PRACTICA PRACTICA Nº 03
REACCIONES QUÍMICAS
I.
OBJETIVOS
Estudiar e identificar los diferentes tipos de reacciones químicas que se producen comúnmente en el laboratorio
II.
GENERALIDADES
La reacción química es el proceso en el cual una sustancia (o sustancias) cambia para formar una o más sustancias nuevas. La ecuación química es la forma de representar matemáticamente el proceso en el que una o más sustancias — los los reactantes — se se transforman en otras sustancias diferentes — los los productos de la reacción. Entre los principales tipos de reacciones químicas tenemos: 1. Reacciones de de adición (síntesis) 2. Reacciones de descomposición descomposición 3. Reacciones de de desplazamiento desplazamiento simple. 4. Reacciones de doble desplazamiento. 5. Reacciones de con transferencia de electrones electrones (REDOX). III. MATERIALES Y REACTIVOS Materiales: Materiales:
- 1 Mechero Bunsen Bunsen - 15 Tubos de ensayo ensayo - 1 Gradilla - 1 Pinza para tubos - 1 Pinza - 1 cápsula Reactivos y sustancias: sustancias:
- Cinta de Magnesio
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- Solución de Sulfato de Cobre CuSO4 0,1M - Granallas de Zinc Zinc - Solución de Nitrato Nitrato de Plata AgNO3 0,1 M - Solución de Yoduro Yoduro de Potasio 0,1M - Solución de acetato de plomo plomo 0,1M - Solución de cloruro de Sodio Sodio 0,5 % - Solución de permanganato de potasio 0,3% - Acido nítrico 0,1 M - Solución de fenolftaleína - Una pieza pequeña de plata (muestra proporcionada por el alumno) - Agua Oxigenada (muestra proporcionada por el alumno 10 ml por grupo) - Alambre de cobre (muestra proporcionada por el alumno) - Fósforos (material proporcionado por el alumno) - Clavo de 2 pulgadas para madera nuevo (material proporcionado por el alumno) IV. PROCEDIMIENTO EXPERIMENTAL
Las reacciones que vamos a realizar tienen por objeto comprobar si se llevan a cabo o no y escribir las ecuaciones químicas con los productos respectivos. a)
Tomar con pinzas un pedazo de cinta de magnesio y calentar. Observar las cenizas colocadas en un mortero o capsula. Luego añadir agua destilada y agitar, observar lo que sucede y escribir las ecuaciones químicas respectivas. Finalmente añada unas gotas de fenolftaleína. +
O2 (g)
Mg+2 O-2
MgO(s) +
H2O
Mg (OH) 2
Mg (s)
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b) En un tubo de ensayo que contenga 3 mL de KI 0,1 M adicione gota a gota 1 mL mL de (CH3COO)2 Pb (Precaución mantenga alejado el tubo de la cara). Observa el fondo del tubo. KI(ac) + (CH3COO)2 Pb(ac)
K +1 (CH3COO)2-1 + Pb+2 I2-1
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c) A 3 ml de la solución de Nitrato de Plata AgNO 3 agregue 3 ml de la solución de Cloruro de sodio NaCl. AgNO3(ac) + NaCl(ac)
+
Ag
Cl- + NaNO3
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d) En un tubo de ensayo colocar 3 ml de solución de Nitrato de Plata AgNO 3, introduzca una granalla de Zinc. AgNO3(ac) +
Zn(s)
Zn (NO)2 + Ag
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e) A 3 ml de solución de de Sulfato de cobre agregue una granalla de zinc, agite y deje reposar por 10 minutos, observe con cuidado las coloraciones de la solución y del metal CuSO4(ac) + Zn(s)
Cu Zn2 + (SOH) 2
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f)
En un tubo de ensayo colocar 5 mL de sulfato de cobre, luego introduzca el clavo clavo para madera (Fe), agite y deje rreposar eposar por 10 minutos, observar los productos formados. CuSO4(ac) + Fe(s)
Cu
Fe2 + (SOH)2
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g) En un tubo de ensayo colocar 1 ml de solución de Permanganato de Potasio KMnO 4, agregar 1 ml de Agua Oxigenada ( H2O2) KMnO4(ac)
+
H2O2(ac) FALTA RESOLUCION
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h) En un tubo de ensayo colocar 3 ml de Solución de AgNO 3, introduzca una pieza pequeña de plata, plata, repita repita la la experien experiencia cia con con CuSO4(ac) AgNO3(ac) + Ag Ag(s)
NO SE DESARROLLO
i) En un tubo de ensayo colocar 3 ml de solución de Nitrato de Plata AgNO 3, introduzca un alambre de cobre. AgNO3(ac) + Cu Cu(s)
Ag Cu + NO3
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j)
Utilizando un mortero o cápsula quemar un trozo de papel. Describa la reacción y escriba la ecuación química respectiva.
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V.
RESULTADOS Y DISCUSIONES 1)
Elaborar una tabla general que indique la reactividad o no de los compuestos.
Compuesto
MgO(s)
Mg(OH)2
PBI2 + 2CH3COOK
AgCl + NaNO3
Ag + Zn(NO3)2
Reactividad
No Reactividad
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2)
Describa las características de los reactivos en cada experimento
Aspecto y color: Polvo blanco, muy fino.
