6. 2 pb(n03)2 - 2 pbo +3£n02 + 02 -...
TRANSCRIPT
Balancing Equations Worksheet #1
1. C2H4+3_o2 - co2 + h2o
2. 2- AlBr + 3 Cl?. 2 MCh + 2 Br2
3. 3_Br2 + Pels 2- FeBr + 3 2
4. 2 BF3+ _H20 - B203 + 2 HF
5. p4Oin + )2 KOH K3P04 + (n H?Q
6. 2_ Pb(N03)2 - 2 PbO +3£n02 + 02
7. SnCl4 +_ Na - NaCl + Sn
8. C3Hg + j2o2 " 2 C02 +4 H2Q
9. Ca(OH)2 +2-HN03 - Ca(N03)2 +_ = H20
10. _Fe + 1H20 - Fe304 + _H2
11. HC1 + BaC03 -> BaCl2 + H20 + C02
12. PbC03 + 2hN03 Pb(N03)2 + H20 + C02
13. P4Oio +_&.H20 - h3PQ4
14. XeF2 + H20 2 Xe + 02 + HF
Name
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Per
Balancing Equations Worksheet #2
Pb(N03)2 + K2Cr04 PbCr04 +2 KN03
Mn02 + hC1 MnCl2 + H2Q + Cl2
K +
BaQ2 BaO + 02
3 ZnlONh + H3P04 Zn3(P04)2 +(t9 H?Q
Fe(N03)3 +3_LiOH Fe(OH)3 +3 LiNQ3
cs2 +3_ci2 CC14 + S2C12
CH4 + Br2 CH3Br + HBr baJ&n c
Ba(CN)2 + H2SO4 BaS04 HC
h20 3KOH + H2
.(NH4)2Cr207 -> Cr203 + 3 H9O + N2
3i_A\ + 3CuS04 - .A12(S04)3 Cu
F2 + 3 KC1 - KF + Cl2
3 BaCl?. + -H3PQ4 Ba3(P04)2 + 3 HC1
CdCl2 + H2S CdS HC114.
Name Per.
Answer Sheet: Equation Balancing Card Game
i* A Cg + H2O > 2- ai(oh)3 + C2H2
2. Be2C + _ H20 Be(OH)2 + CH4
3. NH3 + 02 > NO + ( ? H20 (challenge!)
4. 2 BN + 3 f2 - bf3 + n2
5. 2 Sn + 02 - SnO
6. H2 + Cl2 - z HC1
7. V2O5 + ? Ca CaO + 2 V
8. Fe304 + II, 3 Fe + ±H2O
9. C + S02 _ CO + CS2
10. 2 Na + _2 H20 2 NaOH + H2
11 • NH3 + 02 f 2- N2 I4 + 2- H20 (challenge!)
12. LiH + AICI3 LiAl Lt + LiCl
13. HBr03 + _2_ HBr > _5_ H20 + _3_ Br2 (challenge!)
14. N2 + _ _ H2 2 NH3
15. K2S04 + BaCl2 - KC1 + BaS04
16. CaC2 +2- 02- Ca + 2- C02
Formula Writing/Equation Writing Practice Worksheet
Name Per.
1. Classify the compound as Ionic, Molecular, Acid, or Base. Write the formula for the compound.
a. aluminum hydroxide
b. sodium oxide
c. hydrofluoric acid
d. potassium phosphate
e. copper (I) sulfate
f. phosphorus pentabromide
Classify
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/V\
Formula
Ai(ot-0 3
ti l I 3p04CU2 0 4
TBr?2. Equation writing: Convert all chemical names to formulas and write a balanced equation.
a. Solid barium reacts with oxygen gas to produce solid barium oxide.
B&Cs) + f?)? -
b. Solid iron (III) oxide decomposes to form metallic iron (solid) and oxygen gas.
T -2 3 C5 fees')F
c. Solid iron and aqueous copper (II) sulfate react to form solid copper and aqueous iron (III)sulfate.
f C i(5 F , 5
d. Aqueous copper (II) chloride and aqueous lead (IV) nitrate react to form aqueous copper (II)nitrate and solid lead (IV) chloride.
