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When we know the chemical equation for a reaction, we can determine
the amount of reactant needed or amount of product that can be produced
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the appearance of a substance is altered, but not its composition
physical change
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when the reacting substances change in to new substances that have different compositions and different properties
chemical change
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when the original substances change to new substances with different physical properties and different compositions
chemical reaction
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in a chemical reaction all of the atoms of the original substances are found in
the new substance or product
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tells us the materials we need and the products that will form in a chemical reaction
chemical equation
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in a equation, the formula of the reactants are written on the
left side of the arrow
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in a equation, the formula of the products are written on the
right side of the arrow
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if a substance is dissolved in water it is an
aqueous solution
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in any chemical reaction, the amount of matter
does not change
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a chemical reaction must be written as a
balanced equation
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whole numbers
coefficients
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whole numbers placed in front of the formula in an equation to balance the number of atoms or moles of atom of each element in an equation
coefficient
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when two or more elements or compounds bond to form one product
combination reaction
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when a single reactant splits in to two or more products
decomposition reaction
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when elements in compounds are replaced by other elements
replacement reactions
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when an uncombined element takes the place of an element in a compound
single replacement reaction
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when the positive ions in the reacting compounds switch places
double replacement reaction
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when fuel and oxygen are required and often the reaction produces carbon dioxide, water, and heat
combustion reaction
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combustion reactions can also occur in
the cells of the body in order to metabolize food
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there is no change in the total mass of the substances reacting in a chemical reaction, this is know as?
law of conservation of mass
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a conversion factor that relates the number of moles of two compounds in an equation derived from their coefficients
mole-mole factor
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the reactant that is completely used up in the reaction
limiting reactant
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the reactant that remains after the limiting reactant is use up
excess reactant
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the amount of product we could expect if all the reactants were converted to product according to the mole ratios of the equation
theoretical yield
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the amount of product we collect when the reaction end
actual yield
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why is the actual yield always lees the the theoretical yield?
because some product is always lost
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the ratio of the actual yield of a reaction to the theoretical yield possible for the reaction
percent yield
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Five types of reactions
- combination reaction
- decomposition
- single replacement
- double replacement
- combustion
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when 2 or more elements or compound form one product
combination reaction
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a single reactant splits into 2 or more products
docomposition
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an uncombined element takes the place of an element in a compound
single replacement
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the cations in the two reacting compounds switch places
double replacement
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fuel + oxygen products carbon dioxide, water, heat most of the time
combustion
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AB----->A+B
decomposistion
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2 H2O--->2 H2+O2
Decomposition
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A+B---->AB
combination reaction
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2 H2+O2----->2 H2O
combination reaction
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A+BC----->AC+B
single replacement
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AB+CD--->AD+CB
Double replacement
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solid turns to gas- no temperature change
sublimations
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gas turns to solid
deposition
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energy needed to vaporize 1g of liquid to gas
heat of vaporation
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hv=(mass) (heat of vaporation)
Heat of vaporation equation
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heat of vaporation=
2260 joules/grams
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the amount of heat absorbed or released during a reaction that takes place at a constant pressure
heat of reaction
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the energy of the products is greater than that of the reactants
endothermic
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the products have less energy that the reactants
exothermic
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