{"id":6057,"date":"2020-10-13T14:37:36","date_gmt":"2020-10-13T09:07:36","guid":{"rendered":"http:\/\/astan.lk\/al_virtualclassroom\/?p=6057"},"modified":"2020-10-13T14:37:56","modified_gmt":"2020-10-13T09:07:56","slug":"p-block-elements-2","status":"publish","type":"post","link":"https:\/\/astan.lk\/al_virtualclassroom\/p-block-elements-2\/","title":{"rendered":"p block elements and their compounds"},"content":{"rendered":"

\u00a0Production of ammonia (Haber process)<\/h4>\n

\u2022 Nitrogen and hydrogen gases are used as raw materials.
\n\u2022 Nitrogen is obtained by the fractional distillation of liquid air.<\/p>\n

\u2022 Hydrogen is obtained from naptha or natural gas as follows.
\nC6<\/sub>H14<\/sub>(g) + 6H2<\/sub>O(g) \u2192\u00a06CO(g) + 13H2<\/sub>(g)
\nin naptha
\nCH4<\/sub>(g) + H2<\/sub>O(g) \u2192\u00a0CO(g) + 3H2<\/sub>(g)
\nin natural gas<\/p>\n

or partial oxidation with oxygen:
\nC6<\/sub>H14<\/sub>(g) + 3O2<\/sub>(g) \u2192\u00a06CO(g) + 7H2<\/sub>(g)
\nin naptha
\n2CH4<\/sub>(g) + O2<\/sub>(g) \u2192\u00a02CO(g) + 4H2<\/sub>(g)
\nin natural gas<\/p>\n

\u2022 Nitrogen and hydrogen form an equilibrium mixture containing ammonia.
\nN2<\/sub>(g) + 3H2<\/sub>(g) \u21cc 2NH3<\/sub>(g) \u00a0 \u00a0 \u0394H = -92 kJ mol-1<\/p>\n

\u2022 Le Chatelier’s principle suggests that increase in pressure and decrease in temperature will increase the proportion of ammonia at equilibrium.
\n\u2022 High pressure obviously gives a high yield of ammonia, but the higher the pressure greater the cost and maintenance of equipment. The favoured pressure nowadays is 250 atm.
\n\u2022 The temperature must be low to give a higher yield of ammonia. But at low temperature the rate of reaction is so low that it makes the process uneconomical. In practice, the optimum temperature is usually about 450 0C. As the reaction is exothermic the system must be cooled.<\/p>\n

\u2022 In addition to pressure and temperature, the catalyst is a vitally important variable. Here iron is used as a catalyst and small amounts of potassium oxide and aluminium oxide are used as promoters.<\/p>\n

\u2022 Low concentrations of NH3<\/sub> is favourable for the forward reaction. So NH3<\/sub> is cooled under pressure and the liquid ammonia is removed.<\/p>\n

<\/p>\n

Uses of ammonia<\/h4>\n

\u2022 Production of nitric acid, fertilizers and nylon
\n\u2022 Petroleum industry utilizes ammonia in neutralizing the acid constituents of crude oil.
\n\u2022 Used in water and waste water treatment, such as pH control, in solution form to regenerate weak anion exchange resins.
\n\u2022 Used in stack emission control systems to neutralize sulphur oxides from combustion of sulphur-containing fuels.
\n\u2022 Used as a refrigerant in industrial refrigeration systems found in the food, beverage, petrochemical and cold storage industries.
\n\u2022 Used in the rubber industry for the stabilization of natural and synthetic latex to prevent premature coagulation.<\/p>\n

Production of urea<\/h3>\n

\u2022 Ammonia and carbon dioxide are used as raw materials.<\/p>\n

\"\"<\/a><\/p>\n

\u2022 Production of urea is a two step process.<\/p>\n

(i) 2NH3<\/sub>(g) + CO2<\/sub>(g) \u21cc\u00a0NH2<\/sub>COONH4<\/sub>(s)<\/p>\n

(ii) NH2<\/sub>COONH4<\/sub>(s) \u21cc\u00a0CO(NH2<\/sub>)2<\/sub>(aq) + H2<\/sub>O(l)<\/p>\n

