{"id":40960,"date":"2019-09-25T13:41:09","date_gmt":"2019-09-25T12:41:09","guid":{"rendered":"https:\/\/www.thermal-engineering.org\/que-es-la-ley-de-avogadro-definicion\/"},"modified":"2020-01-13T10:48:03","modified_gmt":"2020-01-13T09:48:03","slug":"que-es-la-ley-de-avogadro-definicion","status":"publish","type":"post","link":"https:\/\/www.thermal-engineering.org\/es\/que-es-la-ley-de-avogadro-definicion\/","title":{"rendered":"\u00bfQu\u00e9 es la Ley de Avogadro? Definici\u00f3n"},"content":{"rendered":"<div class=\"su-quote su-quote-style-default\">\n<div class=\"su-quote-inner su-clearfix\">La Ley de Avogadro es una de las leyes del gas.\u00a0Avogadro estudi\u00f3 la relaci\u00f3n entre el volumen y la cantidad de sustancia del gas presente.<\/div>\n<\/div>\n<div class=\"su-divider su-divider-style-dotted\"><\/div>\n<div class=\"lgc-column lgc-grid-parent lgc-grid-100 lgc-tablet-grid-100 lgc-mobile-grid-100 lgc-equal-heights lgc-first lgc-last\">\n<div class=\"inside-grid-column\">\n<div class=\"su-spacer\"><\/div>\n<h2>Ley de Avogadro<\/h2>\n<p><strong>La Ley de Avogadro<\/strong>\u00a0es una de las leyes del gas.\u00a0A principios del siglo XIX, un cient\u00edfico italiano\u00a0<strong>Lorenzo Romano Amedeo Carlo Avogadro<\/strong>\u00a0estudi\u00f3 la relaci\u00f3n entre el\u00a0<strong>volumen<\/strong>\u00a0\u00a0y la\u00a0<strong>cantidad<\/strong>\u00a0de sustancia del gas presente.\u00a0Los resultados de ciertos experimentos con gases lo llevaron a formular una conocida\u00a0<strong>Ley de Avogadro<\/strong>\u00a0.\u00a0Establece que, bajo las mismas condiciones de temperatura y presi\u00f3n, vol\u00famenes iguales de gases diferentes contienen un n\u00famero igual de mol\u00e9culas, o:<\/p>\n<p><em>Para una masa fija de un gas ideal a presi\u00f3n y temperatura constantes, el volumen y la cantidad del gas son directamente proporcionales.<\/em><\/p>\n<p>Puede expresar esto matem\u00e1ticamente como:<\/p>\n<p><strong><em>V\u00a0<\/em><em>\u221d\u00a0<\/em><em>n<\/em><\/strong><\/p>\n<p>o<\/p>\n<p><strong><em>V = constante.\u00a0norte<\/em><\/strong><\/p>\n<p>donde nR \/ V es constante y:<\/p>\n<ul>\n<li><em>n<\/em>\u00a0es la cantidad de sustancia medida en moles<\/li>\n<li><em>V<\/em>\u00a0es el volumen del gas<\/li>\n<\/ul>\n<p>la constante es igual a RT \/ p, donde\u00a0<em>p<\/em>\u00a0es la presi\u00f3n absoluta del gas,\u00a0<em>T<\/em>\u00a0es la temperatura absoluta y\u00a0<em>R<\/em>\u00a0\u00a0es la constante de gas ideal o universal, igual al producto de la constante de Boltzmann y la constante de Avogadro.<\/p>\n<\/div>\n<\/div>\n<div class=\"lgc-column lgc-grid-parent lgc-grid-100 lgc-tablet-grid-100 lgc-mobile-grid-100 lgc-equal-heights lgc-first lgc-last\">\n<div class=\"inside-grid-column\">\n<div class=\"su-spacer\"><\/div>\n<h2>El n\u00famero de Avogadro<\/h2>\n<div class=\"lgc-column lgc-grid-parent lgc-grid-100 lgc-tablet-grid-100 lgc-mobile-grid-100 lgc-equal-heights  lgc-first lgc-last\">\n<div class=\"inside-grid-column\">\n<p><span>En homenaje a\u00a0<\/span><strong><span>Avogadro<\/span><\/strong><span>\u00a0, el n\u00famero de part\u00edculas (\u00e1tomos, mol\u00e9culas, iones u otras part\u00edculas) en\u00a0<\/span><strong><span>1 mol<\/span><\/strong><span>\u00a0de una sustancia,\u00a0<\/span><strong><span>6.022 \u00d7 10\u00a0<\/span><sup><span>23<\/span><\/sup><\/strong><span>\u00a0, fue nombrado despu\u00e9s de Avogadro como la\u00a0<\/span><strong><span>constante de\u00a0<\/span><\/strong><strong><span>Avogadro<\/span><\/strong><span>\u00a0o el\u00a0<strong>n\u00famero de Avogadro<\/strong>\u00a0.\u00a0La constante de Avogadro es una de las unidades de base SI siete y representada por\u00a0<\/span><em><span>N\u00a0<\/span><\/em><sub><span>A<\/span><\/sub><span>\u00a0.