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    se coloca encima o por debajo de la flecha e indica que se debe suministrar calor para que la reacción se lleve a cabo.

    Santiago

    Chicos, ¿alguien sabe la respuesta?

    obtenga se coloca encima o por debajo de la flecha e indica que se debe suministrar calor para que la reacción se lleve a cabo. de este sitio.

    Pregunta 1: Se coloca encima o por debajo de la flecha e indica que se debe suministrar calor para

    Encuentra una respuesta a tu pregunta Pregunta 1: Se coloca encima o por debajo de la flecha e indica que se debe suministrar calor para que la reacción se llev…

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    Pregunta 1: Se coloca encima o por debajo de la flecha e indica que se debe suministrar calor

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    simbolos auxiliares y tipos de reacciones quimicas

    SÍMBOLOS AUXILIARES Se utilizan para que una ecuación química represente lo mas exactamente posible una reacción, el sentido y las condiciones en que se...

    simbolos auxiliares y tipos de reacciones quimicas

    846 palabras 4 páginas

    Ver más SÍMBOLOS AUXILIARES

    Se utilizan para que una ecuación química represente lo mas exactamente posible una reacción, el sentido y las condiciones en que se realiza.

    Los cuales son los siguientes:

    Una flecha hacia la derecha indica que la reacción es irreversible.

    Una flecha hacia la derecha y otra a la izquierda indican que la reacción puede realizarse de izquierda a derecha y viceversa, es decir los productos pueden regresar a su estado original.

    Un triangulo encima de la flecha, indica que la reacción sólo se realizará si se le suministra calor.

    CaCO3 CaO + CO2

    Para indicar el estado físico de las sustancias se anota dentro de un paréntesis una (s) si la sustancia es un sólido, una (l) si es liquido, una (g) si la sustancia es un

    : Simboliza la energía calorífica.

    TIPOS DE REACCIONES QUIMICAS

    Reacciones de la química inorgánica

    Desde un punto de vista de la química inorgánica se pueden postular dos grandes modelos para las reacciones químicas de los compuestos inorgánicos: reacciones ácido-base o deneutralización (sin cambios en los estados de oxidación) y reacciones redox (con cambios en los estados de oxidación). Sin embargo, podemos clasificarlas de acuerdo al mecanismo de reacción y tipo de productos que resulta de la reacción. En esta clasificación entran las reacciones de síntesis (combinación), descomposición, de sustitución simple, de sustitución doble:

    Nombre Descripción Representación Ejemplo

    Reacción de síntesis

    Elementos o compuestos sencillos que se unen para formar un compuesto más complejo.

    La siguiente es la forma general que presentan este tipo de reacciones:

    A+B → AB

    Donde A y B representan cualquier sustancia química.

    Un ejemplo de este tipo de reacción es la síntesis del cloruro de sodio:

    2Na(s) + Cl2(g) → 2NaCl(s)

    Reacción de descomposición

    Un compuesto se fragmenta en elementos o compuestos más

    fuente : www.monografias.com

    Pasos para escribir las ecuaciones químicas

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    TUTORIAL DEL REACCIONES QUÍMICAS

    TUTORIAL DEL REACCIONES QUÍMICAS Pasos para escribir las Ecuaciones Químicas

    Una ecuación química usa los símbolos y fórmulas de los reactivos y productos, y otros términos simbólicos para representar una reacción química. Las ecuaciones se escriben siguiendo los siguientes pasos:

    Los reactivos se separan de los productos con una flecha ( ) que indica el sentido de la reacción. Una flecha doble ( ) indica que la reacción se efectúa en ambas direcciones y establece un equilibrio entre los reactivos y los productos.

    Los reactivos se colocan a la izquierda y los productos a la derecha de la flecha. Un signo (+) se coloca entre cada reactivo y entre cada producto, cuando es necesario.

    Las condiciones necesarias para efectuar la reacción pueden, si se desea, colocarse arriba o abajo de la flecha o signo de igualdad. Por ejemplo, una letra delta mayúscula () colocada sobre la flecha () indica que se suministra calor a la reacción.

    Se colocan coeficientes (números enteros) frente a los símbolos de las sustancias (por ejemplo, 2 H2O) para equilibrar o balancear la ecuación e indicar el número de unidades fórmula (átomos, moléculas, moles, iones) de cada sustancia que reacciona o que se produce. Cuando no se indica número alguno, se sobrentiende que se trata de una unidad fórmula.

    El estado físico de la sustancias se indica mediante los siguientes símbolos: () para el estado sólido; () para el estado líquido; () para el estado gaseoso; y () para las sustancias en solución acuosa.

    Empiece con las partes más complejas, es decir con los compuestos que tienen varios elementos. En algunos casos, simplemente consiste en ajustar primero los átomos diferentes al hidrógeno y al oxígeno.

    Ajuste el hidrógeno y el oxígeno agregando agua si es necesario, después de que todos los otros elementos estén balanceados.

    Deje los elementos en estado libre hasta el último momento, ya que cambiando los coeficientes de estos sólo cambian esta clase de átomos. Por ejemplo, cuando se escribe un 2 delante del H2O, se duplica el número de átomos de hidrógeno y oxígeno, pero cuando se escribe un 2 delante del Al sólo cambia el número de átomos de Al.

    Para reacciones con iones poliatómicos, ajuste el ion como grupo. Por ejemplo, el SO4-2 se ajusta como ion sulfato y no como átomos de S y átomos de O.

    Generalmente, si aparecen fracciones en la ecuación, se multiplica todo por el número más pequeño que elimine esta fracción. No es esencial hacer desaparecer las fracciones, sin embargo, es más simple en la mayoría de los casos. Además asegúrese al final, que todos los coeficientes estén en relación o proporción más baja posible; si no es el caso, simplifique.

    Considere el siguiente ejemplo:

    Recuerde que es conveniente empezar por la sustancia más compleja.

    Empezando por el fosfato de magnesio (la parte más compleja) y considerando el fosfato de magnesio como grupo, escribimos un 2 delante del H3PO4 para ajustar el grupo fosfato y un 3 delante de Mg(OH)2 para ajustar el Mg dando como resultado:

    Únicamente nos queda el hidrógeno y el oxígeno. Observando el hidrógeno, hay 12 átomos en la izquierda y por tanto necesitamos escribir un 6 delante del H2O. De igual forma se ajustan también los átomos de O que son en total 14. Esto da finalmente:

    Para revisar se puede sumar todos lo átomos de Mg, O, H, y P en cada lado de la ecuación. Esto da:

    Copyright © 2005 Portal Químico. Facultad de Ciencias Médicas.

    fuente : medicina.usac.edu.gt

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