Olor: Inodoro.
Absorbe fácilmente humedad y dióxido de
MgO
carbono cuando se expone al aire.
(óxido de magnesio)
Reacciona vigorosamente con halógenos y ácidos fuertes.
Apariencia: Blanco
Masa molar: 58,3 molar: 58,3 g/mol
Punto de fusión: de fusión: 623 623 K (350 °C)
Solubilidad en agua: 12 mg en 1 L de agua
antiácido usado para aliviar la pirosis la pirosis (acidez o
Mg(OH) 2
(hidróxido de magnesio)
calor estomacal) PBI2 + 2CH3COOK
Cristales o polvo amarillo dorado
Inodoro Soluble en yoduro potásico y soluciones de
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Nitrato de zinc:
Ag + Zn(NO3)2
Su estado físico es sólido.
Apariencia: cristales incoloros a blancos.
pH: 3.5 - 5.5 (solución acuosa acuosa al 5% a 25°C). Compuesto químico cristalino, incoloro, soluble en agua
ZnSO4 + Cu
FeSO4 + Cu
Olor: Sin olor.
Ligeramente soluble en etanol.
Forma de cristales blancos o azules verdosos Óxido de manganeso: Se trata de un polvo de color negro-marrón que reacciona violentamente con el aluminio al calentarlo a altas temperaturas.
MnO2 + KOH + O 2 + H2O
Hidróxido de potasio: Se trata de un sólido de color blanco con
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3)
Describa lo ocurrido en cada experimento
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4)
Escriba las ecuaciones que se llevaron a cabo a. Mg (s) + O2 (g) Mg+2 O-2
MgO(s) + H2O Mg (OH) 2
b. KI(ac) + (CH3COO)2 Pb(ac)
c. AgNO3(ac) + NaCl(ac)
d. AgNO3(ac) +
Zn(s)
e. CuSO4(ac) + Zn(s)
f. CuSO4(ac) + Fe(s)
K +1 (CH3COO)2-1 + Pb+2 I2-1
Ag+ Cl- + NaNO3
Zn (NO)2 + Ag
Cu Zn2 + (SOH) 2
Cu Fe2 + (SOH)2
g. KMnO4(ac) + H2O2(ac) MnO2 + KOH + O 2 + H2O
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5)
Indique las características de los productos formados
•Mg: El magnesio es un metal ligero pero considerablemente duro, de color blanco y
plateado. Es el octavo elemento más abundante en la corteza terrestre de nuestro planeta, ocupando el 2% de ésta, y aunque aunque en estado puro no se lo puede puede encontrar en la naturaleza, sí se lo puede hallar en grandes depósitos en forma de magnesita, dolomita y algunos otros minerales, pero no existe fuera de compuestos. •O2: El oxígeno es un gas incoloro en estado líquido y sólido toma un color azul
pálido, inodoro e insípido que integra el grupo de los anfígenos de la tabla periódica y
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anhídrida (CuSO4) es un polvo verde o gris-blanco pálido, mientras que la forma hidratada (CuSO4•5H2O) es azul brillante. •
Fe(s): Es un un metal maleable, maleable, de color color gris plateado y presenta propiedades propiedades
magnéticas; es ferromagnético a temperatura ambiente y presión atmosférica. Es extremadamente duro y denso. •
KMnO4: El permanganato permanganato de potasio, permanganato permanganato potásico, minerales
chamaleon, cristales de Condy, (KMnO4) es un compuesto químico formado por iones de potasio (K+) y permanganato (MnO4−). Es un f uerte agente oxidante. Tanto sólido
como en solución acuosa presenta un color violeta intenso. •
H2O2(ac)
: Es un líquido viscoso, conocido por ser un poderoso oxidante.
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6)
Identificar qué tipos de reacciones se han dado en las experiencias anteriores
Reacciones
Mg (s)
+
MgO(s) +
O2 (g)
H2O
Tipo de Reacción
MgO(s)
Mg(OH)2
Reacción de adición (síntesis)
Reacción de adición (síntesis)
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CuSO4 (ac) + Fe Fe(s)
FeSO4 + Cu
Reacción de desplazamiento simple
Reacción de con transferencia de KMnO4 (ac)
+
H2O2(ac) MnO2 + KOH +
O2 + H2O
electrones (REDOX).
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VI. CONCLUSIONES
Las reacciones dadas en este laboratorio, son ejemplos muy claros de casos que pueden pasar a diario y que nosotros no analizamos, los pasamos por alto, sabiendo que en ellos podemos aprender mucho sobre conceptos básicos de química.
Las reacciones químicas son de suma importancia ya que son fenómenos que vemos a diario en nuestra vida y son la base de la realización de las funciones vitales y las demás actividades del hombre o cualquier otro ser vivo, como por ejemplo la respiración es una reacción química, ya que al organismo entra O2 y sale CO2. Además todas las sustancias que usamos o usan los demás seres vivos fueron producto de reacciones químicas.
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VI BIBLIOGRAFIA
http://www.monografias.com/trabajos104/practica-laboratorio-clases-reaccionesquimicas/practica-laboratorio-clases-reacciones-quimicas.shtml