{"id":305,"date":"2024-04-01T14:12:21","date_gmt":"2024-04-01T13:12:21","guid":{"rendered":"https:\/\/tutors4you.com\/?page_id=305"},"modified":"2024-04-01T14:12:22","modified_gmt":"2024-04-01T13:12:22","slug":"basic-concepts-of-chemistry","status":"publish","type":"page","link":"https:\/\/tutors4you.com\/index.php\/basic-concepts-of-chemistry\/","title":{"rendered":"Basic Concepts of Chemistry"},"content":{"rendered":"\n\n\t\t<div class=\"well well-sm\">\n\t\t\t<h1>Basic Concepts of Chemistry<\/h1>\n\t\t\t<p align=\"left\"><font color=\"#FF0000\" face=\"Arial\"><b><u>Law\n        of Definite Proportion:<\/u><\/b><\/font><font\n        color=\"#004080\" face=\"Arial\"> We know that mass is\n        conserved. If we were to take a sample of a <strong>pure\n        compound <\/strong>it will always contain the <strong>same\n        elements <\/strong>combined in the <strong>same proportion<\/strong>\n        by mass.<\/font><\/p>\n        <p align=\"left\"><font color=\"#FF0000\" face=\"Arial\"><strong><u>Law\n        of Multiple Proportion:<\/u><\/strong> <\/font><font\n        color=\"#004080\" face=\"Arial\">If one element can combine\n        with another to form more than one compound then the <strong>mass\n        ratios<\/strong> of the elements in the compounds are <strong>simple<\/strong>\n        <strong>whole-number ratios<\/strong> of each other.<\/font><\/p>\n        <p align=\"left\"><font color=\"#FF0000\" face=\"Arial\"><strong><u>Law\n        of Definite Proportion by Volume:<\/u><\/strong> <\/font><font\n        color=\"#004080\" face=\"Arial\">The volumes of <strong>reactants\n        and products<\/strong>, in chemical reactions, are related\n        to each other by <strong>simple whole-numbers<\/strong>.\n        Of course the measurements must be taken at the same\n        temperature and pressure.<\/font><\/p>\n        <p align=\"left\"><font color=\"#FF0000\" face=\"Arial\"><strong><u>Law\n        of Reciprocal Proportions:<\/u><\/strong><\/font><font\n        color=\"#004080\" face=\"Arial\"> The ratio by mass, in which\n        two elements combine with the <strong>fixed mass<\/strong>\n        of a third element, is either the <strong>same or a\n        simple multiple<\/strong> of the ratio in which they\n        combine with each other.<\/font><\/p>\n        <p align=\"left\"><font color=\"#FF0000\" face=\"Arial\"><strong><u>Avogardo&#8217;s\n        Law:<\/u><\/strong><\/font><font color=\"#004080\"\n        face=\"Arial\"> <strong>Equal volumes<\/strong> of all gases\n        contain <strong>equal number of molecules<\/strong> under\n        similar conditions of temperature and pressure.<\/font><\/p>\n        <p align=\"left\"><font color=\"#FF0000\" face=\"Arial\"><strong><u>One\n        Atomic Mass Unit (amu):<\/u><\/strong><\/font><font\n        color=\"#004080\" face=\"Arial\"> It is a mass unit equal to\n        exactly one twelfth the mass of a carbon 12 atom.<\/font><\/p>\n        <p align=\"left\"><font color=\"#FF0000\" face=\"Arial\"><strong><u>Formula\n        Mass of a Substance:<\/u><\/strong><\/font><font\n        color=\"#008080\" face=\"Arial\"> <\/font><font\n        color=\"#004080\" face=\"Arial\">It is the <strong>sum of the\n        atomic masses<\/strong> of all atoms in a formula unit of\n        a compound.<\/font><\/p>\n        <p align=\"left\"><font color=\"#FF0000\" face=\"Arial\"><strong><u>Molar\n        Mass:<\/u><\/strong> <\/font><font color=\"#004080\"\n        face=\"Arial\">The mass of 1 mole of any substance.