<\/span><\/p>\n<p><span>La\u00a0<\/span><strong><span>Ley de Avogadro<\/span><\/strong><span>\u00a0se puede usar para comparar la misma sustancia bajo dos conjuntos diferentes de condiciones:<\/span><\/p>\n<p><strong><em><span>V\u00a0<\/span><\/em><em><sub><span>1<\/span><\/sub><\/em><em><span>\u00a0\/ n\u00a0<\/span><\/em><em><sub><span>1<\/span><\/sub><\/em><em><span>\u00a0= V\u00a0<\/span><\/em><em><sub><span>2<\/span><\/sub><\/em><em><span>\u00a0\/ n\u00a0<\/span><\/em><em><sub><span>2<\/span><\/sub><\/em><\/strong><\/p>\n<\/div>\n<\/div>\n<div class=\"lgc-column lgc-grid-parent lgc-grid-100 lgc-tablet-grid-100 lgc-mobile-grid-100 lgc-equal-heights  lgc-first lgc-last\">\n<div class=\"inside-grid-column\">\n<div class=\"su-spacer\"><\/div>\n<h2><span>Volumen Molar de Gases<\/span><\/h2>\n<p><span>Uno de los resultados m\u00e1s pr\u00e1cticos de esta ley es el\u00a0<\/span><strong><span>volumen molar de un gas<\/span><\/strong><span>\u00a0,\u00a0<\/span><strong><span>V\u00a0<\/span><sub><span>m<\/span><\/sub><\/strong><span>\u00a0, que trata sobre:<\/span><\/p>\n<p><strong><span>V\u00a0<\/span><sub><span>m<\/span><\/sub><span>\u00a0= 22,4 dm\u00a0<\/span><sup><span>3<\/span><\/sup><span>\u00a0\/ mol<\/span><\/strong><\/p>\n<p><span>Significa que, a temperatura est\u00e1ndar (273.15 K, 0 \u00b0 C) y\u00a0<\/span><a title=\"Presi\u00f3n atmosf\u00e9rica\" href=\"https:\/\/www.nuclear-power.com\/nuclear-engineering\/thermodynamics\/thermodynamic-properties\/what-is-pressure-physics\/atmospheric-pressure\/\"><span>presi\u00f3n atmosf\u00e9rica<\/span><\/a><span>\u00a0est\u00e1ndar\u00a0(101.325 kPa), el volumen molar es el mismo para todos los gases ideales.\u00a0Tenga en cuenta que est\u00e1 bajo el supuesto de gas ideal.\u00a0Este valor depende en gran medida de la presi\u00f3n y la temperatura.\u00a0Por ejemplo:<\/span><\/p>\n<ul>\n<li><span>para 273.15 K (0 \u00b0 C) y 100.00 kPa, el volumen molar de un gas ideal es 22.71 dm\u00a0<\/span><sup><span>3<\/span><\/sup><span>\u00a0.mol\u00a0<\/span><sup><span>\u22121<\/span><\/sup><span>\u00a0.<\/span><\/li>\n<li><span>para 298.15 K (25 \u00b0 C) y 100.00 kPa, el volumen molar de un gas ideal es 24.79 dm\u00a0<\/span><sup><span>3<\/span><\/sup><span>\u00a0.mol\u00a0<\/span><sup><span>\u22121<\/span><\/sup><span>\u00a0.<\/span><\/li>\n<\/ul>\n<\/div>\n<\/div>\n<\/div>\n<\/div>\n<p>&#8230;&#8230;&#8230;&#8230;&#8230;&#8230;&#8230;&#8230;&#8230;&#8230;&#8230;&#8230;&#8230;&#8230;&#8230;&#8230;&#8230;&#8230;&#8230;&#8230;&#8230;&#8230;&#8230;&#8230;&#8230;&#8230;&#8230;&#8230;&#8230;&#8230;&#8230;&#8230;&#8230;&#8230;&#8230;&#8230;&#8230;&#8230;&#8230;&#8230;&#8230;&#8230;&#8230;&#8230;&#8230;&#8230;&#8230;&#8230;.<\/p>\n<p>Este art\u00edculo se basa en la traducci\u00f3n autom\u00e1tica del art\u00edculo original en ingl\u00e9s. Para m\u00e1s informaci\u00f3n vea el art\u00edculo en ingl\u00e9s. Puedes ayudarnos. Si desea corregir la traducci\u00f3n, env\u00edela a: translations@nuclear-power.com o complete el formulario de traducci\u00f3n en l\u00ednea. Agradecemos su ayuda, actualizaremos la traducci\u00f3n lo antes posible. Gracias.<\/p>\n","protected":false},"excerpt":{"rendered":"<p>La Ley de Avogadro es una de las leyes del gas.\u00a0Avogadro estudi\u00f3 la relaci\u00f3n entre el volumen y la cantidad de sustancia del gas presente. Ley de Avogadro La Ley de Avogadro\u00a0es una de las leyes del gas.\u00a0A principios del siglo XIX, un cient\u00edfico italiano\u00a0Lorenzo Romano Amedeo Carlo Avogadro\u00a0estudi\u00f3 la relaci\u00f3n entre el\u00a0volumen\u00a0\u00a0y la\u00a0cantidad\u00a0de sustancia &#8230; <a title=\"\u00bfQu\u00e9 es la Ley de Avogadro? 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