introductionto chemicalreactions...by a chemical equation. ! the basic formula for a chemical...
TRANSCRIPT
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INTRODUCTION TO CHEMICAL REACTIONS
Balancing Chemical Equations
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Introduction to Chemical Reactions
§ A chemical reaction takes place when two or more chemicals mix and a new compound is formed.
§ Burning a piece of wood shows us an example of this.
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Introduction to Chemical Reactions
Wood that is burned turns into ash, soot, water vapor, and carbon dioxide
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Introduction to Chemical Reactions
§ A scientist by the name of Antoine Lavoisier discovered that matter cannot be created, nor can it be destroyed.
§ He named this the law of conservation of mass.
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Introduction to Chemical Reactions
§ Basically what this means is that the amount of material remaining after a reaction takes place must equal the amount that was present before the reaction.
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Introduction to Chemical Reactions
Starting material
Ending material
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Introduction to Chemical Reactions
§ This law is not easily observed in our everyday lives.
§ For example – a log that has burned seems to have “lost” mass (the leftover ash is a lot smaller than the original log).
§ This is because much of the material escaped into the air.
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Introduction to Chemical Reactions
§ If all the smoke, ash, and water vapor could be collected; what we would find is that it would equal the original weight of the unburned log.
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Writing Chemical Equations
§ In chemistry a reaction is represented by a chemical equation.
§ The basic formula for a chemical equation is made of two parts.
§ The REACTANT is the starting material. § The PRODUCT is the ending material. § An ARROW between the two represents
the reaction taking place.
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Writing Chemical Equations
Reactant Product
The arrow stands for “yields” or “produces”
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Writing Chemical Equations
§ Here is an example of a chemical reaction:
H2 + O2 H2 O
§ However…what do you notice if you count up the number of atoms on each side of the arrow?
An oxygen atom seems to have been destroyed!
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Writing Chemical Equations
§ In the real situation, no atoms were lost. The equation was just written incorrectly.
§ There are three rules to writing chemical equations in order to make sure all the atoms are balanced correctly.
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Balancing Chemical Equations
§ Rule 1 – the subscripts of molecules cannot be changed (otherwise you make a completely new molecule)
§ Example: CO2 and CO are both made of carbon and oxygen, but one is a relatively harmless byproduct of your body and the other is a potentially lethal gas!
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Balancing Chemical Equations
§ Rule 2 – You can only add more atoms by putting coefficients in front of the entire molecule.
§ Example: In order to get four oxygen atoms out of CO2, you cannot write CO4.
§ Instead, you must write 2CO2.
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Balancing Chemical Equations
§ Writing 2CO2 means you have two carbon dioxide molecules:
CO2 + CO2 § A total of two carbon atoms and four
oxygen atoms.
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Balancing Chemical Equations
§ Rule 3 – Continue adding coefficients until all the atoms are balanced.
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Balancing Chemical Equations
§ Lets go back to our first equation:
H2 + O2 H2 O
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Balancing Chemical Equations
§ Try another one:
N2 + H2 NH3
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Practice Problems
H2 + Cl2 HCl
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Practice Problems
Zn + HCl ZnCl2 + H2
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Practice Problems
Na + OH Na2O + H2
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