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    cual es la composición porcentual de cada uno de los elementos en la molécula de agua

    Santiago

    Chicos, ¿alguien sabe la respuesta?

    obtenga cual es la composición porcentual de cada uno de los elementos en la molécula de agua de este sitio.

    cual es la composición porcentual del H2O? explicada

    Aprendizaje efectivo en grupo

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    cual es la composición porcentual del H2O? explicada - Brainly.lat

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    Composiciones porcentuales y fórmulas químicas

    Kimikaren oinarrizko lege baten arabera, konposatu kimiko guztiak bi edo elementu gehiagok osatu behar dute. Elementu horiek portzentaje kantitate edo konposizio jakin batean ageri dira konposatu horretan.

    Composiciones porcentuales y fórmulas químicas

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    La composición porcentual a través de la fórmula química

    La fórmula química de un compuesto a través de su composición porcentual

    El volumen molar

    Una ley fundamental de la química afirma que en todo compuesto químico que esté formado por dos o más elementos diferentes, éstos se encuentran presentes en dicho compuesto en una cantidad o composición porcentual determinada. Lo que quiere decir, por ejemplo, que el hidróxido de aluminio Al(OH)3 que se obtenga en España tendrá el mismo porcentaje de aluminio, de oxígeno y de hidrógeno que el que se pueda obtener en cualquier otra parte del mundo.

    La composición porcentual a través de la fórmula química

    Conocida la fórmula de un compuesto químico, es posible saber el porcentaje de masa con el que cada elemento que forma dicho compuesto está presente en el mismo.

    Ejemplo:

    Una molécula de dióxido de azufre, SO2, contiene un átomo de azufre y dos de oxígeno. Calcular la composición en tanto por ciento de dicha molécula.

    Datos: la masa atómica del azufre es 32,1 y la del oxígeno, 16,0 u.

    El problema puede resolverse por dos vías:

    Utilizando unidades de masa atómica:

    Masa molecular del SO2 = (32,1) + (2 · 16) = 64,1 u.

    Porcentaje de azufre en el compuesto:

    Porcentaje de oxígeno en el compuesto:

    Utilizando gramos:

    1 mol de moléculas de SO2 (64,1 g) contiene 1 mol de átomos de azufre (32,1 g) y 2 moles de átomos de oxígeno (16,0 g).

    Porcentaje de azufre en el compuesto:

    Si en 64,1 g de SO2 hay ® 32,1 g de azufre, en 100 g habrá ® x, luego

    Porcentaje de oxígeno en el compuesto:

    Si en 64,1 g de SO2 hay ® 32,0 g de oxígeno, en 100 g habrá ® x, luego

    La fórmula química de un compuesto a través de su composición porcentual

    Conocida la composición porcentual de un compuesto o su composición elemental en gramos, se puede determinar su fórmula más simple mediante cálculos elementales.

    La fórmula más simple o fórmula empírica de un compuesto es la menor relación entre el número de átomos presentes en una molécula de ese compuesto.

    A través de la composición porcentual de un compuesto, puede conocerse su fórmula empírica.

    Ejemplo:

    El análisis de una muestra de un compuesto puro revela que contiene un 27,3% de carbono y un 72,7% de oxígeno en masa. Determinar la fórmula empírica de ese compuesto.

    Para resolver el problema consideramos 100 g del compuesto. Dada la composición porcentual del mismo, de esos 100 g corresponden 27,3 al carbono y 72,7 al oxígeno. Con ello, se puede calcular el número de moles de átomos de cada elemento:

    Dividiendo los dos números obtenidos se llega a una relación empírica entera entre ambos, a partir de la cual se tiene la relación de átomos en la fórmula empírica:

    La fórmula empírica corresponde al CO2, dióxido de carbono.

    El volumen molar

    En los cálculos con gases es conveniente adoptar una unidad universal de volumen: el volumen molar. Se denomina así al volumen de cualquier gas, medido en condiciones normales de presión y temperatura (1 atmósfera y0 ºC). Este volumen molar tiene un valor de 22,4 l.

    Volumen molar

    Gas Masa Volumen en c.n. Número de partículas

    1 mol de helio 4 g 22,4 l 6,023 × 1023 átomos

    1 mol de hidrógeno 2 g 22,4 l 6,023 × 1023 moléculas

    1 mol de butano 58 g 22,4 l 6,023 × 1023 moléculas

    fuente : www.amarauna.euskadi.eus

    Ejemplo resuelto: cálculo del porcentaje en masa (video)

    Aprende gratuitamente sobre matemáticas, arte, programación, economía, física, química, biología, medicina, finanzas, historia y más. Khan Academy es una organización sin fines de lucro, con la misión de proveer una educación gratuita de clase mundial, para cualquier persona en cualquier lugar.

    Contenido principal

    Tiempo actual: 0:00Duración total:6:06

    Para calcular el porcentaje en masa de un elemento en un compuesto, dividimos la masa del elemento en 1 mol del compuesto entre la masa molar del compuesto y multiplicamos el resultado por 100. Creado por Sal Khan.

    ¿Quieres unirte a la conversación?

    Inicia sesión jacobobee06 hace 2 años

    Publicado hace hace 2 años. Enlace directo a la publicación “En este caso, ¿Cuál es el...” de jacobobee06

    En este caso, ¿Cuál es el porcentaje de el hidrogeno en la glucosa?

