Unit 7: Chemical Equations Chemistry. In a reaction: atoms are rearranged AND mass energy charge are...
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Unit 7: Chemical Equations Chemistry. In a reaction: atoms are rearranged AND mass energy charge are conserved Balancing Chemical Equations = law of conservation
In a reaction: atoms are rearranged AND mass energy charge are
conserved Balancing Chemical Equations = law of conservation of
mass same # of atoms of each type on each side of equation
Slide 3
CH 4 + 2 O 2 CO 2 + 2 H 2 O Reactants Products 1 C atom 1 C
atom 4 H atoms 4 H atoms 4 O atoms 4 O atoms
Slide 4
EX. solid iron reacts with oxygen gas to yield solid iron (III)
oxide If all coefficients are 1 If we change subscripts Fe 3+ O 2
___Fe(s) + ___O 2 (g) ___Fe 2 O 3 (s) + ___Fe(s) + ___O 2 (g)___Fe
2 O 3 (s) 1 1 1 ___Fe 2 (s) + ___O 3 (g)___Fe 2 O 3 (s) 1 1 1 + But
we cant!!!
Slide 5
Changing a ___________ changes the substance. To balance,
modify only _____________. Right now, _______________ dont enter
into our balancing picture. subscript coefficients superscripts
___Fe(s) + ___O 2 (g)___Fe 2 O 3 (s) + 23 Hint: Start with most
complicated substances first and leave simplest substances for
last. 4
Slide 6
2 solid sodium reacts w/oxygen to form solid sodium oxide ___O
2 (g) ___Na(s) ___Na 2 O(s) + Na + O 2 + 14 Aqueous aluminum
sulfate reacts w/aqueous calcium chloride to form a white
precipitate of calcium sulfate. The other compound remains in
solution. Al 3+ SO 4 2 Ca 2+ Cl _ Al 2 (SO 4 ) 3 (s) + _ CaCl 2 _
CaSO 4 _ AlCl 3 (aq) + 1332
Slide 7
1 1 Methane gas (CH 4 ) reacts with oxygen to form carbon
dioxide gas and water vapor. _ CH 4 (g) + _ O 2 (g) _ CO 2 (g) _ H
2 O(g) + 212 _ CaC 2 (s) + _ H 2 O(l) _ C 2 H 2 (g) + _ CaO(s) _
CaSi 2 + _ SbI 3 _ Si + _ Sb + _ CaI 2 _ Al + _ CH 3 OH _ Al(CH 3
O) 3 + _ H 2 111 32263 3 26 2 13 Furnaces burn primarily
methane.
Slide 8
2 _ C 2 H 2 (g) + _ O 2 (g) _ CO 2 (g) + _ H 2 O(l) ** 5 42 121
1 _ C 3 H 8 + _ O 2 _ CO 2 + _ H 2 O ** 534 1 _ C 5 H 12 + _ O 2 _
CO 2 + _ H 2 O ** 856 ** = complete combustion (+ O 2 ) of a
hydrocarbon (C x H y ) yields CO 2 and H 2 O Write equations for
the combustion of C 7 H 16 and C 8 H 18 1 _ C 7 H 16 + _ O 2 _ CO 2
+ _ H 2 O 1178 1 _ C 8 H 18 + _ O 2 _ CO 2 + _ H 2 O 2589 21618 Odd
# Oxy
Slide 9
Signs of Chemical Reactions There are five main signs that
indicate a chemical reaction has taken place: change in colorchange
in odorproduction of new gases or vapor input or release of energy
difficult to reverse release input
Slide 10
Evidence of a chemical reaction: A reaction has occurred if the
chemical and physical properties of the reactants and products
differ. heat light sound gas emitted color change odor For a
reaction to occur, particles of reactants must collide, and with
sufficient energy collision theory
Slide 11
activation energy: Chemical reactions release or absorb energy.
energy needed to start a reaction exothermic reactions endothermic
reactions The reaction in an oxy- acetylene torch is exothermic.
Photosynthesis is an endothermic reaction.
