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Chemical Equations & Balancing. What is a chemical equation?. A standard way to describe a chemical reaction. This means that scientists worldwide use this system. Show the number and combinations of elements & compounds involved in the reaction. Chemical Equations …. - PowerPoint PPT Presentation
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Chemical Equations & Balancing
What is a chemical equation?
• A standard way to describe a chemical reaction.–This means that scientists worldwide
use this system.
• Show the number and combinations of elements & compounds involved in the reaction.
Chemical Equations …• 2 Parts to a chemical equation:
– Reactants = original substance(s) (substances before any reaction occurs)
– Products = created during the reaction (ending substances)
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NaHCO3 CH3COOHhttp://www.achilles-online.com/catalog/pics/
Sodium_Acetate__Anhydrous.jpg
NaCH3COO
http://keetsa.com/blog/wp-content/uploads/2008/03/water-
conservation.jpg
H2Ohttp://
www.scienceclarified.com/images/uesc_02_img0110.jpg
CO2
General Chemical Equations:
Reactant + Reactant Product + Product
• Not all reactions have 2 reactants and 2 products (could be one or more for each).
Reactantswritten before
the arrow.
Productswritten afterthe arrow.
Arrow representschemical reaction.
For example: Label the reactants and products in this equation.
• How do you say this?
Sodium and chlorine react to form sodium chloride.
2Na + Cl2 2NaCl
Reactants Product
In chemical reactions, the number and kinds of elements are always the same!
Chemical Equations also show Conservation of Mass:
• There must be the same amount of each element in the reactants as in the products (although the element could be part of different compounds). http://media.photobucket.com/image/balance%20scales/
nbest221/scales.jpg
Coefficients:
• Used to show conservation of mass in a chemical equation.
• Whole number put in front of a reactant or product to show a balanced chemical equation.
2Na + Cl2 2NaCl
• Multiplies the element(s) found in that specific reactant or product.
Balancing Chemical Equations:
• Write each reactant and product. (Remember how ions form chemical bonds.)
• Add coefficients to change the number of atoms within a substance.
• Never change the subscripts!
2 H2O2 2 H2O + O2a. Reactants?
b. H in reactants?
c. H in products?
d. O in reactants?
e. O in products?
f. Mass conserved? Why?
g. Without coefficients – conservation?
H
O
4 =
4 =
H = 2 X 2 = 4
H = 2 X 2 = 4
= 4
= 4
O = 2 X 2 = 4
O = 2 + 2 = 4
YES!
WhenReactants = Products
then massis conserved!
H2O2 H2O + O2
= 2
= 3
2 =
2 =
Does NOT showConservation ofMass because
Reactants do NOTequal Products.