A + P O-JOs) Z Pfccl s)e. Metallic magnesium (solid) reacts with aqueous silver nitrate to form aqueous magnesium
nitrate and metallic (solid) silver.
(M5 cl +¦ _h f5)
f. Aqueous sulfuric acid reacts with aqueous potassium hydroxide to form aqueous potassiumsulfate and water.
+- - . -
g. Chlorine gas reacts with aqueous potassium bromide to form aqueous potassium chloride andliquid bromine.
Ci c* + ci+
Directions: Write an example of an actual chemical reaction fitting each of the following types of reactions.
1. Synthesis: Example lit + .302 z± &iQ3
2. Decomposition: Example 2H2O2 2 l- O ± 0z
3. Single Replacement:
Example Li K l /jCl + K(Metal)
Example _
(Halogen)
lKCl + fz ~ KF -l-Cli
m
4. Double Replacement: Example I ojC I t M<j|(0H)2 -» MgCI? +-2N«0H
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Name Class Date
Types of Chemical Reactions
Write the type chemical reaction on the line synthesis (combination), decomposition, combustion, singlereplacement, or double replacement. Then, balance the equations using the lowest possible integers. For
questions 21 and 22, predict the products before balancing.
D DRCD6 D5DR
DK.
CD
C
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9.
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.11.
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. 14.
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. 16.
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.20.
.21.
22.
Zn +
2. Na +
HC1 +
2. h202
h2so4 ->
_ Br2 »¦ NaBr
_NaOH -
2 H20 +
ZnS04 +
NaCl +
H2
H20
02
Cu + 2 AgN03 Ag + _ Cu(N03)2
C2H5OH + _J_o2 co, + > Hbo
2 KOH -
Mg + 2 H2O
k7o + h2o
Mg(OH)2 + H,
2 AlCB
H2 +
KI +
2 ai + 5 cb
o2 2 h7o
.Pb(N03)2 Pbl2 2 kno3
4 p + _5_o2
Ca(C103)2
Fe203 5 C
H Fe + 3 02
2 p Qi
. CaCl2 + 5 02
_CO + 2 Fe
2 Fe203
3 Ca + 2 A1C13 3 CaCl2 + Al
N? + 3 h2 nh3
Ba(N03)2 + Na2S04
c3h8 + _5_ o2 co2 + £_ h2o
HgO _ Hg + 02
_Na + Cl2 -> f\faCl
BaS04 + 2 NaNOj
ch4 + J o2coz WzO
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Name Per.
Practice Worksheet: Predicting ProductsPredict the products of the following equations and then balance them.
I. Synthesis
1. 2JH2 + __o2 z H 0
2. Fe+ 3_S f 2 (use Fe+3)
3. 2- A1+ 3 C12 z Cf?
4. 2> Pb +__o2 pbO (use Pb2+)
5. Mg + Br2 ->
II. Decomposition
6. AI2S3 /V( -f- 3 £
7. 2- CaO -A Z Ccv F 0
8. 2- LiF -> 2 L <
9. PbS2 Pl F 2 S
10. Z NaCl -A z
III. Single Replacement Make sure to check the activity series; if the reaction doesnot occur, write NR for no reaction.
11. _K + _CuC12 + C -
12. 2_Na + Pb(N03)2 -
13. Cl2 + KF -A (\o r -O t •
14. Mg + Li2C03 - i e v' -
15. Br2 + . Nal 2. X a
(continued)
IY, Double Replacement
16. MCb + NaOH ? MOlCA foCotf)?.
17. AgNOa + KC1 1<L I'J 0 i C I
18. Ba(N03)2 + Li2S04 S 0
The next 2 reactions are a special type of double replacement called neutralization. Thisoccurs when an acid and a base react to form a salt + water.
