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Writing and Balancing Equations Worksheet # 1

Write a balanced chemical equation for the following reactions:

  1. iron + sulfur  iron (II) sulfide
  1. zinc + cupric sulfate  zinc sulfate + copper
  1. silver nitrate + sodium bromide  Sodium nitrate + silver bromide
  1. potassium chlorate (heated)  potassium chloride + oxygen
  1. water (in presence of electricity)  hydrogen + oxygen
  1. mercury (II) oxide (heated)  mercury + oxygen
  1. potassium iodide + lead (II) nitrate  lead (II) iodide + potassium nitrate
  1. aluminum + oxygen  aluminum oxide
  1. magnesium chloride + ammonium nitrate  magnesium nitrate + ammonium chloride
  1. iron (III) chloride + ammonium hydroxide  iron (III) hydroxide + ammonium chloride
  1. iron (III)oxide + carbon  iron + carbon monoxide
  1. iron + water  hydrogen + iron (III)oxide
  1. iron (III) chloride + potassium hydroxide  potassium chloride + iron (III) hydroxide
  1. aluminum + sulfuric acid  aluminum sulfate + hydrogen

Writing and Balancing Equations Worksheet #2

I. Counting Atoms

_____1. How many total atoms are there in 5 formula units of calcium hydroxide?

_____2. How many total atoms are there in 3 formula units of tin (IV) carbonate?

_____3. How many atoms of oxygen are there in 4 formula units of copper(II) sulfite?

____4. How many atomsof hydrogen are there in 5 molecules of acetic acid?

____5. How many atoms of oxygen are there in 7 molecules of oxygen gas?

II. Balancing Equations-Write balanced equations for each of the following reactions

l. magnesium plus oxygen gas yields magnesium oxide

2. Iron plus oxygen gas yields iron (III) oxide

3. water plus dinitrogen trioxide yields HNO2

4. sodium oxide plus water yields sodium hydroxide.

5. iron plus water yields (in the presence of heat) Fe3O4 plus hydrogen gas.

6. potassium chlorate yields (in the presence of heat) potassium chloride plus oxygen gas.

7. aluminum plus lead (II) nitrate yields aluminum nitrate plus lead.

8. copper plus silver nitrite yields copper (II) nitrite plus silver

9. calcium hydroxide plus hydrochloric acid yields calcium chloride and water.

10. potassium hydroxide plus phosphoric acid yields potassium phosphate and water.

11. sodium sulfite plus hydrochloric acid yields sodium chloride and water and sulfur dioxide.

12. ammonium sulfate plus potassium hydroxide yields potassium sulfate plus NH3 plus water.

Predicting Products and Balancing Equations Worksheet #1

Identify the reaction type to the left of the problem number (synthesis, decomposition, and combustion). If the reaction occurs, predict the products and write a balanced equation. If there would be no reaction, write NO REACTION.

______1. nitrogen gas combines with calcium metal

______2. propane is combusted completely

______3. potassium bromide is synthesized from its constituent elements

______4. iron and fluorine react

______5. copper (I) carbonate decomposes

______6. calcium oxide is heated

______7. ethane is combusted completely

______8. strontium hydroxide decomposes

______9. lead (IV) oxide is heated

______10. lithium oxide is heated

______11. sodium chlorate decomposes

______12. barium nitride decomposes

______13. Sodium chloride is separated by electrolysis

______14. Dihydrogen monoxide separates by electrolysis

______15. copper and oxygen react

______16. complete combustion of decane

______17. oxygen gas combines with sodium

______18. heptadecane is combusted completely

______19. aluminum and chlorine react

______20. iron (II) carbonate decomposes

______21. sodium oxide is heated

______22. methane is combusted completely

______23. aluminum hydroxide decomposes

______24. lead (II) oxide is heated

______25. magnesium chlorate decomposes

______26. Carbon tetrahydride decomposes

______27. Propane decomposes

Predicting and Balancing Equations Worksheet #2

Determine if the following chemicals react when they come into contact with each other. Identify the reaction type to the left of the problem number (single replacement or double replacement). If the reaction occurs predict the products and write a balanced equation using symbols (g), (aq), (l), (s) when appropriate. If there would be no reaction, write NO REACTION.

