Chapter 7
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Transcript of Chapter 7
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Chemical Reactions
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A. Matter can change physically or chemically; a process that produces a chemical change is a chemical reaction
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B. A chemical equation is a shorthand form of what reactants are used and what products are formed in a chemical reaction
1. Some use words or chemical names to identify the products and reactants
Ex: Iron + Oxygen + Water Rust
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2. Chemical formulas can represent chemical names in an equation
Ex: Fe + H2O FeO2 + H2
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C. The mass of the reactants and products in a chemical reaction is always the same due to the Law of Conservation of Mass
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D. Chemical equations are balanced when the number of atoms is the same on each side of the equation
Ex: Fe + 2H2O FeO2 + 2H21 iron atom
1 iron atom
2 oxygen 2 oxygen
4 Hydrogen
4 Hydrogen
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1. In a chemical equation the reactants (substances going into reaction) are on the left and the products (substances being produced) are on the right
Ex: Fe + 2H2O FeO2 + 2H2
Reactants Products
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E. Energy is released or absorbed during a chemical reaction
1. Exothermic reactions – release energy
2. Endothermic reactions – absorb energy
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A.Different chemical reactions take different amounts of time
B.Activation Energy – the amount of energy needed to start a reaction
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C. The rate of reaction measures how quickly a reactant is disappearing and how quickly a product is appearing
1. Tells how quick a substance changes per unit time
2. Important in industry; the faster a product can be made the lower the cost
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3. Factors that change reaction rates:
a) Temperature – higher temp. faster particles are move and collide which makes reactions happen more quickly
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b) Concentration – amount of substance per volume
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c) Particle size/Surface area – more surface area the faster the rate due to more area to react
on
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D. Inhibitor – a substance that slows down the rate of a chemical reaction
E. Catalyst – a substance that speeds up the rate of reaction
ex: Enzymes – special proteins in the human body