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REACTION PREDICTION Pre-AP CHEMISTRY
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Reactants Products The arrow means “yields” or “produces”
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(s) = solid (g)= gas (l)= liquid (aq)= aqueous (dissolved in water) = reversible reaction = catalyst (in this case, Pt is the catalyst) = heat is added = heat is added
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Practice “translating” a word equation: Solid zinc metal reacts with aqueous copper(II) sulfate to produce solid copper metal and aqueous zinc sulfate. Zn(s) + CuSO4(aq) Cu(s) + ZnSO4(aq)
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Balancing Equations *Balancing is a trial and error process and is best done in pencil!! *We balance an equation so that the reactants and products each have the same number of atoms of each element (conservation of mass). *We must correctly write the formulas for all reactants and products before we balance.
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Coefficients = Numbers placed in front of reactants and products 2H2 + O2 2H2O This means that 2 moles or molecules of hydrogen gas react with 1 mole or molecule of oxygen gas to produce 2 moles or molecules of water. The coefficients must be in the lowest ratio.
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Hints:. Balance elements one at a time
Hints: *Balance elements one at a time. *Balance polyatomic ions that appear on both sides of the equation as single units. (Ex. Count sulfate ions, not sulfur and oxygen separately) *Balance H and O last.
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Zn + HCl ZnCl2 + H2 Zn + 2HCl ZnCl2 + H2
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Al2(SO4)3 + Ca(OH)2 Al(OH)3 + CaSO4
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K + H2O KOH + H2 2K + 2H2O 2KOH + H2
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CH4 + O2 CO2 + H2O CH4 + 2O2 CO2 + 2H2O
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Fe + Cl2 FeCl3 2Fe + 3Cl2 2FeCl3
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C6H14 + O2 CO2 + H2O 2C6H O2 12CO H2O
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Al4C3 + H2O CH4 + Al(OH)3 Al4C H2O 3CH4 + 4Al(OH)3
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Balance the following chemical equations.
___ Ca + ____ H2O ____Ca(OH)2+____H2 Ca + 2 H2O Ca(OH)2 + H2 2. ____Cu2S + _____O2 ____Cu2O + ______SO2 2 Cu2S + 3 O2 2 Cu2O + 2SO2 3. _____MnO2 + _____HCl ______MnCl2 + ______H2O + _____Cl2 MnO2 + 4 HCl MnCl2 + 2H2O + Cl2 4. _____NH4NO3 + _____NaOH _____NH3 + _____H2O + _____NaNO3 NH4NO3 + NaOH NH3 + H2O + NaNO3
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3 Zn(OH)2 + 2 H3PO4 Zn3(PO4)2 + 6H2O 3 CO + Fe2O3 2 Fe + 3 CO2
5. ____Fe(OH)3 _____Fe2O3 + _____H2O 2Fe(OH)3 Fe2O3 + 3H2O 6. _____C3H6 + _____O2 _____CO2 + _____H2O 2C3H6 + 9O2 6CO2 + 6H2O 7. __Zn(OH)2 + __H3PO4 __Zn3(PO4)2 + ___H2O 3 Zn(OH)2 + 2 H3PO4 Zn3(PO4)2 + 6H2O 8. _____CO + _____Fe2O3 _____Fe + _____CO2 3 CO + Fe2O3 2 Fe + 3 CO2 _ NH4Cl + __Ca(OH)2 ___NH3 + ___H2O + __CaCl2 2NH4Cl + Ca(OH)2 2 NH3 + 2 H2O + CaCl2 ___HC2H3O2 + ___NaHCO3 __CO2 + __NaC2H3O2 + __H2O HC2H3O2 + NaHCO3 CO2 + NaC2H3O2 + H2O
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Write a balanced chemical equation for each of the following reactions
Write a balanced chemical equation for each of the following reactions. Include physical state symbols. 1. Copper metal heated with oxygen gives solid copper(II) oxide. 2Cu(s) + O2(g) 2CuO(s)
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2. Mixing ammonium nitrate and sodium hydroxide solutions gives aqueous sodium nitrate, ammonia gas, and water. NH4NO3(aq) + NaOH(aq) NaNO3(aq) + NH3(g) + H2O(l)
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3. Mercury(II) nitrate solution reacts with potassium iodide solution to give a mercury(II) iodide precipitate and potassium nitrate solution. Hg(NO3)2(aq) + 2KI(aq) HgI2(s) + 2KNO3(aq)
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4. Solutions of acetic acid and lithium hydroxide produce water and aqueous lithium acetate.