For the following assume all compounds are aqueous (dissolved in water).

______1. silver bromide and iodine crystals

______2. sodium phosphate and pure iron metal

______3. zinc nitrate and strontium fluoride

______4. calcium nitrate and sodium sulfate

______5. solid calcium and aluminum chloride

______6. copper (II) chloride and aluminum hydroxide

______7. lead (II) nitrate and sodium iodide

______8. nickel (II) carbonate and solid lithium

______9. ammonium chlorate and magnesium hydroxide

______10. lead (II) bisulfate and solid aluminum

______11. solid potassium and hydrochloric acid

______12. zinc metal and phosphoric acid

______13. magnesium fluorine and copper (I) chloride

______14. lithium metal and hydrochloric acid

______15. chlorine gas and barium fluoride

______16. sulfuric acid and aluminum metal

______17. solid sodium and lithium sulfite

______18. pure silver jewelry and hydrochloric acid

______19. aluminum iodide and potassium sulfide

Predict and balance the following double-replacement reactions using symbols (g), (aq), (l), and (s) when appropriate then write a net ionic equation for the reaction.

1. silver nitrate and potassium chromate

Balanced Equation:

Net Ionic Equation:

2. zinc acetate and cesium hydroxide

Balanced Equation:

Net Ionic Equation:

3. ammonium sulfide and lead (II) nitrate

Balanced Equation:

Net Ionic Equation:

4. iron (III) sulfate and barium iodide

Balanced Equation:

Net Ionic Equation:

More Practice - Predicting and Balancing Equations Worksheet

Balance the equations using symbols (g), (aq), (l), (s) when appropriate. Identify the reaction to the left of the number (synthesis, decomposition, combustion, single replacement, double replacement, or redox). If a reaction would not occur write NO REACTION. If the reaction is a redox reaction identify the elements that go through oxidation and reduction.

______1. aqueous silver bromide is reacted with chlorine gas

______2. aqueous sodium phosphate is brought in contact with solid iron

______3. aqueous zinc sulfide is poured into aqueous strontium fluoride

______4. aqueous silver nitrate and aqueous sodium phosphate are mixed

______5. solid calcium is added to aqueous copper (II) chloride

______6. aqueous copper (II) chloride is mixed with solid iodide

______7. solid magnesium chloride is heated

______8. aqueous lead (II) nitrite plus aqueous lithium iodide

______9. bromine gas plus solid copper

______10. aqueous nickel (II) carbonate plus solid magnesium

______11. complete combustion of ethane gas

______12. aqueous potassium chlorate is mixed with aqueous magnesium hydroxide

Predict and balance the following double-replacement reactions based on the solubility of the products. Use the abbreviations (aq) and (s) for the reactants and products. All reactants are aqueous. If the reaction does not occur write NO REACTION. If a reaction does occur, write a net ionic equation for the reaction.

  1. silver nitrate and potassium chromate
  1. ammonium chloride and cobalt (III) sulfate
  1. lithium hydroxide and sodium chromate
  1. rubidium phosphate and calcium hydroxide
  1. iron (III) sulfate and barium iodide

Properties and Changes in Matter and Chemical Reactions Test Review

Review notes and all worksheets! Make sure you know the polyatomic ions (formulas, names, and charges)!

Physical and Chemical Changes and Properties:

1. Define and give examples of a physical property, chemical property, physical change, and chemical change.

2. What are four indicators of a chemical change?

3. Define solid, liquid, gas, and plasma.

Counting Atoms:

_____4. How many total elements are in 4 molecules of sulfur trioxide? How many total atoms in those 4 molecules of sulfur trioxide?______

_____5. How many atoms are in 8 molecules of nitrogen?

_____6. How many hydrogen atoms are present in 4 molecules of phosphoric acid?

Equations: You must be able to recognize the type of reaction in order to predict the products and balance the equations.

