First Research
1 .- Definition of plating or electroplating.
"The galvanosplastía is a process using electricity, a metal is placed over another. It does carry an electric current of the submerged foils (anode) to the object that has a lining through a metal salt solution (electrolysis). The metal ions are attracted by objects that are lined and
here shed their electrical charges and are deposited on their surfaces
. "
Electrolysis is an electrochemical process which produces the chemical breakdown of a substance by passing an electric current.
1. © Copyright 1996 - 2004, Multimedia Ecological Environment. Ecological Dictionary: http://www.ambiente-ecologico.com/ediciones/diccionarioEcologico/diccionarioEcologico.php3?letra=G&numero=01&rango=GAIA_-_GIPS% C3% 93FILO
2. This page was last modified at 00:14, 24 September, 2005. Electrolysis http://www.uc.cl/quimica/agua/glos2.htm
3. oxidation-reduction. Image available on the Web
equation 2 .- Concepts chemical and chemical reaction. Elements.
chemical equation: is the formal representation of a chemical reaction in terms symbols of elements and formulas of the compounds involved in chemical processing.
Chemical reaction: process during which a substance (or substances) to make a change or more new substances.
4.
Glossary. Chemical equation. Available in 5. QUIMIKA Copyright © 2004-2005. www.quimika.com / sections / diccionario.htm
3 .- The difference between these two concepts.
- esros The difference between two concepts is that the chemical reaction is the Prosesa of the union of the reactants, while the chemical equations is the symbolic representation of the expresinon.
"The chemical reactions are substances that change, to form new substances, while the chemical equation symbolically describes the components involved in the reaction.
"In the chemical reaction, bonds in the reactants are broken and new bonds forming stem products. The chemical reaction is represented by the chemical equation, which is equal training new links.
eg
Unadjusted H2O H2 + O2 ===
Adjusted: 2 H2 + O2 2 H2O ===
6. CHEMICAL REACTIONS . Accessed on 26 September, available on the Web http://www.teletel.com.ar/quimica/reacciones_quimicas.htm
7. The National Science Foundation Contact us / Report a Bug Copyright © 2003 - 2005, Vision Learning, Inc. http://www.visionlearning.com/library/module_viewer.php?mid=56&l = s & c3
8. This web page belongs to Librys.com. Available online http://ptro1.tripod.com/chemistry/id5.html
4 .- Criteria for classifying chemical reactions.
NAME EXPLANATION EXAMPLE composition or synthesis is that where two or more substances unite ra p to form a single product decomposition or analysis O incurs when an atom replaces another in a molecule: Neutralization E n it an acid reacts with a base to form a salt and water release. H 2 SO 4 (c) → Displacement An atom replaces another in a molecule → Exchange or double displacement S and performed by exchange of atoms between related substances K 2 S + → No electron transfer Only present a redistribution of the elements to form other substances. There is no exchange of electrons. With electron transfer (redox) There is change in the number of atoms in oxidation of some reagents for products. 2NaH 2Na (s) + H 2 (g) → DH = 54.85 kcal
2CaO (s) + H 2 O (l) → Ca (OH ) 2 (c)
2HgO ( s ) → 2HG (l) + O 2 (g)
+ 2NaOH (c) Na 2 SO 4 (c) + 2H 2 O (l)
CuSO4 + Fe FeSO4 + Cu
MgSO 4 K 2 SO 4 + MGS double displacement reactions synthesis reactions, decomposition, displacement endothermic reaction is that you need to supply heat to be conducted.
exothermic reaction is one that releases heat when it occurs.
2C (graphite) + H 2 (g) C 2 H 2 (g)
http://www.cespro.com/Materias/MatContenidos/Contquimica/
5 .- Table to classify the different chemical reactions.
- According to the shape of the kinetic equation:
- Elemental (concentrations of the reactants with exponents equal to the stoichiometric coefficients).
- No elementary (concentrations of the reactants with exponents different from the stoichiometric coefficients).
-
Depending on the number of phases:
w
Homogeneous (single phase).
w Not homogeneous (more than one phase).
-
depending on their complexity:
w
Simple (single stoichiometric equation, A + B ------> R).
w Multiple (or complex, not just a single stoichiometric equation). Can be in:
- Series (A ------> ------> R S).
- Parallel (A ------> R; The ------> S).
- Series-Parallel (A + B ------> R, R & B ------> S).
-
Regarding the balance:
- Irreversible (full conversion).
- Reversible (equilibrium is reached before it reaches 100% conversion).
| not catalyzed | Catalyzed | |
| Homogeneous | Most of the gas-phase reactions | Most liquid-phase reactions |
| Heterogeneous | Combustion | carbon synthesis of ammonia|
| Oxidation of ammonia to nitric acid to | ||
| solid attack by acids | Cracking oil | |
| gas-liquid absorption with reaction | Oxidation of SO 2 to SO 3 |
According to its temperature
6 .- Write 5 examples of each class of chemical reactions with their respective equations and names.
endothermic reactions to occur for these reactions have to provide energy. For example, to separate the components of water is necessary power input: A reaction which absorbs energy.
exothermic reactions are those in which it is released or energy is released, usually in the form of heat (energy)
If you put nails in a glass with muriatic acid (hydrochloric acid), touching the glass will feel a bit hot due to the exothermic reaction that occurs .
For your studies, you know that chemical reactions can be represented by equations. The reaction between the iron nails and hydrochloric acid is represented as follows:
http://www.huascaran.edu.pe/estudiantes/acurriculares/cta-reacciones-quimicas.htm
for equilibrium reactions:
When the reaction reaches chemical equilibrium then the speed of the two reactions is the same:
The equilibrium constant is defined as the reaction rate constant of production between the reversal rate constant:
reactions can occur in a single step (elementary reactions):
Example:
http://docentes.uacj.mx/lcamacho/cinetica.htm
http://www.sc.ehu.es/iawfemaf/archivos/materia/00311.htm
CHEMICAL EQUATION
chemical equation in the relative numbers of molecules of reactants and products are indicated by the coefficients of the formulas that represent these molecules .
| HCl | + reagents | NaOH → NaCl | + products | H 2 O |
characteristics of the equation:
1. Indicates the physical state of the reactants and products ( (l) liquid (s) solid (g) gaseous (c) aqueous (solution))
2. Indicate the catalysts substances that speed up or slow down the reaction and are not consumed are above or below the arrow that separates reactants and products.
EXAMPLE:
| 6CO 2 | + | 6H 2 O | → l solar uz | C 6 H O 12 6 | + | 6O 2 |
3. Indicate the release or absorption of energy
4. The equation should be balanced, ie the number of atoms that enter must be the same as those emerging
EXAMPLE:
| 2H (g) | + | O 2 (g) | → | 2H 2 O (l) | + | 136 kcal |
5. If a delta on the arrow indicates
work heat is supplied to the reaction EXAMPLE:
| KClO 3 | | KCl | + | O 2 |
http://www.fortunecity.com/campus/dawson/196/energrea.htm
Http://www.huascaran.edu.pe/estudiantes/acurriculares/cta-reacciones-quimicas.htm
http://web.educastur.princast.es/proyectos/biogeo_ov/2ESO/05_quimica / index.htm
http://www.ilustrados.com/publicaciones/EplVFukuZyDhBkhsiu.php
http://html.rincondelvago.com/reacciones-quimicas_8.html
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