<\/font><\/p>\n        <p align=\"left\"><a name=\"Molar Volume\"><font\n        color=\"#FF0000\" face=\"Arial\"><strong><u>Molar Volume <\/u><\/strong><strong>(V<\/strong><sub><strong>m<\/strong><\/sub><strong>)<\/strong><\/font><\/a><font\n        color=\"#FF0000\" face=\"Arial\"><strong>:<\/strong> <\/font><font\n        color=\"#004080\" face=\"Arial\">The volume of 1 mole of the\n        substance.<\/font><\/p>\n        <p align=\"left\"><font color=\"#FF0000\" face=\"Arial\"><strong><u>Mole\n        (m):<\/u><\/strong><\/font><\/p>\n        <ul>\n            <li><p align=\"left\"><font color=\"#004080\"\n                face=\"Arial\">It is a number which is equal to <strong>6.023\n                x 10<\/strong><sup><strong>23<\/strong><\/sup><strong>\n                <\/strong>.<\/font><\/p>\n            <\/li>\n            <li><p align=\"left\"><font color=\"#004080\"\n                face=\"Arial\">It is the amount of substance which\n                contains as many entities (atoms, molecules, ions\n                or other particles) as there are <strong>atoms in\n                exactly 12 grams<\/strong> of Carbon 12 isotope.<\/font><\/p>\n            <\/li>\n            <li><p align=\"left\"><font color=\"#004080\"\n                face=\"Arial\">It is also known as <strong>Avogadro&#8217;s\n                Constant<\/strong>.<\/font><\/p>\n            <\/li>\n        <\/ul>\n        <p align=\"left\"><font color=\"#FF0000\" face=\"Arial\"><strong><u>Number\n        of Mole Method:<\/u><\/strong><\/font><\/p>\n        <p align=\"left\"><font color=\"#004080\" face=\"Arial\">Number\n        of moles of a substance n = w (in gms)\/m<\/font><\/p>\n        <p align=\"left\"><font color=\"#004080\" face=\"Arial\">also n\n        = volume (in lt) at NTP\/22.4lt<\/font><\/p>\n        <p align=\"left\"><font color=\"#004080\" face=\"Arial\">also n\n        = M x vol in lt (where M is Molarity = number of moles of\n        solute per lt of solution)<\/font><\/p>\n        <p align=\"left\"><font color=\"#004080\" face=\"Arial\">M=\n        (w\/m) x (1000\/ <\/font><a href=\"#Molar Volume\"><font\n        color=\"#004080\" face=\"Arial\">V<sub>m<\/sub><\/font><\/a><font\n        color=\"#004080\" face=\"Arial\"> )<\/font><\/p>\n        <p align=\"left\"><font color=\"#004080\" face=\"Arial\">Number\n        of mole method is used only in the case of <strong>balanced\n        chemical equations<\/strong>.<\/font><\/p>\n        <p align=\"left\"><font color=\"#004080\" face=\"Arial\">The\n        coefficients of balanced equations represent the ratios\n        in terms of <strong>number of moles<\/strong> in which the\n        reactants react or products are formed.<\/font><\/p>\n        <p align=\"left\"><font color=\"#004080\" face=\"Arial\">Number\n        of particles(ions, atoms or molecules) in a given number\n        of moles = number of moles x 6.023 x 10<sup>23<\/sup> .<\/font><\/p>\n        <p align=\"left\"><font color=\"#FF0000\" face=\"Arial\"><strong><u>Equivalent\n        Weight of an Element (E):<\/u><\/strong> <\/font><font\n        color=\"#004080\" face=\"Arial\">It is defined as the number\n        of parts by weight of the element which combine with or\n        displace from a compund 1 part by weight of Hydrogen, 8\n        parts by weight of Oxygen or 35.5 parts by weight of\n        Chlorine.