\u2022 Reaction of the step 1 is fast and exothermic and essentially goes to completion under reaction conditions used industrially. Unreacted NH3<\/sub> and CO2<\/sub> are fed into the first step.
\n\u2022 Reaction of step 2 is slower and endothermic and does not go to completion. The conversion is in the order of 50-80%.<\/p>\n

Uses of urea<\/h4>\n

\u2022 Urea is a popular solid nitrogen fertilizer because of its high nitrogen content (46%).
\n\u2022 Urea is used in the manufacture of urea-formaldehyde polymer.<\/p>\n

Manufacture of nitric acid (Ostwald process)<\/h3>\n

\u2022 Ammonia, air and water are used as raw materials.<\/p>\n

\"\"<\/a><\/p>\n

\u2022 The oxidation of ammonia by air to give nitric oxide is an exothermic reaction. The temperature is adjusted to and maintained at about 900 \u00b0C by controlling the flow rate of the gases.<\/p>\n

\u2022 The process is operated under increased pressure because this packs more reactants into the same capacity plant and increases the rate slightly by increasing the number of molecular collisions per second at the catalyst surface.<\/p>\n

\u2022 An excess air is used to ensure complete oxidation of NH3<\/sub><\/p>\n

\u2022 Cold air is added to the mixture as it leaves the catalyst because the next stage is an exothermic equilibrium and is therefore favoured by low temperature.<\/p>\n

\u2022 Extensive cooling of the gases is necessary before nitrogen dioxide is absorbed in water in the presence of air to give nitric acid.<\/p>\n

Thus the actual conditions used leading to about 96% conversion are
\n\u2022 Pressure: 1 – 9 atm
\n\u2022 Temperature : 850 -1225 0C
\n\u2022 Catalyst : platinum containing 10% rhodium<\/p>\n

\u00a0Uses of nitric acid<\/h4>\n

\u2022 Used in the synthesis of ammonium nitrate for use as a fertilizer and in explosives.
\n\u2022 Used to prepare nitrates which are of great importance in industry.
\n\u2022 NaNO3<\/sub> is used as a preservative for meat.
\n\u2022 KNO3<\/sub> is used in fertilizers and for making gun powder.
\n\u2022 AgNO3<\/sub> is used to prepare photographic film and paper.
\n\u2022 For the preparation of aquaregia.
\n\u2022 Used to clean soldering surfaces<\/p>\n

\u00a0Production of phosphate fertilizers<\/h3>\n

\u2022 Phosphorus is an essential nutrient for all living organisms.
\n\u2022 An important phosphorus containing fertilizer for plants is superphosphate which is a mixture of calcium dihydrogenphosphate Ca(H2<\/sub>PO4<\/sub>)2<\/sub> and hydrated calcium sulphate (gypsum) CaSO4<\/sub>.2H2<\/sub>O.
\n\u2022 Eppawela apatite [3Ca3<\/sub>(PO4<\/sub>)2<\/sub>.CaX2<\/sub> or Ca5<\/sub>(PO4<\/sub>)3X where X = F\/Cl\/OH] is a good raw material for the prodution of phosphate fertilzers.
\n\u2022 Apatite is insoluble and made soluble for short term crops by complete and partial acidulation.<\/p>\n

\u2022 Sulphuric acid, nitric acid, hydrochloric acid and phosphoric acid can be used for acidulation.<\/p>\n

3Ca3<\/sub>(PO4<\/sub>)2<\/sub>.CaX2<\/sub>(s) + 7H2<\/sub>SO4<\/sub>(aq) \u21923Ca(H2<\/sub>PO4sub>2)2<\/sub>(s) + 7CaSO4<\/sub>(s)+ 2HX(aq) —(1)
\n3Ca3<\/sub>(PO4<\/sub>)2<\/sub>.CaX2<\/sub>(s) + 14HCl(aq) \u2192 3Ca(H2<\/sub>PO4<\/sub>)2<\/sub>(s) + 7CaCl2<\/sub>(s)+ 2HX(aq) —–(2)<\/p>\n

