chapter five chemical quantities and reactions the mole molar mass chemical changes chemical...
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Chapter Five Chemical Quantities and Reactions
The Mole Molar Mass Chemical Changes Chemical Equations Types of Reactions Mole Relationships in Chemical Equations Mass Calculations Energy in Chemical Reactions
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The Mole Many things
have names for a quantity or group.
In chemistry, a quantity of atoms, molecules, etc. is called a mole.
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The Mole
Why a “mole”?
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The Mole A mole of anything is 6.02 E+23 particles. This is sometimes referred to as
Avogadro’s Number. Written as a number:
602,000,000,000,000,000,000,000 A mole of marbles would easily fill the
entire Grand Canyon with much to spare.
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The Mole One mole of:
Carbon = 6.02 E+23 carbon atoms CO2 =6.02 E+23 CO2 molecules NaCl = 6.02 E+23 NaCl formula units 1 mole of anything = 6.02 E+23
particles
anything of mole 1
particles 10 6.02or
particles 10 02.6
anything of mole 1 23
23
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Learning Check
Ex) Convert 0.0242 moles of CH4 to molecules.
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Learning Check Ex) Convert 4.45 E+21 atoms of Zn
to moles.
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Subscripts and Moles The subscripts in a formula can be
interpreted on either an atom or mole level.
Ex) C6H12O6
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Learning Check Ex) How many moles of H atoms are
present in 0.0150 moles of NH3? How many H atoms?
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Molar Mass A molar mass of
an element is the atomic mass expressed in grams.
The molar mass of carbon is 12.01g
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Molar Mass The molar mass of any compound is
equal to the sum of all the atomic weights for each element in the formula.
Ex) The molar mass of CO2 is:1C + 2O = 1(12.0g) + 2(16.0g) = 44.0gThus, 1 mole of CO2 = 44.0g
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Learning Check
What is the molar mass of MgCl2?a) 94.0gb) 59.8gc) 95.3gd) 119.6g
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Learning Check
What is the molar mass of Al(OH)3?a) 78.0gb) 46.0gc) 132.0gd) 44.0g
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Molar Mass Any molar mass can written as a
conversion factor. From earlier:
1 mole of CO2 = 44.0g
2
2
CO mole 1
g 44.0or
g 0.44
CO mole 1
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Molar Mass This allows for the conversion
between grams and moles. Ex) 45.0g of BaCl2 = ? moles
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Molar Mass Ex) 1.52 x 10-3 moles of phosphorous
tribromide = ? grams
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Moles Combining both molar mass and
Avogadro’s number concepts.
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Learning Check
An 8.15 E+21 molecules of C2H6
would have a mass of:
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Learning Check A 45.3g sample of lead(II) chloride
would contain how many formula units?
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Learning Check
A 6.50 x 10-5 g sample of C5H10O5 will contain how many Hydrogen atoms?
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Physical Changes A physical change is one in which
the state, shape, or size of the substance is altered but not its identity. Ex) Ice melting Ex) Ripping a piece of paper Ex) Boiling ethanol Ex) Pulverizing a rock
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Chemical Changes A chemical change is one in which
matter is transformed into new kinds of matter by the rearrangement of atoms. Ex) Iron rusting Ex) Burning a log Ex) Fermenting grapes Ex) Antacid neutralizing stomach acid
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Learning Check Decide whether each is Physical or
Chemical change. a) Making Kool-aid b) Baking cookies c) Cutting an aspirin in half d) Bleaching a stained shirt
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Chemical Equations Shows the before and after for a
chemical reaction using chemical formulas.
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Chemical Equations Symbols added
having various meanings.
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Chemical Equations A Chemical Equation is always
written so that the total numbers of atoms on each side of the equation are equal.
To do this, coefficients are added in front of each substance.
Must use lowest whole number coefficients!
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Chemical Equations
__Al + __Cl2 __AlCl3
Reaction is NOT balanced! Note: can NOT alter any subscripts! Make a tally sheet.
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Learning Check Balance the following:
__FeCl2 + __Al __AlCl3 + __Fe
__Al2(SO4)3 + KOH Al(OH)3 + K2SO4
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Learning Check Balance the following:
__H3PO3 __H3PO4 + __PH3
__C3H8 + __O2 __CO2 + __H2O
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Learning Check Balance the following:
__C4H8O + __O2 __CO2 + __H2O
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Types of Reactions Combination Reaction
2Al(s) + 3Br2(l) 2AlBr3(s) CaO(s) + CO2(g) CaCO3(s)
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Types of Reactions Decomposition Reaction
(NH4)2Cr2O7(s) Cr2O3(s) + 4H2O(g) + N2(g)
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Types of Reactions
Single Replacement Reactions
Mg(s) + CuCl2(s) MgCl2(s) + Cu(s)
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Types of Reactions
Double Replacement Reactions
Pb(NO3)2(aq) + K2CrO4(aq) PbCrO4(s) + 2KNO3(aq)
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Combustion
A rapid reaction with oxygen from the air. CH4(g) + 2O2(g) CO2(g) + 2H2O(l)
Also occurs in the cells of animals when glucose, C6H12O6, is converted to energy.
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Chemical Reactions A reaction can be interpreted in
many ways. Atoms and molecules Moles Masses
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Chemical Reactions
N2 + 3 H2 2 NH3
Molecular interpretation
Mole interpretation
Mass interpretation
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Law of Conservation of Mass
In any chemical reaction, matter cannot be created nor destroyed.
Masses of reactants = Masses of products.
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N2 H2 NH3
15 molecules
2.4 moles
0.014 moles
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Stoichiometry The calculation of chemical
quantities in a reaction. Relates a mass of a reactant or
product to any other reactant or product.
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Stoichiometry
Mass of A
Moles of A Moles of B
Mass of B
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Stoichiometry
If 45.1g of N2 are used, then what mass of H2 is required?
N g 1.45 2
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Stoichiometry
If 7.25g of H2 completely reacts, what mass of NH3 is produced?
H g 25.7 2
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Stoichiometry For the reaction:
2C2H2 + 5O2 4CO2 + 2H2O
If 6.85g of C2H2 is completely combusted, then what mass of CO2 is produced? a. 13.7g b. 11.6g c. 23.2g d. 5.80g
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Stoichiometry For the reaction:
4Al + 3O2 2Al2O3
When 0.452g of Al completely reacts, what mass of Al2O3 is produced? a. 3.42g b. 0.853g c. 0.226g d. 23.1g
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Energy in Reactions
Collision Theory In the game of pool (billiards), in order
to sink a ball in the pocket what is needed?
In reactions, what is needed?
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Activation Energy The activation
energy is the minimum amount of energy required to produce a reaction.
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Exo- and Endothermic Reactions
Reactions that release heat energy are said to be ________________.
Reactions that absorb heat energy are said to be ________________.
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Exo- and Endothermic Reactions
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Exothermic Reactions
Energy level of the products is lower than that of the reactants.
Heat is a product and can be included in the balanced reaction.
Ex) C(s) + 2H2(g) CH4(g) + 18 kcal
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Endothermic Reactions
Energy level of the products is higher than that of the reactants.
Heat is a reactant.
Ex) N2(g) + O2 (g) + 43.3 kcal 2NO(g)
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Rate of a Reaction
Reactions can range from instantaneous (very fast) to very slow.
We can affect the rate of reaction by: Increasing the concentration of the
reactants.
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Rate of a Reaction Increasing the
temperature of the reactants. This increases the fraction of molecules that have enough energy to react.
Adding a catalyst. A catalyst lowers the activation energy.
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2H2O2(aq) 2H2O(l) + O2(g)