<\/font><\/p>\n        <p align=\"left\"><font color=\"#004080\" face=\"Arial\">E = M\n        ( Molar Mass) \/ n<sub>f<\/sub> (n factor)<\/font><\/p>\n        <p align=\"left\"><font color=\"#004080\" face=\"Arial\">where:<\/font><\/p>\n        <p align=\"left\"><font color=\"#004080\" face=\"Arial\">n<sub>f<\/sub>\n        = Valency in case of an atom<\/font><\/p>\n        <p align=\"left\"><font color=\"#004080\" face=\"Arial\">=\n        Total positive or negative oxidation number of an atom in\n        a molecule<\/font><\/p>\n        <p align=\"left\"><font color=\"#004080\" face=\"Arial\">=\n        Basicity or Acidity.<\/font><\/p>\n        <p align=\"left\"><font color=\"#004080\" face=\"Arial\">=\n        Change in oxidation number in case of a redox reacton.<\/font><\/p>\n        <p align=\"left\"><font color=\"#FF0000\" face=\"Arial\"><strong><u>Number\n        of Gram Equivalents:<\/u><\/strong><\/font><\/p>\n        <p align=\"left\"><font color=\"#004080\" face=\"Arial\">=\n        weight in gms \/ E (Equivalent wt)<\/font><\/p>\n        <p align=\"left\"><font color=\"#004080\" face=\"Arial\">=\n        Normality x vol in lt<\/font><\/p>\n        <p align=\"left\"><font color=\"#004080\" face=\"Arial\">Normality\n        = (w\/E) x (1000\/<\/font><a href=\"#Molar Volume\"><font\n        color=\"#004080\" face=\"Arial\">V<sub>m<\/sub><\/font><\/a><font\n        color=\"#004080\" face=\"Arial\"><sub> <\/sub>)<\/font><\/p>\n        <p align=\"left\"><font color=\"#FF0000\" face=\"Arial\"><strong><u>Number\n        of Equivalents Method:<\/u><\/strong> <\/font><font\n        color=\"#004080\" face=\"Arial\">In this method you need not\n        balance the chemical equation. The basic principle is\n        that the equivalents of each reactant which have\n        dissapeared are equal to the number of equivalents of\n        each of the products formed. The working tool for this is\n        equivalent weight.<\/font><\/p>\n        <p align=\"left\"><font color=\"#004080\" face=\"Arial\">Number\n        of equivalents = W in gms \/ Eq Wt = (W x n<sub>f<\/sub> )\n        \/ M<\/font><\/p>\n        <p align=\"left\"><font color=\"#FF0000\" face=\"Arial\"><strong><u>Dulong\n        and Petit&#8217;s Law:<\/u><\/strong><\/font><font color=\"#004080\"\n        face=\"Arial\"> <\/font><\/p>\n        <p align=\"left\"><font color=\"#004080\" face=\"Arial\">Atomic\n        wt (approx) = 6.4\/specific heat(in calories)<\/font><\/p>\n\t\t\n\t\t<\/div>\n\t\n","protected":false},"excerpt":{"rendered":"<p>Basic Concepts of Chemistry Law of Definite Proportion: We know that mass is conserved. If we were to take a sample of a pure compound it will always contain the same elements combined in the same proportion by mass. Law of Multiple Proportion: If one element can combine with another to form more than one [&hellip;]<\/p>\n","protected":false},"author":1,"featured_media":0,"parent":0,"menu_order":0,"comment_status":"closed","ping_status":"closed","template":"","meta":{"footnotes":""},"class_list":["post-305","page","type-page","status-publish","hentry"],"blocksy_meta":[],"yoast_head":"<!-- This site is optimized with the Yoast SEO plugin v25.9 - https:\/\/yoast.com\/wordpress\/plugins\/seo\/ -->\n<title>Basic Concepts of Chemistry - Tutors 4 You<\/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:\/\/tutors4you.com\/index.php\/basic-concepts-of-chemistry\/\" \/>\n<meta property=\"og:locale\" content=\"en_US\" \/>\n<meta property=\"og:type\" content=\"article\" \/>\n<meta property=\"og:title\" content=\"Basic Concepts of Chemistry - Tutors 4 You\" \/>\n<meta property=\"og:description\" content=\"Basic Concepts of Chemistry Law of Definite Proportion: We know that mass is conserved. 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