HC2H3O2(aq) + LiOH(aq) H2O(l) + LiC2H3O2(aq)
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5. Heating solid potassium chlorate in the presence of manganese dioxide catalyst produced potassium chloride and oxygen gas. 2KClO3(s) MnO2 2KCl(s) + 3O2(g)
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DECOMPOSITION REACTIONS -Reaction where a compound breaks down into two or more elements or compounds. Heat, electrolysis, or a catalyst is usually necessary.
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A compound may break down to produce two elements.
Ex. Molten sodium chloride is electrolyzed. 2NaCl 2Na + Cl2
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A compound may break down to produce an element and a compound.
Ex. A solution of hydrogen peroxide is decomposed catalytically. 2H2O2 2H2O + O2
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A compound may break down to produce two compounds.
Ex. Solid magnesium carbonate is heated MgCO3 MgO + CO2
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Metallic carbonates break down to yield metallic oxides and carbon dioxide.
K2CO3 K2O + CO2
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Metallic chlorates break down to yield metallic chlorides and oxygen.
2RbClO3 2RbCl + 3O2
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Metallic sulfites break down to yield metallic oxides and sulfur dioxide.
BaSO3 BaO + SO2
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Hydrogen peroxide decomposes into water and oxygen.
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Sulfurous acid decomposes into water and sulfur dioxide.
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Carbonic acid decomposes into water and carbon dioxide.
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Hydrated salts decompose into the salt and water
Sodium carbonate monohydrate is heated. Na2CO3.H2O Δ Na2CO3 + H2O
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Complete and balance the following reactions:
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1. ZnCO3 ZnCO3 ZnO + CO2
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2. KClO3 2KClO3 2KCl + 3O2
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3. HgO 2HgO 2Hg + O2
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4. H2CO3 H2CO3 H2O + CO2
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2NaCl electricity > 2Na + Cl2
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6. H2SO3 H2SO3 H2O + SO2
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7. CaCO3 CaCO3CaO + CO2
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2H2O electricity > 2H2 + O2
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9. Na2SO4.10H2O Na2SO4.10H2O Na2SO4 +10H2O
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10. H2O2 MnO2 > 2H2O2 MnO2 >2H2O + O2
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11. CuSO4.5H2O CuSO4.5H2O CuSO4 + 5H2O
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ADDITION REACTIONS -also called synthesis, combination or composition reactions -Two or more elements or compounds combine to form a single product.
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-A Group IA or IIA metal may combine with a nonmetal to make a salt.
Ex. A piece of lithium metal is dropped into a container of nitrogen gas. 6Li + N2 2Li3N
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-Two nonmetals may combine to form a molecular compound. C + O2 CO2
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-Two compounds combine to form a single product.
Sulfur dioxide gas is passed over solid calcium oxide SO2 + CaO CaSO3
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-A metallic oxide plus carbon dioxide yields a metallic carbonate
-A metallic oxide plus carbon dioxide yields a metallic carbonate. (Carbon keeps the same oxidation state) Li2O + CO2 Li2CO3
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-A metallic oxide plus sulfur dioxide yields a metallic sulfite
-A metallic oxide plus sulfur dioxide yields a metallic sulfite. (Sulfur keeps the same oxidation state) K2O + SO2 K2SO3
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-A metallic oxide plus water yields a metallic hydroxide
-A metallic oxide plus water yields a metallic hydroxide CaO + H2O Ca(OH)2
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-A nonmetallic oxide plus water yields an acid. CO2 + H2O H2CO3
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Complete and balance the following equations:
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1. Li + I2 2Li + I2 2LiI
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2. Mg + N2 3Mg + N2 Mg3N2
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3. SO3 + H2O SO3 + H2O H2SO4
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4. Sr + S Sr + S SrS
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5. Mg + O2 2Mg + O2 2MgO
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6. Ag + O2 4Ag + O2 2Ag2O
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7. Na2O + H2O Na2O + H2O 2NaOH
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8. SO2 + H2O SO2 + H2O H2SO3
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9. BaO + CO2 BaO + CO2 BaCO3
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10. CaO + SO2 CaO + SO2 CaSO3
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Double Replacement (metathesis)
Two compounds react to form two new compounds. All double replacement reactions must have a "driving force" that removes a pair of ions from solution. Ions keep their same charges as reactants and products.