Slide 12
Endothermic Reaction Energy + Reactants Products Reaction
progress Energy Reactants Products Activation Energy
Slide 13
Exothermic Reaction Reactants Products + Energy 10 energy = 8
energy + 2 energy Reactants Products Energy Energy of reactants
Energy of products Reaction Progress
Slide 14
Decomposition of Nitrogen Triiodide 2 NI 3 (s) N 2 (g) + 3 I 2
(g) NI 3 I2I2 N2N2
Slide 15
Slide 16
catalyst: speeds up reaction w/o being consumed it lowers the
activation energy (E a ) AE timetime without catalystwith catalyst
Examples: enzymes catalyze biochemical reactions catalytic
converters convert CO into CO 2 Energy
Slide 17
Reaction Conditions and Terminology Certain symbols give more
info about a reaction (s) = solid (l) = liquid (g) = gas (aq) =
aqueous (dissolved in H 2 O) NaCl(s) NaCl(aq) More on aqueous
soluble or in solution indicates that a substance is dissolved in
water (usually) all acids are aqueous solutions
Slide 18
Other symbols means... Temp. at which we perform rxn. might be
given. The catalyst used might be given. means ______ is added to
the reaction MgCO 3 (s) MgO(s) + CO 2 (g) C 2 H 4 (g) + H 2 (g)C 2
H 6 (g) Pt C 6 H 5 Cl + NaOHC 6 H 5 OH + NaCl 400 o C yields or
produces heat (i.e., clues about the reaction)
Slide 19
Factors that influence the rate of a reaction To make reaction
rate increase concentration of reactants particle size temperature
mechanical mixing pressure catalystuse one nature of
reactantsN/A
Slide 20
Types of Chemical Reactions Synthesis (combination) reaction
Decomposition reaction A Single-replacement reaction B
Double-replacement reaction Combustion reaction (of a hydrocarbon)
A + B AB AB A + B A + BC AC + B AB + CD AD + CB C x H y + O 2 CO 2
+ H 2 O A use activity series to predict products/reactivity B use
solubility chart to predict products/reactivity
elementcompoundelementcompound All compounds
Slide 21
Classifying Reactions four types synthesis: simpler substances
combine to form more complex substances oxygen + rhombic sulfur
sulfur dioxide sodium + chlorine gas sodium chloride A + B AB AB +
C ABC A + B + C ABC __ O 2 __ S 8 + __ SO 2 __ Na __ Cl 2 + __ NaCl
818 212
Slide 22
decomposition: complex substances are broken down into simpler
ones lithium chlorate lithium chloride + oxygen water hydrogen gas
+ oxygen gas Li + ClO 3 Li + Cl _ LiClO 3 _ LiCl + _ O 2 2 2 3 _ H
2 O 2 _ H 2 + _ O 2 21 AB A + B ABC AB + C ABC A + B + C
Slide 23
single-replacement: one element replaces another AB + C A +
CBAB + C B + AC chlorine sodium bromide sodium chloride bromine ++
? aluminum copper (II) sulfate + _ Cl 2 Na + Br _ NaBr 1 _ Br 2 +
Na + Cl _ NaCl + 221 Cu 2+ SO 4 2 _ CuSO 4 _ Al + Al 3+ SO 4 2 _ Al
2 (SO 4 ) 3 1 _ Cu + 323 copper aluminum sulfate +
Slide 24
double-replacement: AD + CB AB + CD iron (III) chloride +
potassium hydroxide ? Fe 3+ Cl _ FeCl 3 + 1 K+K+ OH _ KOH Fe 3+ OH
K + Cl _ KCl_ Fe(OH) 3 + 313 iron (III) hydroxide + potassium
chloride lead (IV) nitrate + calcium oxide ? Pb 4+ O 2 _ Pb(NO 3 )
4 + 1 Ca 2+ NO 3 _ CaO_ Ca(NO 3 ) 2 _ PbO 2 + 212 Pb 4+ O 2 Ca 2+
NO 3 lead (IV) oxide + calcium nitrate
Slide 25
Balance and classify the following reactions: _ F 2 _ MgI 2 1 _
I 2 + _ MgF 2 + 111 Single replacement _ C 3 H 5 N 3 O 9 4 _ N 2 +
_ CO 2 6 12 + _ H 2 O 10 + _ O 2 1 Decomposition 1 _ C 5 H 12 + _ O
2 _ CO 2 + _ H 2 O 856 Double Replacement? Combustion
Slide 26
Word Equations Solid iron reacts with oxygen gas to yield solid
iron(III) oxide. word equation: balanced equation: iron Fe +oxygen
iron(III) oxide O 2 + Fe 3+ O 2 Fe 2 O 3 243
Slide 27
2 Solid sodium reacts w /oxygen to form solid sodium oxide. O 2
(g) Na(s) Na 2 O(s) + Na + O 2 + 4 Aqueous aluminum sulfate reacts
w /aqueous calcium chloride to form a white precipitate of calcium
sulfate. The other compound remains in solution. Al 3+ SO 4 2 Ca 2+
Cl Al 2 (SO 4 ) 3 (s) + CaCl 2 CaSO 4 AlCl 3 (aq) + 332 Write a
balanced equation ( w /rxn conditions) from the following word
equations.
