# Balancing Chemical Equations Worksheet

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1 Balancing Chemical Equations Worksheet Student Instructions 1. Identify the reactants and products and write a word equation. 2. Write the correct chemical formula for each of the reactants and the products. 3. Check to see whether there are the same NUMBERS and TYPES of atoms on both sides of the equation. i.e. The Law of Conservation of Matter. 4. Balance each chemical equation by placing whole numbers in front of the chemical formula. eg. The burning of steel wool(iron) in air. Step 1. Iron + Oxygen Iron(II) oxide Step 2 & 3 Fe + O 2 FeO Step 4 2Fe + O 2 2FeO Chemical formula help Acids Acetic acid, CH 3 COOH, produces acetate salts, CH 3 COO - Hydrochloric acid, HCl, produces chloride salts, Cl - Nitric acid, HNO 3, produces nitrate salts, NO 3 - Sulfuric acid, H 2 SO 4, produces sulfate salts, SO 4 2- Alkalis (Bases) Ammonia NH 3 Potassium hydroxide, KOH Sodium hydroxide, NaOH Cations (positive ions) aluminum Al 3+, ammonium NH 4 +, barium Ba 2+, calcium Ca 2+, copper Cu 2+, iron(ii) Fe 2+, iron(iii) Fe 3+, lead Pb 2+, lithium Li +, magnesium Mg 2+, mercury Hg 2+, sodium Na +, potassium K +, silver Ag +, zinc Zn 2+ Anions (negative ions) bromide Br -, carbonate CO 3 2-, chloride Cl -, hydroxide OH -, nitrate NO 3 -, phosphate PO 4 3- and sulfate SO 4 2- Diatomic molecules: Bromine Br 2, chlorine Cl 2, hydrogen H 2, nitrogen N 2 and oxygen O 2 Valencies or Combining Powers of Elements Element Metal Lithium Li, potassium K, sodium Na Silver Ag Non-metal Hydrogen H Bromine Br, chlorine Cl Barium Ba, calcium Ca, magnesium Mg Copper Cu, iron(ii) Fe, mercury Hg, zinc Zn Lead Pb Oxygen O, sulfur S Aluminium Al Iron(III) Fe Nitrogen N May be used for educational purposes upon acknowledgement 1

2 Write balanced equations for the following reactions 1. Magnesium ribbon burns in air to produce a white powder. A synthesis reaction. 2. Aluminum reacts with oxygen to produce a compound. 3. Hydrochloric acid and magnesium react to produce hydrogen gas and a magnesium salt 4. Sulfuric acid and zinc react to produce hydrogen gas and a zinc salt. 5. The action of sulfuric acid on calcium carbonate produces water, a calcium salt and a gas that turns limewater milky. 6. The heating of mercury(ii) oxide, HgO, causes it to decompose into its elements. This is an example of a decomposition reaction. 7. The heating of copper carbonate produces carbon dioxide gas and copper oxide. 8. Copper oxide reacts with hydrochloric acid to produce a green solution of copper(ii) chloride and water. 9. A strip of copper metal when placed in a solution of silver nitrate produces metallic silver and a copper salt. 10. When a solution of silver nitrate comes into contact with a solution of sodium chloride a white precipitate of silver chloride and a solution of sodium nitrate are produced. 11. Potassium hydroxide can be used to neutralise a solution of hydrochloric acid. It produces a potassium salt and water. 12. Sodium hydroxide can be used to neutralise a solution of sulfuric acid. It produces a salt plus water. 13. Chlorine gas and potassium bromide react to produce potassium chloride and bromine. 14. Aluminum and bromine combine violently to produce a single compound. 15. Sodium reacts violently with water to produce a solution of sodium hydroxide and hydrogen gas. 16. Iron(III) oxide when heated in hydrogen produces iron and water. 17. Limewater (calcium hydroxide) reacts with carbon dioxide to produce water and a precipitate of calcium carbonate. 18. Limestone (calcium carbonate) when strongly heated decomposes into carbon dioxide and quicklime (calcium oxide). 19. Copper oxide and carbon when heated together produce the copper metal and carbon monoxide gas. 20. Hydrochloric acid and sodium sulfide produce hydrogen sulfide gas and a salt. May be used for educational purposes upon acknowledgement 2