Determine the type of reaction to the left of the problem, write and balance the following equations. Use symbols when appropriate.

7. ______C2H5OH reacts with oxygen to produce carbon dioxide gas and water vapor.

8. ______Solid sodium oxide and water produce sodium hydroxide

9. ______Solutions of plumbic chloride and sodium chromate react to produce solid plumbic chromate and a solution of sodium chloride.

10. ______Hydrogen and flourine gases react to form gaseous hydrogen fluoride.

  1. ______Aluminum sulfate solution is added to a solution of calcium hydroxide to produce two insoluble products: aluminum hydroxide and calcium sulfate.

12. ______solid magnesium chlorate decomposes

13. ______iron (III) carbonate decomposes with heat

  1. ______potassium hydroxide is heated and begins to decompose

15. ______lithium oxide is heated

16. ______radium oxide is heated

17. ______complete combustion of liquid octane, C8H18

18. ______chlorine gas is bubbled through a solution of sodium bromide

19. ______pure barium is added to a solution of silver acetate.

20. ______copper powder reacts with oxygen when heated

21. ______solid iron reacts with oxygen gas

  1. ______aluminum acetate is added to a solution of strontium hydroxide
  1. ______silver metal comes into contact with a potassium sulfide solution
  1. ______chlorine gas is exposed to barium fluoride
  1. ______zinc is placed into a solution of sodium carbonate
  1. ______solutions of sodium sulfate and potassium phosphate are mixed together
  1. ______solutions of ammonium carbonate and sodium sulfide are mixed together

Net Ionic Reactions: Write the equation and net ionic equations for the following reactions. (Use your solubility rules.)

28. ammonium sulfide solution is poured in an aqueous cadmium nitrate solution.

29. solutions of zinc nitrate and calcium sulfide are mixed.

Redox Reactions Practice Problems (Remember that oxidation is losing electrons and reduction is gaining electrons.)

30. Assign, using page 591, oxidation states to the following:a. Lib. Fe3+c.HCl

d. SO2e. HBrf. CaSO4g. KNO3h. NO2-i. SO32-

31. Determine if the following are oxidation half reactions or reduction half reactions.

a. Ag  Ag1+ + 1e-

b. Al3+ + 3e-  Al

32. Determine if the following equations are redox reactors or not. Write and label the oxidation half reaction and the reduction half reaction for the redox reactions:

a. H2 + Br2  2HBr

b. CuO + Mg  MgO + Cu

c. 2CuO  O2 + 2Cu

d. 8H2 + S8  8H2S

e. SrBr2 + 2NaI  2NaBr + SrI2

Redox Reactions Worksheet

1. Calculate the oxidation state of each element in each of the following:

a. P2O5b. ZnSc. CuSO3d. PO43-e. (NH4)2SO4f. Ag3PO3

g. HgCl2h. MnCO3i. I2O7j. Fe(MnO4)3

2. Label each of the following half-reactions as either an oxidation or a reduction half-reaction:

a. Br2 + 2e- → 2Br-

b.. Ag → Ag1+ + 1e-

c. Fe3+ + 1e- → Fe2+

3. Determine which of the following are redox reactions. For each redox reaction write the oxidation– reduction half-reaction and identify the oxidizing and reducing agent.

a. 2KNO3 → 2KNO2 + O2

b. H2 + CuO → Cu + H2O

c. NaOH + HCl → NaCl + H2O

d. I2 + H2SO3 + H2O → 2HI + H2SO4

e. 8Al + 3NaNO3 + 5NaOH + 2H2O → 8NaAlO2 + 3NH3

f. 18KI + 2K2CrO7 + 28HCl → 2CrCl3 + 22KCl + 14H2O + 9I2