{"id":5967,"date":"2020-10-13T12:07:42","date_gmt":"2020-10-13T06:37:42","guid":{"rendered":"http:\/\/astan.lk\/al_virtualclassroom\/?p=5967"},"modified":"2020-10-13T12:08:15","modified_gmt":"2020-10-13T06:38:16","slug":"molecular-kinetic-theory","status":"publish","type":"post","link":"https:\/\/astan.lk\/al_virtualclassroom\/molecular-kinetic-theory\/","title":{"rendered":"Molecular kinetic theory"},"content":{"rendered":"<p><span style=\"text-decoration: underline;\"><strong>Assumptions of the molecular kinetic theory of an ideal gas<\/strong><\/span><\/p>\n<p>\u2022 Molecules move randomly in straight lines in all directions and at various speeds.<\/p>\n<p>\u2022 Gas molecules in random motion collide with each other and with the wall of the container. Such collisions are completely elastic.<\/p>\n<p>\u2022 There are no attractions or repulsions between molecules.<\/p>\n<p>\u2022 When compared with the distance between molecules, volume of molecules is considered as negligible. \u2022 When molecules collide with one another and bounce off the total kinetic energy of the system remains the same.<\/p>\n<p>\u2022 The pressure exerted by a gas is the result of collisions of the molecules on the walls of the container.<\/p>\n<p><strong>Molecular kinetic equation is\u00a0<\/strong><a href=\"http:\/\/astan.lk\/al_virtualclassroom\/wp-content\/uploads\/2017\/01\/pv.png\"><img loading=\"lazy\" decoding=\"async\" class=\"aligncenter wp-image-8477\" src=\"http:\/\/astan.lk\/al_virtualclassroom\/wp-content\/uploads\/2017\/01\/pv.png\" alt=\"pv\" width=\"193\" height=\"80\" \/><\/a><\/p>\n<p>P = pressure, V = volume of gas , \u00a0 \u00a0 m = mass of a gas particle\/molecule \u00a0 , \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 N = number of gas particles\/molecules<\/p>\n<p>_\u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 c\u00b2= mean square speed<\/p>\n<p>&nbsp;<\/p>\n<p><a href=\"http:\/\/astan.lk\/al_virtualclassroom\/wp-content\/uploads\/2017\/01\/cc.png\"><img loading=\"lazy\" decoding=\"async\" class=\"aligncenter wp-image-8486\" src=\"http:\/\/astan.lk\/al_virtualclassroom\/wp-content\/uploads\/2017\/01\/cc.png\" alt=\"cc\" width=\"318\" height=\"195\" \/><\/a><\/p>\n<p>&nbsp;<\/p>\n<p>&nbsp;<\/p>\n<p>The spreading of a certain type of molecules throughout space occupied by another type of molecules is called diffusion. \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 Example :- When a substance with a scent is kept inside a room, diffusion takes place until the scent is distributed uniformly throughout the room.<\/p>\n<p>Rate of diffusion &#8211; solids &lt; liquids &lt; gases<\/p>\n<p>It has been experimentally found that different gases diffuse at different rates. The production of ammonium chloride by the diffusion of ammonia and hydrogen chloride molecules through air can be demonstrated by the following apparatus. From this it is clear that the rate of diffusion of ammonia molecules with a low molecular mass is higher than that of hydrogen chloride molecules.<\/p>\n<p><a href=\"http:\/\/astan.lk\/al_virtualclassroom\/wp-content\/uploads\/2017\/01\/Diffusion__4-1.gif\"><img loading=\"lazy\" decoding=\"async\" class=\"aligncenter wp-image-8481\" src=\"http:\/\/astan.lk\/al_virtualclassroom\/wp-content\/uploads\/2017\/01\/Diffusion__4-1.gif\" alt=\"Diffusion__4 (1)\" width=\"256\" height=\"210\" \/><\/a><\/p>\n<p>Factors affecting the rate of diffusion of a gas &#8211; molar mass, area, concentration gradient and temperature.<\/p>\n<p><span style=\"text-decoration: underline;\"><strong>Variation of the mean speed of a gas with temperature is shown by the following Maxwell &#8211; Boltzmann curves.<\/strong> <\/span><\/p>\n<p><a href=\"http:\/\/astan.lk\/al_virtualclassroom\/wp-content\/uploads\/2017\/01\/CNX_Chem_09_05_MolSpeed21.jpg\"><img loading=\"lazy\" decoding=\"async\" class=\"aligncenter wp-image-8482\" src=\"http:\/\/astan.lk\/al_virtualclassroom\/wp-content\/uploads\/2017\/01\/CNX_Chem_09_05_MolSpeed21.jpg\" alt=\"CNX_Chem_09_05_MolSpeed21\" width=\"304\" height=\"239\" \/><\/a><\/p>\n<p>&nbsp;<\/p>\n","protected":false},"excerpt":{"rendered":"<p>Assumptions of the molecular kinetic theory of an ideal gas \u2022 Molecules move randomly in straight lines in all directions and at various speeds. \u2022 Gas molecules in random motion collide with each other and with the wall of the container. Such collisions are completely elastic. \u2022 There are no attractions or repulsions between molecules. [&hellip;]<\/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":[14,1658],"tags":[],"class_list":["post-5967","post","type-post","status-publish","format-standard","hentry","category-chemistry","category-unit-04"],"acf":[],"yoast_head":"<!-- This site is optimized with the Yoast SEO plugin v26.9 - https:\/\/yoast.com\/product\/yoast-seo-wordpress\/ -->\n<title>Molecular kinetic theory - Learning &amp; 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\/molecular-kinetic-theory\/\" \/>\n<meta property=\"og:locale\" content=\"en_US\" \/>\n<meta property=\"og:type\" content=\"article\" \/>\n<meta property=\"og:title\" content=\"Molecular kinetic theory - Learning &amp; Education Portal\" \/>\n<meta property=\"og:description\" content=\"Assumptions of the molecular kinetic theory of an ideal gas \u2022 Molecules move randomly in straight lines in all directions and at various speeds. \u2022 Gas molecules in random motion collide with each other and with the wall of the container. Such collisions are completely elastic. \u2022 There are no attractions or repulsions between molecules. 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