","# Overview\n# Haber Process\n## Purposes and reaction\n## Equilibrium and catalysts\n## True/False checks\n## Matching concepts\n# Le Chatelier: Effect of pressure\n## Increased pressure\n## Decreased pressure\n## Optimum pressure","[{\"question\":\"Why is nitrogen important to plants, and in what forms can they absorb it?\",\"answer\":\"Nitrogen is found in all proteins, making it an essential nutrient. Plants can absorb dissolved urea, nitrate, nitrite, and ammonium ions.\"},{\"question\":\"What is the purpose of the Haber Process and what is the balanced reversible equation?\",\"answer\":\"The Haber Process produces ammonia (NH3) from nitrogen (N2) and hydrogen (H2). The reversible balanced equation is N2 + 3H2 ⇌ 2NH3.\"},{\"question\":\"How does an iron oxide catalyst (and ruthenium) affect the Haber Process?\",\"answer\":\"A catalyst speeds up the reaction by lowering its activation energy, acting as a binding site where the reaction can occur.\"},{\"question\":\"How do increased and decreased pressure affect the Haber Process equilibrium and ammonia production?\",\"answer\":\"Increased pressure increases gaseous crowding and temporarily shifts equilibrium toward the reaction that forms fewer gas molecules, producing more ammonia at equilibrium; Kc changes accordingly. Decreased pressure decreases crowding and shifts equilibrium toward the reaction that forms more gas molecules, resulting in less ammonia at equilibrium, with Kc changing as well.\"}]","FERTILISERS MEMO - Haber Process and Le Chatelier's Effect of Pressure | PDF"]