{"id":8198,"date":"2022-08-24T06:01:25","date_gmt":"2022-08-24T06:01:25","guid":{"rendered":"https:\/\/physics.educour.in\/isc-physics\/?page_id=8198"},"modified":"2022-08-24T06:12:58","modified_gmt":"2022-08-24T06:12:58","slug":"kinetic-theory-of-gases-class-11-isc-physics","status":"publish","type":"page","link":"https:\/\/physics.educour.in\/isc-physics\/kinetic-theory-of-gases-class-11-isc-physics\/","title":{"rendered":"Kinetic Theory of Gases Class 11 ISC Physics"},"content":{"rendered":"\t\t
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Kinetic Theory of Gases<\/h1>\t\t\t\t\t\t\t\t<\/div>\n\t\t\t\t<\/div>\n\t\t\t\t
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ISC Syllabus<\/h2>\t\t\t\t\t\t\t\t<\/div>\n\t\t\t\t<\/div>\n\t\t\t\t
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Kinetic Theory: Equation of state of a perfect\u00a0gas, work done in compressing a gas. Kinetic\u00a0theory of gases – assumptions, concept of\u00a0pressure. Kinetic interpretation of\u00a0temperature; rms speed of gas molecules;\u00a0degrees of freedom, law of equi-partition of\u00a0energy (statement only) and application to
specific heat capacities of gases; concept\u00a0of mean free path, Avogadro’s number.<\/p>\t\t\t\t\t\t\t\t<\/div>\n\t\t\t\t<\/div>\n\t\t\t\t

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Elaboration of Syllabus<\/h3>\t\t\t\t\t\t\t\t<\/div>\n\t\t\t\t<\/div>\n\t\t\t\t
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(a) Kinetic Theory of gases; derive p=1\/3(\u03c1 2<\/sup> c )from the assumptions and applying Newton\u2019s laws of motion. The average thermal velocity (rms value) crms<\/sub>=\u221a3p\/\u03c1;\u00a0calculations for air, hydrogen and their\u00a0comparison with common speeds. Effect\u00a0of temperature and pressure on rms\u00a0speed of gas molecules.\u00a0[Note that pV=nRT the ideal gas\u00a0equation cannot be derived from kinetic\u00a0theory of ideal gas. Hence, neither can\u00a0other gas laws; pV=nRT is an
experimental result. Comparing this\u00a0with p = \u2153 (\u03c1 2<\/sup> c) , from kinetic theory of
gases, a kinetic interpretation of\u00a0temperature can be obtained as\u00a0explained in the next subunit]<\/p>\t\t\t\t\t\t\t\t<\/div>\n\t\t\t\t<\/div>\n\t\t\t\t

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(b) From kinetic theory for an deal gas (obeying all the assumptions
especially no intermolecular attraction\u00a0and negligibly small size of molecules,
we get p = (1\/3)\u03c1 2<\/sup> c or pV = (1\/3)M 2<\/sup> c .
(No further, as temperature is not a\u00a0concept of kinetic theory). From\u00a0 experimentally obtained gas laws, we\u00a0have the ideal gas equation (obeyed by
some gases at low pressure and high\u00a0temperature) pV = RT for one mole.
Combining these two results (assuming they can be combined), RT=(1\/3)M2<\/sup> c =(2\/3).\u00bdM2<\/sup> c =(2\/3)K;\u00a0Hence, kinetic energy of 1 mole of an\u00a0ideal gas K=(3\/2)RT. Average K for 1\u00a0molecule = K\/N = (3\/2) RT\/N = (3\/2) kT\u00a0where k is Boltzmann\u2019s constant. So,\u00a0temperature T can be interpreted as a\u00a0measure of the average kinetic energy of\u00a0the molecules of a gas.<\/p>

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(c) Degrees of freedom and calculation of\u00a0specific heat capacities for all types of\u00a0gases. Concept of the law of\u00a0equipartition of energy (derivation not
required). Concept of mean free path and Avogadro\u2019s number NA<\/sub>.<\/p>\t\t\t\t\t\t\t\t<\/div>\n\t\t\t\t<\/div>\n\t\t\t\t

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Kinetic Theory of Gases (Video + Class Notes)<\/span><\/h4>

(a) Gas Laws<\/a><\/p>

(b) Pressure of an Ideal Gas (Derivation using KTG)<\/a><\/p>

(c) Root Mean Square speed and Average Kinetic Energy of Gas molecule.<\/a><\/p>

(d) Derivation of Gas Laws<\/a><\/p>

(e) Law of Equipartition of energy<\/a><\/p>

(f) Mean Free Path<\/a><\/p>\t\t\t\t\t\t\t\t<\/div>\n\t\t\t\t<\/div>\n\t\t\t\t\t<\/div>\n\t\t<\/div>\n\t\t\t\t\t<\/div>\n\t\t<\/section>\n\t\t\t\t<\/div>\n\t\t","protected":false},"excerpt":{"rendered":"

Kinetic Theory of Gases ISC Syllabus Kinetic Theory: Equation of state of a perfect gas, work done in compressing a gas. Kinetic theory of gases – assumptions, concept of pressure. Kinetic interpretation of temperature; rms speed of gas molecules; degrees of freedom, law of equi-partition of energy (statement only) and application to specific heat capacities of gases; concept of mean free path, … Read more<\/a><\/p>\n","protected":false},"author":1,"featured_media":0,"parent":0,"menu_order":0,"comment_status":"closed","ping_status":"closed","template":"","meta":{"footnotes":""},"folder":[42],"class_list":["post-8198","page","type-page","status-publish"],"_links":{"self":[{"href":"https:\/\/physics.educour.in\/isc-physics\/wp-json\/wp\/v2\/pages\/8198","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/physics.educour.in\/isc-physics\/wp-json\/wp\/v2\/pages"}],"about":[{"href":"https:\/\/physics.educour.in\/isc-physics\/wp-json\/wp\/v2\/types\/page"}],"author":[{"embeddable":true,"href":"https:\/\/physics.educour.in\/isc-physics\/wp-json\/wp\/v2\/users\/1"}],"replies":[{"embeddable":true,"href":"https:\/\/physics.educour.in\/isc-physics\/wp-json\/wp\/v2\/comments?post=8198"}],"version-history":[{"count":20,"href":"https:\/\/physics.educour.in\/isc-physics\/wp-json\/wp\/v2\/pages\/8198\/revisions"}],"predecessor-version":[{"id":8219,"href":"https:\/\/physics.educour.in\/isc-physics\/wp-json\/wp\/v2\/pages\/8198\/revisions\/8219"}],"wp:attachment":[{"href":"https:\/\/physics.educour.in\/isc-physics\/wp-json\/wp\/v2\/media?parent=8198"}],"wp:term":[{"taxonomy":"folder","embeddable":true,"href":"https:\/\/physics.educour.in\/isc-physics\/wp-json\/wp\/v2\/folder?post=8198"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}