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Balancing Chemical Equations

Balancing Chemical Equations. Rules:. 1. LEARN THESE DIATOMIC MOLECULES : O 2 H 2 N 2 F 2 Cl 2 Br 2 I 2 2. The same number of atoms of each element appearing in reactants must appear in the products .

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Balancing Chemical Equations

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  1. Balancing Chemical Equations

  2. Rules: 1. LEARN THESE DIATOMIC MOLECULES: O2 H2 N2 F2 Cl2 Br2 I2 2. The same number of atoms of each element appearing in reactants must appear in the products. 3. The subscripts of a formula cannot be changed to balance the equation. Each compound must retain its stableness via oxidation states. 4. Choose compound with greatest number of atoms first. 5. Balance by placing necessary coefficients in front of entire molecules. NO SUBSCRIPT CHANGES!

  3. Rules cont. 6. Be certain each side of equation has same number of atoms of each type. 7. Make sure coefficients are in lowest whole number ratios. 8. Polyatomic ions usually stay intact, but multiple polyatomic ions may be separated. 9. (aq.) stands for aqueous which is Latin for water solution: (g) gas (l) liquid (s) solid (c) crystalline solid

  4. More Rules: •  means “yields” and shows direction of action • ∆ above arrow shows heat has been added •  shows reaction is reversible • MINOH: try Metals first, then Ions, then Nonmetals, and Oxygen, then Hydrogen last

  5. Sample Problem: C8H18 + O2 CO2 + H2O C8H18 + O2 __ CO2 + __ H2O C8H18 + __ O2 __ CO2 + __ H2O __ C8H18 + __ O2 __ CO2 + __ H2O

  6. Practice Problems: H2CrO4 + AgNO3 Ag2CrO4 + HNO3 (aq) (aq) (s) (aq) Chromic + Silver  Silver + Nitric Acid Nitrate Chromate Acid 1, 2, 1, 2 Double displacement

  7. Problem # 6 Cu(NO3)2 CuO + NO2 + O2 (aq) (s) (g) (g) Copper (II)  Copper (II) + Nitrogen + Oxygen Nitrate Oxide Dioxide Gas 2, 2, 4, 1 Decomposition

  8. Problem # 14 AlBr3 + Cl2 AlCl3 + Br2 (aq) (g) (aq) (g) Aluminum + Chlorine  Aluminum + Bromine Bromide Gas Chloride Gas 2, 3, 2, 3 Single Displacement

  9. Problem # 2 P4 + O2 + H2O  H3PO4 (s) (g) (aq) (aq) Phosphorus + Oxygen + Water  Phosphoric (free) gas acid 1, 5, 6, 4 Synthesis

  10. Problem # 20 sodium permanganate + sulfuric acid  sodium sulfate + manganese (VII) oxide + water NaMnO4 + H2SO4 Na2SO4 + Mn2O7 + H2O (aq) (aq) (aq) (s) (l) 2, 1, 1, 1, 1 Double Displacement

  11. Problem # 3 Th(NO3)4 + K3PO4 Th3(PO4)4 + KNO3 (aq) (aq) (s) (aq) Thorium + Potassium  Thorium + Potassium Nitrate Phosphate Phosphate Nitrate 3, 4, 1, 12 Double Displacement

  12. Problem # 22 sulfur trioxide + nitric acid  sulfuric acid + dinitrogen pentoxide SO3 + HNO3  H2SO4 + N2O5 (g) (aq) (aq) (g) 1, 2, 1, 1 Double Displacement

  13. Problem # 7 NH4NO3 + Ca(OH)2 Ca(NO3)2 + NH3 + H2O (aq) (aq) (aq) (g) (l) Ammonium + Calcium  Calcium + Ammonia + water Nitrate Hydroxide Nitrate 2, 1, 1, 2, 2 Double Displacement

  14. Missing Products sodium chloride + potassium iodide  NaCl + KI  ________ + _________ (aq) (aq) (?) (?) Does a reaction take place?

  15. Balancing Wars Problem # 1 CuSO4 + H3PO4 _____ + ______ (aq) (aq) • 3, 1, 2, 1 • 3, 1, 1, 3 • 2, 3, 3, 2 • 3, 2, 1, 3 • 2, 3, 3, 1 ((D)) Copper (II) + Phosphoric  Copper (II) + Sulfuric Sulfate Acid Phosphate Acid

  16. Balancing Wars Problem # 2 Mg(OH)2 + H3PO4 _____ + ______ (aq) (aq) • 1, 1, 1, 1 • 3, 2, 1, 3 • 2, 3, 1, 6 • 2, 3, 1, 1 • 3, 2, 1, 6 ((E.)) Magnesium + Phosphoric  Magnesium + Water Hydroxide Acid Phosphate

  17. Balancing Wars Problem # 3 CuCl2 + Na3PO4  _____ + ______ (aq) (aq) • 1, 2, 1, 2 • 2, 3, 1, 6 • 2, 3, 1, 1 • 3, 2, 1, 6 • 1, 1, 1, 1 ((D)) Copper (II) + Sodium  Copper (II) + Sodium Chloride Phosphate Phosphate Chloride

  18. Balancing Wars Problem 4 Potassium + Nickel (II)  _____ + ______ Permanganate Nitrate • 2, 1, 2, 1 • 2, 1, 3, 1 • 1, 2, 1, 2 • 1, 2, 1, 3 • 1, 1, 1, 1 ((A)) KMnO4 + Ni(NO3)2  KNO3 + Ni(MnO4)2

  19. Balancing Wars Bonus Problem KMnO4 + Na2C2O4 + H2SO4 K2SO4+ Na2SO4+ MnSO4+ CO2+ H2O Balance this equation and show your atom inventory and earn a grade pass.

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