3 21. Copper sulfate and sodium hydroxide when mixed together produce a precipitate of copper hydroxide and a solution of sodium sulfate. 22. Copper hydroxide when heated produces black copper oxide and steam(h 2 O). 23. Copper oxide when heated in the presence of hydrogen gas produces copper metal and water. 24. Sodium hydroxide reacts with a solution of ammonium chloride to produce ammonia gas, salt and water. 25. A mixture of sodium iodide and lead nitrate produces a solution of sodium nitrate and a precipitate. 26. The complete combustion of methane (CH 4 ) produces carbon dioxide and water. Note: In a combustion reaction a fuel reacts with oxygen. 27. The combustion of ethanol, (C 2 H 5 OH) produces carbon dioxide and water 28. The combustion of glucose, (C 6 H 12 O 6 ) produces carbon dioxide and water 29. Barium hydroxide reacts with sulfuric acid to produce a white precipitate and water 30. A solution of mercury(ii) nitrate reacts with a solution of potassium iodide to produce a bright orange mercury(ii) iodide precipitate and a solution of potassium nitrate. 31. In the process of fermentation, yeast breakdown glucose molecules (C 6 H 12 O 6 ) to produce ethanol(c 2 H 5 OH) and carbon dioxide gas. 32. In the process of photosynthesis, plants use carbon dioxide and water to make glucose(c 6 H 12 O 6 ) and oxygen. 33. A solution of silver nitrate reacts with a solution of potassium phosphate to produces a yellow precipitate of silver phosphate and a solution of potassium nitrate. 34. Sodium hydrogen carbonate, NaHCO 3 and acetic acid react to produce carbon dioxide, water and sodium acetate, CH 3 COONa 35. In the Haber process nitrogen and hydrogen combine to produce ammonia 36. In the Solvay process calcium carbonate and sodium chloride are used to produce calcium chloride and sodium carbonate via an indirect pathway. 37. Brown nitrogen dioxide gas(no 2 ) combines with water to produce a mixture of nitric acid and nitrous acid (HNO 2 ). 38. Sodium oxide dissolves in water to produce a strong alkali solution 39. Lithium hydroxide is used in space missions to remove carbon dioxide from the air. Lithium carbonate and water are produced. 40. Colourless nitrogen monoxide(no) combines with oxygen to produce brown nitrogen dioxide(no 2 ). May be used for educational purposes upon acknowledgement 3