19. HC1 + KOH •<- (-1 0
20. H2SO4+ Ca(OH)2 - ( SOi/ f z-O
V. Combustion
21. CHU + 2- Q2 C'O + Z z-O
22. CiiH24 + r 02 || C0 +• i2 l4z.O
23. C12H22O11 + I 2- O2 12, 2- + fl Ht. O
24. C9H20 + .O2 -> 4- /a (-1-2 0
25. 2 C2H6+ ~7 O2 C& -x.
Name (VCM Period Date
Oxidation Number Practice
Based on the oxidation numbers known for the other element(s), determine the oxidation number of theunderlined element.
1. Na2S04 16. C02 _±1
2. CaO a 17. CaC03
3. K2C1O4 Up 18. KC!04 t
4. Qr203 +3 19. S03 tip5. KI03 f5 20. Cu20 +1
6. H20 + 1 21. KCIO3
7. S042' tip 22. Cl2 0
8. H3PO4 23. H2SO3 in
9. LiMn04 +7 24. A!3+ t3
10. Ag _Q_ 25. S02
11. K?Cr?07 ip 26. H2SO4 ip
12. HN03 27. M0O2 t
13. C!03' +5 28. N03'
14. S 2 -2 29. NaCI +115. CO tz 30. Fe203 t3
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REDOX PRACTICE
First, indicate the type of chemical reaction (synthesis, decomposition, single replacement, or doublereplacement). Then, label the oxidation numbers for each element in the reaction on both the reactants andproducts side. Last, identify which element has been oxidized and which has been reduced.
0 O .j. | ~ Z.
1. 2Ag + S - Ag2S Circle Type: S/D/SR/DRElement Ox.# Reactants side Ox.# Products side Lose/Gain e' Oxidized/Reduced
A3 0 -H 105+ O icliz-ed
0 1 g i ci fc v/ccot
0 +2-I +! -I 02. 2Na + FeCI2 - 2NaCl + Fe Circle Type: S/D/ DRElement Ox.# Reactants side Ox.# Products side Lose/Gain e" Oxidized/Reduced
l\lq 0 + 1 los+ oXidizd
Fe + 2 0 cjcord ( t vc
Cl -i 1
3.
f3 -I 0 O2AICI3 ±2AI + 3CI2 Circle Type: S/D/SR/DR
Element Ox.# Reactants side Ox.# Products side Lose/Gain e Oxidized/Reduced
Al + 3 0 gain .
Cl -1 0 |DS Ojxid i d
i3 -2. + 1 -1 +3-1 il -z4. Fe203 + 6HCI 2FeCI3 + 3H20 Circle Type: S/D/Sr/6r) o+ Element Ox.# Reactants side Ox.# Products side Lose/Gain e' Oxidized/Reduced
ft + 3 i50 2 ~ 2
+ 1 + 1 -
Cl -I -1
10
+ 2 -3Circle Type: s)d/SR/DR
Element Ox.# Reactants side Ox.# Products side Lose/Gain e' Oxidized/Reduced
M9 0 + 2 lost O idiz dN 0 -3 g iofc toWced
+l -I 0 +l -I 06. 2NaBr +CI2 - 2NaCI + Br2 Circle Type: S/D/ DRElement Ox.# Reactants side Ox.# Products side Lose/Gain e' Oxidized/Reduced
Nq + i T | -- -
-i 0 I0S Oxidize
Cl 0 -i gavneol tel we
+ 2-1 0 07. 2HgO ->2Hg + 02 Circle Type: S®SR/DRElement Ox.# Reactants side Ox.# Products side Lose/Gain e" Oxidized/Reduced
H5 a 0 gai e (Zcdwccl
0 ~ z 0 I0ST Oxidizeo
0+3-1+2-10 8. 3Ca + 2AICI3 3CaCI2 + 2AI Circle Type: SJD/SR/DRElement Ox.# Reactants side Ox.# Products side Lose/Gain e' Oxidized/Reduced
o 0 iz |0TT oxidiz dAl + 3 0 ted e Cl i 1 - __
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