Chemical Reactions Unit
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1 Name: Hour: Teacher: ROZEMA / Chemistry Chemical Reactions Unit 1 P a g e
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7 Chemistry Balancing Equations Balance the following equations by inserting the proper coefficients. For selected reactions, draw Before and After particle diagrams to show the particles involved in the reaction. Be sure to provide a key. 1. C + H2O CO + H2 2. MgO Mg + O2 3. Al + O2 Al2O3 4. Zn + H2SO4 ZnSO4 + H2 Hint: For #4 and #13, since the sulfate group, SO4, stays together, balance it as a whole and don t worry about individual S and O atoms. For #15, balance NH4 as a whole. 7 P a g e
8 5. Cl2 + KI KCl + I2 6. CuCl Cu + Cl2 7. Na + Cl2 NaCl 8. Al + HCl AlCl3 + H2 9. Fe2O3 Fe + O2 8 P a g e
9 10. P + O2 P2O5 11. Mg + HCl MgCl2 + H2 12. H2 + N2 NH3 13. BaCl2 + H2SO4 BaSO4 + HCl 14. CH4 + O2 CO2 + H2O 9 P a g e
10 15. ZnCl2 + (NH4)2S ZnS + NH4Cl Part II: Write the formulas of the reactants and products; then balance the equations. (See Clues and Hints below.) 1. Nitric oxide (NO) reacts with ozone (O3) to produce nitrogen dioxide (NO2) and oxygen gas. (Hints #2 & 4) 2. Iron burns in air to form a black solid, Fe3O4. (Hint #4) 3. Sodium metal reacts with chlorine gas (diatomic element) to form sodium chloride. (Hint #2) 4. Acetylene, C2H2, burns in air to form carbon dioxide and water. (Hint #4) 5. Hydrogen peroxide (H2O2) easily decomposes into water and oxygen gas. (Hint #2) 6. Hydrazine (N2H4) and hydrogen peroxide are used together as rocket fuel. The products are nitrogen gas and water. (Hints #2, 4) 10 P a g e
11 7. If potassium chlorate (KClO3) is strongly heated, it decomposes to yield oxygen gas and potassium chloride. (Hints #2, #6) 8. When sodium hydroxide (NaOH) is added to sulfuric acid (H2SO4), the products are water and sodium sulfate. (Sulfate ion is SO4 2, hint #6) 9. In the Haber process, hydrogen gas and nitrogen gas react to form ammonia, NH3. (Hint #2) CLUES and HINTS: 1. Products usually follow words like produces, yields, forms 2. Watch for our diatomic elements (H2, N2, O2, F2, Cl2, Br2, I2), which are often (but not always) gases 3. Include state subscripts behind each substance [ (s), (l), (g) ] when the state is given 4. Remember air is a mixture of (primarily) two gases, O2 and N2. Which is most likely to participate in a reaction? 5. Elemental metals exist as single, unbonded atoms. (Ex: formula for copper metal is Cu) 6. Watch for ionic vs molecular compounds. Use your periodic table to figure out the formulas for these. 11 P a g e
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14 Balancing Chemical Reactions- Worksheet 2 Balance the following equations by inserting the proper coefficients. 1. SO2 + O2 SO3 2. CH4 + O2 CO + H2O 3. P + Cl2 PCl3 4. CO + O2 CO2 5. CH4 + O2 CH3OH 6. Li + Br2 LiBr 7. Al2O3 Al + O2 8. Na + H2O NaOH + H2 14 P a g e
15 9. CO2 + H2O C6H12O6 + O2 10. H2SO4 + NaCl HCl + Na2SO4 Two reactions used to get rid of sulfur dioxide, a pollutant from burning coal: 11. H2 + SO2 H2S + H2O 12. CaCO3 + SO2 + O2 CaSO4 + CO2 13. AgNO3 + CaCl2 AgCl + Ca(NO3)2 14. HCl + Ba(OH)2 BaCl2 + H2O 15. H3PO4 + NaOH Na3PO4 + H2O 16. Pb(NO3)2 + KI PbI2 + KNO3 15 P a g e
16 17. CuO + NH3 N2 + Cu + H2O 18. C2H5OH + O2 CO2 + H2O 19. C2H6 + O2 CH3COOH + H2O 20. NO2 + H2O HNO3 + NO Write the formulas of the reactants and products - including the symbols for the state - (s), (l), (g), (aq) - then balance the equations. 1. When a solution of hydrogen chloride is added to solid sodium bicarbonate (NaHCO3), the products are carbon dioxide, water and aqueous sodium chloride. 2. Steam (gaseous water) reacts with carbon at high temperatures to produces carbon monoxide and hydrogen gases. 3. Limestone, CaCO3, decomposes when heated to produce lime, CaO, and gaseous carbon dioxide. 4. Ethyl alcohol (a liquid), C2H6O, burns in air (refer to last worksheet to see what the burning reaction is) to produce carbon dioxide and gaseous water. 16 P a g e
17 5. Solid titanium(iv) chloride reacts with water, forming solid titanium(iv) oxide and aqueous hydrogen chloride. 6. At high temperatures, the gases chlorine and water react to produce hydrogen chloride and oxygen gases. 7. Steel wool (nearly pure Fe) burns in air to form the solid iron oxide, Fe2O3. 8. During photosynthesis in plants, carbon dioxide and water are converted into glucose, C6H12O6, and oxygen gas. 9. Solutions of calcium hydroxide, Ca(OH)2 and nitric acid, HNO3, react to produce water and aqueous calcium nitrate, Ca(NO3)2. 17 P a g e
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