chapter five
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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. The Mole. Many things have names for a quantity or group. - PowerPoint PPT PresentationTRANSCRIPT
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
The Mole Many things
have names for a quantity or group.
In chemistry, a quantity of atoms, molecules, etc. is called a mole.
The Mole Why a “mole”?
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.
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 1particles 10 6.02or
particles 10 02.6anything of mole 1 23
23
Learning Check Ex) Convert 0.0242 moles of CH4 to
molecules.
Learning Check Ex) Convert 4.45 E+21 atoms of Zn
to moles.
Subscripts and Moles The subscripts in a formula can be
interpreted on either an atom or mole level.
Ex) C6H12O6
Learning Check Ex) How many moles of H atoms are
present in 0.0150 moles of NH3? How many H atoms?
Molar Mass A molar mass of
an element is the atomic mass expressed in grams.
The molar mass of carbon is 12.01g
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
Learning Check What is the molar mass of MgCl2?
a) 94.0gb) 59.8gc) 95.3gd) 119.6g
Learning Check What is the molar mass of Al(OH)3?
a) 78.0gb) 46.0gc) 132.0gd) 44.0g
Molar Mass Any molar mass can written as a
conversion factor. From earlier:
1 mole of CO2 = 44.0g
2
2
CO mole 1g 44.0or
g 0.44CO mole 1
Molar Mass This allows for the conversion
between grams and moles. Ex) 45.0g of BaCl2 = ? moles
Molar Mass Ex) 1.52 x 10-3 moles of phosphorous
tribromide = ? grams
Moles Combining both molar mass and
Avogadro’s number concepts.
Learning Check An 8.15 E+21 molecules of C2H6
would have a mass of:
Learning Check A 45.3g sample of lead(II) chloride
would contain how many formula units?
Learning Check A 6.50 x 10-5 g sample of C5H10O5 will
contain how many Hydrogen atoms?
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
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
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
Chemical Equations Shows the before and after for a
chemical reaction using chemical formulas.
Chemical Equations Symbols added
having various meanings.
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!
Chemical Equations __Al + __Cl2 __AlCl3 Reaction is NOT balanced! Note: can NOT alter any subscripts! Make a tally sheet.
Learning Check Balance the following:
__FeCl2 + __Al __AlCl3 + __Fe
__Al2(SO4)3 + KOH Al(OH)3 + K2SO4
Learning Check Balance the following:
__H3PO3 __H3PO4 + __PH3
__C3H8 + __O2 __CO2 + __H2O
Learning Check Balance the following:
__C4H8O + __O2 __CO2 + __H2O
Types of Reactions Combination Reaction
2Al(s) + 3Br2(l) 2AlBr3(s) CaO(s) + CO2(g) CaCO3(s)
Types of Reactions Decomposition Reaction
(NH4)2Cr2O7(s) Cr2O3(s) + 4H2O(g) + N2(g)
Types of Reactions Single Replacement Reactions
Mg(s) + CuCl2(s) MgCl2(s) + Cu(s)
Types of Reactions Double Replacement Reactions
Pb(NO3)2(aq) + K2CrO4(aq) PbCrO4(s) + 2KNO3(aq)
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.
Chemical Reactions A reaction can be interpreted in
many ways. Atoms and molecules Moles Masses
Chemical Reactions N2 + 3 H2 2 NH3
Molecular interpretation
Mole interpretation
Mass interpretation
Law of Conservation of Mass In any chemical reaction, matter
cannot be created nor destroyed. Masses of reactants = Masses of
products.
N2 H2 NH3
15 molecules
2.4 moles
0.014 moles
Stoichiometry The calculation of chemical
quantities in a reaction. Relates a mass of a reactant or
product to any other reactant or product.
StoichiometryMass of A
Moles of A Moles of B
Mass of B
Stoichiometry If 45.1g of N2 are used, then what
mass of H2 is required?
N g 1.45 2
Stoichiometry If 7.25g of H2 completely reacts,
what mass of NH3 is produced?
H g 25.7 2
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
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
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?
Activation Energy The activation
energy is the minimum amount of energy required to produce a reaction.
Exo- and Endothermic Reactions Reactions that release heat energy
are said to be ________________. Reactions that absorb heat energy
are said to be ________________.
Exo- and Endothermic Reactions
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
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)
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.
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.
2H2O2(aq) 2H2O(l) + O2(g)