Slide 28
Single and Double Replacement Reactions Double-replacement
reaction CaCO 3 + 2 HCl CaCl 2 + H 2 CO 3 General form: AB + CD AD
+ CB Single-replacement reaction Mg + CuSO 4 MgSO 4 + Cu General
form: A + BC AC + B
Slide 29
single-replacement: one element replaces another AB + C A +
CBAB + C B + AC chlorine sodium bromide sodium chloride bromine ++
? aluminum copper (II) sulfate + _ Cl 2 Na + Br _ NaBr 1 _ Br 2 +
Na + Cl _ NaCl + 221 Cu 2+ SO 4 2 _ CuSO 4 _ Al + Al 3+ SO 4 2 _ Al
2 (SO 4 ) 3 1 _ Cu + 323 copper aluminum sulfate +
Slide 30
Ca Activity Series Foiled again: Aluminum is knocked out by
Calcium Element Reactivity Li Rb K Ba Ca Na Mg Al Mn Zn Cr Fe Ni Sn
Pb H 2 Cu Hg Ag Pt Au Halogen Reactivity F 2 Cl 2 Br 2 I 2
Printable Version of Activity Series Printable Version of Activity
Series
Slide 31
Mg + AlCl 3 Al + MgCl 2 Predict if these reactions will occur
Al + MgCl 2 Can magnesium replace aluminum? Activity Series YES,
magnesium is more reactive than aluminum. 2233 Can aluminum replace
magnesium? NO, magnesium is less reactive than aluminum. Therefore,
no reaction will occur. NR (No Reaction) MgCl 2 + Al No reaction We
must determine if the lone element is more reactive than the bonded
one metals replace metals or non-metals replace nonmetals Order of
reactants DOES NOT determine how they react.
Slide 32
1 How do we know if a reaction will occur? For
single-replacement reactions, use Activity Series. In general,
elements above replace elements below. _ Ba + _ FeSO 4 _ Mg + _
Cr(ClO 3 ) 3 _ Pb + _ Al 2 O 3 _ NaBr + _ Cl 2 _ FeCl 3 + _ I 2 _
CoBr 2 + _ F 2 _ Fe + _ BaSO 4 _ Cr + _ Mg(ClO 3 ) 2 NR _ NaCl + _
Br 2 NR _ CoF 2 + _ Br 2 111 3223 21 11 21 11
Slide 33
double-replacement: AD + CB AB + CD iron (III) chloride +
potassium hydroxide ? Fe 3+ Cl _ FeCl 3 + 1 K+K+ OH _ KOH Fe 3+ OH
K + Cl _ KCl_ Fe(OH) 3 + 313 iron (III) hydroxide + potassium
chloride lead (IV) nitrate + calcium oxide ? Pb 4+ O 2 _ Pb(NO 3 )
4 + 1 Ca 2+ NO 3 _ CaO_ Ca(NO 3 ) 2 _ PbO 2 + 212 Pb 4+ O 2 Ca 2+
NO 3 lead (IV) oxide + calcium nitrate
Slide 34
Formation of a solid: AgCl AgNO 3 (aq) + KCl(aq) KNO 3 (aq) +
AgCl(s) Double Replacement Reactions
Slide 35
precipitate: a solid product that forms in an aqueous solution
reaction When ionic substances have (aq) written after them, the
individual ions have dissociated from the ionic crystal and are
floating around separately. Na 3 PO 4 (aq) means3 Na + (aq) + PO 4
3 (aq) Sodium phosphate, Na 3 PO 4, (sometimes called sodium
phosphate, tribasic) is a cleaning agent and food
preservative.
