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

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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

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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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