4 Balancing Chemical Equations Answers 1. Magnesium + oxygen magnesium oxide 2Mg + O 2 2MgO 2. Aluminum + oxygen aluminium oxide 4Al + 3O 2 2Al 2 O 3 3. Hydrochloric acid + magnesium magnesium chloride + hydrogen 2HCl + Mg MgCl 2 + H 2 4. Sulfuric acid + zinc zinc sulfate + hydrogen H 2 SO 4 + Zn ZnSO 4 + H 2 5. Sulfuric acid + calcium calcium sulfate + water + carbon dioxide H 2 SO 4 + Ca CaSO 4 + H 2 O + CO 2 6. Mercury(II) oxide mercury + oxygen 2HgO Hg + O 2 7. Carbon carbonate copper oxide + carbon dioxide CuCO 3 CuO + CO 2 8. Copper oxide + hydrochloric acid copper(ii) chloride + water CuO + 2HCl CuCl 2 + H 2 O 9. Copper + silver nitrate copper(ii) nitrate + silver Cu + 2AgNO 3 Cu(NO 3 ) 2 + 2Ag 10. Silver nitrate + sodium chloride silver chloride + sodium nitrate AgNO 3 + NaCl AgCl(s) + NaNO 3 where (s) = solid or precipitate 11. Potassium hydroxide + hydrochloric acid potassium chloride + water KOH + HCl KCl + H 2 O 12. Sodium hydroxide + sulfuric acid sodium sulfate + water 2NaOH + H 2 SO 4 Na 2 SO 4 + 2H 2 O 13. Chlorine + potassium bromide potassium chloride + bromine Cl 2 + 2KBr 2KCl + Br Aluminum + bromine aluminum bromide 2Al + 3Br 2 2AlBr Sodium + water sodium hydroxide + hydrogen 2Na + 2H 2 O 2NaOH + H Iron(III) oxide + hydrogen iron + water Fe 2 O 3 + 3H 2 2Fe +3H 2 O 17. Calcium hydroxide + carbon dioxide water + calcium carbonate Ca(OH) 2 + CO 2 H 2 O + CaCO Calcium carbonate calcium oxide + carbon dioxide CaCO 3 CaO + CO Copper oxide + carbon copper + carbon monoxide CuO + C Cu + CO 20. Hydrochloric acid + sodium sulfide hydrogen sulfide + sodium chloride 2HCl + Na 2 S H 2 S + 2NaCl May be used for educational purposes upon acknowledgement 4

5 21. Copper sulfate + sodium hydroxide copper hydroxide + sodium sulfate CuSO 4 + 2NaOH Cu(OH) 2 (s) + Na 2 SO Calcium hydroxide copper oxide + water Cu(OH) 2 CuO + H 2 O 23. Copper oxide + hydrogen copper + water CuO + H 2 Cu + H 2 O 24. Sodium hydroxide + ammonium chloride sodium chloride + ammonia + water NaOH + NH 4 Cl NaCl + NH 3 + H 2 O 25. Sodium iodide + lead nitrate 2NaI + Pb(NO 3 ) 2 2NaNO 3 + PbI 2 (s) 26. Methane + oxygen carbon dioxide + water CH 4 + 2O 2 CO 2 + 2H 2 O 27. Ethanol + oxygen carbon dioxide + water C 2 H 5 OH + 3O 2 2CO 2 + 3H 2 O 28. Glucose + oxygen carbon dioxide + water C 6 H 12 O 6 + 6O 2 6CO 2 + 6H 2 O 29. Barium hydroxide + sulfuric acid barium sulfate + water Ba(OH) 2 + H 2 SO 4 BaSO 4 + H 2 O 30. Mercury(II) nitrate + potassium iodide mercury iodide + potassium nitrate Hg(NO 3 ) 2 + 2KI HgI 2 (s) + 2KNO Glucose ethanol + carbon dioxide C 6 H 12 O 6 2C 2 H 5 OH + 2CO Carbon dioxide + water glucose + oxygen 6CO 2 + 6H 2 O C 6 H 12 O 6 + 6O Silver nitrate + potassium phosphate silver phosphate + potassium nitrate 3AgNO 3 + K 3 PO 4 Ag 3 PO 4 + 3KNO Sodium hydrogen carbonate + acetic acid sodium acetate + carbon dioxide + water NaHCO 3 + CH 3 COOH CH 3 COONa + CO 2 + H 2 O 35. Nitrogen + hydrogen ammonia N 2 + 3H 2 2NH Calcium carbonate + sodium chloride sodium carbonate + calcium chloride CaCO 3 + 2NaCl Na 2 CO 3 + CaCl Nitrogen dioxide + water nitric acid + nitrous acid NO 2 + 2H 2 O HNO 3 + HNO Sodium oxide + water sodium hydroxide Na 2 O + H 2 O 2NaOH 39. Lithium hydroxide + carbon dioxide lithium carbonate + water 2LiOH + CO 2 Li 2 CO 3 + H 2 O 40. Nitrogen monoxide + oxygen nitrogen dioxide 2NO + O 2 2NO 2 May be used for educational purposes upon acknowledgement 5

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