\u2022 Apatite is finely ground and mixed with acid and left for 4-6 weeks. Then the product
\nsingle superphosphate (SSP) is obtained.
\n\u2022 Addition of ammonium sulphate to products of reaction (2) produces a non hygroscopic fertilizer.
\nCaCl2<\/sub>(s) + (NH4<\/sub>)2<\/sub>SO4<\/sub>(aq) \u2192 CaSO4<\/sub>(s) + 2NH4<\/sub>Cl(aq)<\/p>\n

Manufacture of sulphuric acid (Contact process)<\/h3>\n

\u2022 Sulphur or sulphur containing minerals, air and water are used as raw materials. Sulphur dioxide produced during the extraction of metals such as lead and zinc from their sulphide ores can also be used.<\/p>\n

<\/p>\n

\u2022 The reaction between sulphur dioxide and oxygen is reversible. Sulphur trioxide continuously breaks down again to sulphur dioxide and oxygen. So the mixture is passed over several beds of catalyst to let the gases react again.<\/p>\n

\u2022 The sulphur trioxide is removed between the last two beds of catalyst in order to increase the yield.<\/p>\n

\u2022 As the reaction of formation of sulphur trioxide is exothermic and three moles of reactants form two moles of products, Le Chatelier’s principle predicts that the maximum yield of SO3<\/sub> at equilibrium will be obtained at high pressure and at low temperature.<\/p>\n

\u2022 In practice, a compromise temperature of 450 \u00b0C is chosen. This is the lowest that can be used without reducing the reaction rate to an unacceptable level. There are other reasons for keeping the temperature as low as possible. Fuel cost and corrosion of reaction chambers increase rapidly with rising temperature.<\/p>\n

\u2022 At 450 \u00b0C conversion to SO3 is 97% and this high conversion even at atmospheric pressure, makes it unnecessary to carry out the process at increased pressure.<\/p>\n

\u2022 As the reaction proceeds, the heat evolved in the exothermic reaction moves the systemto higher temperature. At this higher temperature the percentage conversion to SO3<\/sub> ismuch reduced. Thus, it is necessary to cool gases between successive beds of catalyst.This is done using cold water pipes. The water is converted to steam and used to generate power(electricity).<\/p>\n

\u2022 The sulphur trioxide is dissolved in concentrated acid rather than water. If it is dissolved in water, a thick mist of acid forms. This would be a pollution hazard.<\/p>\n

\u2022 Oleum is mixed carefully with water to produce concentrated sulphuric acid.<\/p>\n

Uses of sulphuric acid<\/h4>\n

\u2022 Manufacture of phosphate fertilizers
\n\u2022 Manufacture of ammonium sulphate fertilizers
\n\u2022 Manufacture of synthetic fibres rayon and plastics
\n\u2022 In the production of detergents – mostly alkyl and aryl sulphonates
\n\u2022 In the production of dyes, explosives and drugs
\n\u2022 In the production of battery acid
\n\u2022 Drying gases (Cl2<\/sub>)<\/p>\n

 <\/p>\n

 <\/p>\n

 <\/p>\n","protected":false},"excerpt":{"rendered":"