    • JACSZ hace 9 días

    Publicado hace hace 9 días. Enlace directo a la publicación “mas o menos seria asi hid...” de JACSZ

    mas o menos seria asi

    hidrogeno=7% oxigeno=53% carono=40%

    Gabriela Lizet Pérez Domínguez

    hace un año

    Publicado hace hace un año. Enlace directo a la publicación “Ejemplo de como se realiz...” de Gabriela Lizet Pérez Domínguez

    Ejemplo de como se realiza el cálculo de la composición porcentual

    • Axel Antonio Huerta hace 4 meses

    Publicado hace hace 4 meses. Enlace directo a la publicación “El compuesto PbSO4el elem...” de Axel Antonio Huerta

    El compuesto PbSO4el elemento químico presente en menor porcentaje es

    ¿Sabes inglés? Haz clic aquí para ver más discusiones en el sitio en inglés de Khan Academy.

    Transcripción del video

    por aquí tengo la fórmula molecular de la glucosa así que vamos a decir que tenemos una muestra de glucosa pura por aquí esta es la glucosa y no nos dicen su masa pero con base en su fórmula molecular podemos encontrar el porcentaje de la masa del carbono de la muestra pausa el vídeo y piénsalo y como pista nos dan la masa atómica promedio del carbono del hidrógeno y del oxígeno muy bien vamos a trabajar juntos la razón del por qué no importa la cantidad de glucosa es que el porcentaje de la masa del carbono debe de ser el mismo sin importar la cantidad para ayudarnos a pensar esto podemos imaginar una cierta cantidad de glucosa supongamos que tenemos un molde glucosa entonces ahora podemos pensar que si tenemos un molde glucosa tenemos 6 moldes de carbono porque cada molécula de glucosa tiene 6 átomos de carbono y con esto en mente podemos preguntarnos cuál será la masa de 6 moles de carbono dividido entre la masa de un molde glucosa una vez más la razón del por qué tenemos seis moldes de carbono es que si suponemos que este es un molde de glucosa y cada molécula de glucosa tiene seis átomos de carbono entonces habrá seis moles de carbono por cada molde glucosa ahora cuánto será esto bueno esto será igual a en nuestro numerador tendremos seis moles de carbono por la masa molecular del carbono cual es la masa molecular del carbono bueno podemos obtener la de la masa atómica promedio del carbono si la masa atómica promedio es de 12.01 unidades de masa atómica unificadas entonces tenemos 12.01 gramos por mol de carbono entonces esto por 12.01 gramos formol de carbono y podemos observar que en el numerador nos quedaremos sólo con gramos como unidades y ahora en el denominador que tendremos bueno necesitamos la masa de un molde glucosa ahora cada molécula de glucosa se forma con 6 átomos de carbono 12 de hidrógeno y 6 de oxígeno entonces necesitaremos la masa de 6 moles de carbono 12 moles de hidrógeno y 6 moles de oxígeno ahora vamos a dividir lo que tenemos aquí entre 6 moles de carbono por la masa molar del carbono que es 12.01 gramos por mol de carbono ya esto le sumaremos 12 moles de hidrógeno por la masa molar del hidrógeno que es 1.008 gramos por mol de hidrógeno más 6 moles de oxígeno por la masa molar del oxígeno que es 16.00 gramos por mol de oxígeno y la buena noticia es que los moles de los elementos se cancelan así que nos quedaremos con gramos como unidad del denominador y esto tiene mucho sentido ya que nos quedaremos con gramos en el numerador y con gramos en el denominador por lo que se cancelarán y obtendremos sólo un porcentaje al final y veamos en el numerador tenemos 6 por 12.01 es 72 puntos 0 6 mientras que en el denominador bueno primero hagamos los cálculos y después nos preocupamos por las cifras significativas en el denominador tendremos 72 puntos 0 6 + 12 por 1.008 es 12.0 96 y después tenemos 6 por 16 lo cual es 96.000 y esto será igual a 72 puntos 0 6 entre 72 más 12 es 84 96 es 180 0.06 más 0.0 96 es lo mismo que 0.156 lo hice bien sólo sumamos todo esto sin preocuparnos por las cifras significativas ahora podemos escribir esto en la calculadora pero debemos recordar que nuestra respuesta debes de tener más de cuatro cifras significativas incluso acá abajo en esta operación azul sólo deberíamos tener cuatro cifras significativas así que tenemos que obtener una respuesta hasta el lugar de los centésimos incluso en la suma si redondeamos con el fin de tener cifras significativas tendríamos al menos cuatro de hecho tendríamos cinco cifras significativas así que cuatro serán nuestro factor limitante de cifras significativas por lo tanto calculamos esto y vamos a redondear a cuatro cifras significativas 72.0 6 entre 180.169 firmas y si redondeamos a cuatro cifras significativas tendremos punto 4000 así que vamos a decir que esto es igual a punto 4000 o podemos decir que tenemos un 40 por ciento de la masa del carbono en nuestra muestra cuando redondeamos a cuatro cifras significativas y ya está hemos acabado

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    fuente : es.khanacademy.org

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    Santiago 8 day ago
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