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Chapter 9 Balancing Equations
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Parts of a Reaction H 2 SO 3 (aq) H 2 O (l) + SO 2 (g) ReactantsProducts l = liquid g = gas aq = aqueous (water solution) Mixture NaCl (aq) s or cr = crystalline solid
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Arrows Ex. O 2 -- gas given off Ex. Ba(OH) 2 –-- precipitate formed (solid) in double displacement -- yields or forms -- reversible reaction (rxn)
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Types of Reactions Video
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Classifying Reactions Synthesis –Element + element compound A + X AX Ex. 2H 2 + O 2 2 H 2 O 4 Fe + 3 O 2 2 Fe 2 O 3
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Decomposition –Compound 2 or more simpler substances AX A + X Ex. 2 H 2 O 2 2 H 2 O + O 2 2 H 2 O 2H 2 + O 2
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Single Displacement ( or replacement) –Element + compound element + compound Nonmetal displaces nonmetal + - - CY + D CD + Y Metal displaces metal + - + AX + B BX + A Ex. Cu + 2 AgNO 3 Cu(NO 3 ) 2 +2Ag Ex. Cl 2 + 2 KBr 2 KCl + Br 2
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Double Displacement –compound+compound compound + compound –Normally in aqueous solution –Forms a precipitate + - + - AX + BY AY + BX Ex. CuCl 2 + 2 NaOH 2NaCl + Cu(OH) 2
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Combustion –Also called oxidation –This is a burning reaction w/ oxygen –Produces heat, light and CO 2 and H 2 O –Hydrocarbon + oxygen CO 2 + H 2 O –CH 4 + 2 O 2 CO 2 + 2 H 2 O
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Balancing Equations Video
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Balancing Equations Reaction equations give correct ratios between reactants and products Follows Law of Conservation of Mass (what was there b/4 must be there after)
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Steps in Balancing: 1.Determine the reactants and products 2.Assemble the parts of the chemical equation Write the formulas properly (w/ the proper oxidation numbers) and (diatomics) Diatomics: H 2, O 2, N 2, I 2, F 2, Br 2, Cl 2
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3. Balance the equation Use coefficients (# b/4 the symbol) to show equal # of atoms for each element on both sides of the equation Change only COEFFICIENTS NEVER, EVER touch the subscripts CaCO 3 subscript NEVER place coefficients in middle of formula Na3Cl You may need to use the least common multiple
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4. Check: count up each element and make sure the # atoms in each of the reactants equals the # of atoms in each of the products
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Water hydrogen + oxygen
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Lead (II) nitrate + sodium hydroxide lead (II) hydroxide + sodium nitrate
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Balancing combustion: Balance C (carbons) then H (hydrogens) then O (oxygens) If that doesn’t work and you get an odd number of O’s –Erase – double the hydrocarbon and do again (C, H, O)
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C 8 H 18 + O 2 CO 2 + H 2 O C 8 H 18 + O 2 8 CO 2 + 9 H 2 O 25 O’s 2 C 8 H 18 + 25O 2 16 CO 2 + 18H 2 O
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Precipitates Check every double displacement reaction for precipitates (check products) Use chart, anything other than a “s” on chart is a precipitate place a down arrow ( ) after that compound –AgCl
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