\u00a0Production of ammonia (Haber process) \u2022 Nitrogen and hydrogen gases are used as raw materials. \u2022 Nitrogen is obtained by the fractional distillation of liquid air. \u2022 Hydrogen is obtained from naptha or natural gas as follows. C6H14(g) + 6H2O(g) \u2192\u00a06CO(g) + 13H2(g) in naptha CH4(g) + H2O(g) \u2192\u00a0CO(g) + 3H2(g) in natural gas or […]<\/p>\n","protected":false},"author":842,"featured_media":0,"comment_status":"open","ping_status":"open","sticky":false,"template":"","format":"standard","meta":{"_acf_changed":false,"_monsterinsights_skip_tracking":false,"_monsterinsights_sitenote_active":false,"_monsterinsights_sitenote_note":"","_monsterinsights_sitenote_category":0,"footnotes":""},"categories":[14,1680],"tags":[],"class_list":["post-6057","post","type-post","status-publish","format-standard","hentry","category-chemistry","category-unit-15"],"acf":[],"yoast_head":"\np block elements and their compounds - Learning & Education Portal<\/title>\n<meta name=\"robots\" content=\"index, follow, max-snippet:-1, max-image-preview:large, max-video-preview:-1\" \/>\n<link rel=\"canonical\" href=\"https:\/\/astan.lk\/al_virtualclassroom\/p-block-elements-2\/\" \/>\n<meta property=\"og:locale\" content=\"en_US\" \/>\n<meta property=\"og:type\" content=\"article\" \/>\n<meta property=\"og:title\" content=\"p block elements and their compounds - Learning & Education Portal\" \/>\n<meta property=\"og:description\" content=\"\u00a0Production of ammonia (Haber process) \u2022 Nitrogen and hydrogen gases are used as raw materials. \u2022 Nitrogen is obtained by the fractional distillation of liquid air. \u2022 Hydrogen is obtained from naptha or natural gas as follows. C6H14(g) + 6H2O(g) \u2192\u00a06CO(g) + 13H2(g) in naptha CH4(g) + H2O(g) \u2192\u00a0CO(g) + 3H2(g) in natural gas or […]\" \/>\n<meta property=\"og:url\" content=\"https:\/\/astan.lk\/al_virtualclassroom\/p-block-elements-2\/\" \/>\n<meta property=\"og:site_name\" content=\"Learning & Education Portal\" \/>\n<meta property=\"article:published_time\" content=\"2020-10-13T09:07:36+00:00\" \/>\n<meta property=\"article:modified_time\" content=\"2020-10-13T09:07:56+00:00\" \/>\n<meta property=\"og:image\" content=\"http:\/\/chemistry.need.org\/Files\/Haber%20Bosch%20Ammonia%20Process_0.jpg\" \/>\n<meta name=\"author\" content=\"Admin\" \/>\n<meta name=\"twitter:card\" content=\"summary_large_image\" \/>\n<meta name=\"twitter:label1\" content=\"Written by\" \/>\n\t<meta name=\"twitter:data1\" content=\"Admin\" \/>\n\t<meta name=\"twitter:label2\" content=\"Est. reading time\" \/>\n\t<meta name=\"twitter:data2\" content=\"6 minutes\" \/>\n<script type=\"application\/ld+json\" class=\"yoast-schema-graph\">{\"@context\":\"https:\/\/schema.org\",\"@graph\":[{\"@type\":\"Article\",\"@id\":\"https:\/\/astan.lk\/al_virtualclassroom\/p-block-elements-2\/#article\",\"isPartOf\":{\"@id\":\"https:\/\/astan.lk\/al_virtualclassroom\/p-block-elements-2\/\"},\"author\":{\"name\":\"Admin\",\"@id\":\"https:\/\/astan.lk\/al_virtualclassroom\/#\/schema\/person\/ffb0504e2cfb71518790b2fffd668c59\"},\"headline\":\"p block elements and their compounds\",\"datePublished\":\"2020-10-13T09:07:36+00:00\",\"dateModified\":\"2020-10-13T09:07:56+00:00\",\"mainEntityOfPage\":{\"@id\":\"https:\/\/astan.lk\/al_virtualclassroom\/p-block-elements-2\/\"},\"wordCount\":1225,\"commentCount\":0,\"publisher\":{\"@id\":\"https:\/\/astan.lk\/al_virtualclassroom\/#organization\"},\"image\":{\"@id\":\"https:\/\/astan.lk\/al_virtualclassroom\/p-block-elements-2\/#primaryimage\"},\"thumbnailUrl\":\"http:\/\/chemistry.need.org\/Files\/Haber%20Bosch%20Ammonia%20Process_0.jpg\",\"articleSection\":[\"Chemistry\",\"Unit 15\"],\"inLanguage\":\"en-US\",\"potentialAction\":[{\"@type\":\"CommentAction\",\"name\":\"Comment\",\"target\":[\"https:\/\/astan.lk\/al_virtualclassroom\/p-block-elements-2\/#respond\"]}]},{\"@type\":\"WebPage\",\"@id\":\"https:\/\/astan.lk\/al_virtualclassroom\/p-block-elements-2\/\",\"url\":\"https:\/\/astan.lk\/al_virtualclassroom\/p-block-elements-2\/\",\"name\":\"p block elements and their compounds - 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