Slide 36
precipitate: a solid product that forms in an aqueous solution
reaction Na 2 CO 3 + Ca(NO 3 ) 2 CaCO 3 + (aq) (aq) Na + Ca 2+ CO 3
2 NO 3 2 (aq) (s) Na + NaNO 3 NO 3 ppt clear Na 2 CO 3 solution
clear Ca(NO 3 ) 2 solution cloudy solution containing CaCO 3 (s)
and NaNO 3 (aq) chunks sinkies floaties
Slide 37
FeCO 3 Na + Fe 2+ iron (II) chloride + sodium carbonate Cl 2
Using the SOLUBILITY TABLE: sodium chloride is soluble iron (II)
carbonate is insoluble CO 3 Fe 2+ Fe Na + Na 2 Cl - CO 3 2- Cl- CO
3 2- NaCl sodium chloride iron (II) carbonate + (aq) (s) 2 FeCl 2
Na 2 CO 3 NaCl FeCO 3 (aq) (s) ++ Predict if a reaction will occur
when you combine aqueous solutions of iron (II) chloride and sodium
carbonate If the reaction does occur, write a balanced chemical
equation showing it (be sure to include phase notation). (aq)
Balanced chemical equation
Slide 38
(?) For double-replacement reactions, reaction will occur if
any product is: water a gas a precipitate driving forces _ Pb(NO 3
) 2 (aq) + _ KI (aq) _ KOH (aq) + _ H 2 SO 4 (aq) _ FeCl 3 (aq) + _
Cu(NO 3 ) 2 (aq) H+H+ OH Fe 3+ Cl NO 3 Pb 2+ NO 3 K+K+ II Pb 2+ NO
3 K+K+ II Check new combinations to decide. (?) K+K+ SO 4 2 Cu 2+
H+H+ OH K+K+ SO 4 2 (?) Cl Cu 2+ (?) Fe 3+ NO 3 (?) (ppt)(aq)
(water) (aq) NR _ K 2 SO 4 (aq) + _ H 2 O (l) _ PbI 2 (s) + _ KNO 3
(aq) 1212 2112
Slide 39
Ions in Aqueous Solution Pb(NO 3 ) 2 (s) Pb(NO 3 ) 2 (aq) Pb 2+
(aq) + 2 NO 3 (aq) add water dissociation: Pb 2+ NO 3 Pb 2+ NO 3
splitting into ions NaI(s) NaI(aq) Na + (aq) + I (aq) Na + II II
add water ChemThink
Slide 40
Mix them and get the overall ionic equation __Pb 2+ (aq) + __NO
3 (aq) + __Na + (aq) + __I (aq) __PbI 2 (s) + __NO 3 (aq) + __Na +
(aq) yields reactants products Cancel spectator ions to get net
ionic equation __PbI 2 (s) 1 1222 221 Pb 2+ NO 3 Na + II NO 3 Na +
II __Pb 2+ (aq) + __I (aq) 12 Pb 2+ II II II II II II
Slide 41
Mix together Zn(NO 3 ) 2 (aq) and Ba(OH) 2 (aq): Zn(NO 3 ) 2
(aq) Ba(OH) 2 (aq) Zn 2+ (aq) + 2 NO 3 (aq)Ba 2+ (aq) + 2 OH (aq)
Ba 2+ OH Zn 2+ NO 3 clear Zn(NO 3 ) 2 solutionclear Ba(OH) 2
solution
Slide 42
Mix them and get the overall ionic equation __Zn 2+ (aq) + __NO
3 (aq) + __Ba 2+ (aq) + __OH (aq) __Zn(OH) 2 (s) + __NO 3 (aq) +
__Ba 2+ (aq) yields reactants products Cancel spectator ions to get
net ionic equation __Zn(OH) 2 (s) 1 1212 121 Zn 2+ NO 3 OH NO 3
__Zn 2+ (aq) + __OH (aq) 12 Zn 2+ OH Ba 2+ Zn 2+ OH Zn 2+ OH
Slide 43
Polymers and Monomers polymer: a large molecule (often a chain)
made of many smaller molecules called monomers Polymers can be made
more rigid if the chains are linked together by way of a
cross-linking agent.
Slide 44
MonomerPolymer amino acids nucleotides ( w /N- bases
A,G,C,T/U).. styrene PVA. proteins nucleic acids polystyrene slime
polyvinyl alcohol HNCCOH H H O R
Slide 45
Quantitative Relationships in Chemical Equations 4 Na(s) + O 2
(g) 2 Na 2 O(s) Particles4 atoms1 mcule2 mcules Moles4 mol1 mol2
mol Grams4 g1 g2 g ** Coefficients of a balanced equation represent
# of particles OR # of moles, but NOT # of grams.
Slide 46
Part. Vol. Mass MOL Mass Vol. Part. MOL SUBSTANCE A SUBSTANCE B
(known) (unknown) Use coeff. from bal. eq. to go from moles of A to
moles of B
Slide 47
Na 2 O 4 Na(s) + O 2 (g) 2 Na 2 O(s) How many moles oxygen will
react with 16.8 moles sodium? How many moles sodium oxide are
produced from 87.2 moles sodium? How many moles sodium are required
to produce 0.736 moles sodium oxide? () 4 mol Na 1 mol O 2 16.8 mol
Na = 4.20 mol O 2 87.2 mol Na = 43.6 mol Na 2 O () 2 mol Na 2 O 4
mol Na 0.736 mol Na 2 O = 1.47 mol Na () 2 mol Na 2 O 4 mol Na O2O2
NaNa 2 ONa