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Formation of a precipitate: A precipitate is an insoluble substance formed by the reaction of two aqueous substances. Two ions bond together so strongly that water can not pull them apart.
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SOLUBILITY SONG Nitrates and Group One and Ammonium,
To the tune of “ My Favorite Things” from “The Sound of Music” Nitrates and Group One and Ammonium, These are all soluble, a rule of thumb. Then you have chlorides, they’re soluble fun, All except Silver, Lead, Mercury I. Then you have sulfates, except for these three: Barium, Calcium and Lead, you see. Worry not only few left to go still. We will do fine on this test. Yes, we will! Then you have the--- Insolubles Hydroxide, Sulfide and Carbonate and Phosphate, And all of these can be dried!
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Ex. Solutions of silver nitrate and lithium bromide are mixed.
AgNO3(aq) + LiBr(aq) AgBr(s) + LiNO3(aq)
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Formation of a gas: Gases may form directly in a double replacement reaction or can form from the decomposition of a product such as H2CO3 or H2SO3. (Don't leave carbonic or sulfurous acids, or ammonium hydroxide as products of double replacement reactions, decompose them!)
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2HCl(aq) + K2SO3(aq) 2KCl(aq) + H2O(l) + SO2(g)
Ex. Excess hydrochloric acid solution is added to a solution of potassium sulfite. 2HCl(aq) + K2SO3(aq) 2KCl(aq) + H2O(l) + SO2(g)
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NaOH(aq)+ NH4Cl(aq) NH3(g) + H2O(l) + NaCl(aq)
Ex. A solution of sodium hydroxide is added to a solution of ammonium chloride. NaOH(aq)+ NH4Cl(aq) NH3(g) + H2O(l) + NaCl(aq)
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Formation of a molecular substance: When a molecular substance such as water or acetic acid is formed, ions are removed from solution and the reaction "works".
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LiOH(aq) + HBr(aq) LiBr(aq) + H2O
Ex. Dilute solutions of lithium hydroxide and hydrobromic acid are mixed. LiOH(aq) + HBr(aq) LiBr(aq) + H2O
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Complete and balance the following equations:
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2NaOH + CuSO4 Na2SO4 + Cu(OH)2(s)
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NH4I + AgNO3 NH4NO3 + AgI(s)
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K2CO3 + Ba(OH)2 2KOH + BaCO3(s)
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4. KOH + HI KOH + HIKI + H2O(l)
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5. K2CO3 + HNO3 K2CO3 + 2HNO3 2KNO3 + H2O + CO2
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(NH4)2SO4 + BaCl2 2NH4Cl + BaSO4(s)
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Na2S + NiSO4 NiS(s) + Na2SO4
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Pb(NO3)2 + 2KBr PbBr2(s) + 2KNO3
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Fe2(SO4)3 + 3Ba(OH)2 2Fe(OH)3(s) + 3BaSO4(s)
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Hg2(NO3)2 + 2KI 2KNO3 + Hg2I2(s)
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Single Replacement Reaction where one element displaces another in a compound. One element is oxidized and another is reduced A + BC B + AC
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Active metals replace less active metals or hydrogen from their compounds in aqueous solution. Use an activity series to determine the activity of metal.
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Ex. Magnesium turnings are added to a solution of iron(III) chloride.
3Mg(s) + 2FeCl3(aq) 2Fe(s) + 3MgCl2(aq)
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Ex. Sodium is added to water.
2Na(s) + 2H2O(l) 2NaOH(aq) + H2(g) Reactions of Alkali metals
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Ex. Fe + H2O Fe + H2O no reaction
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Active nonmetals replace less active nonmetals from their compounds in aqueous solution. Each halogen will displace heavier halogens from their binary salts.
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Activity Series of Nonmetals Most Active F2 Cl2 Br2 Least Active I2
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Ex. Chlorine gas is bubbled into a solution of potassium iodide.
Cl2(g) + 2KI(aq) I2(s) + 2KCl(aq)
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Ex. I2 + KCl I2 + KCl no reaction
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Complete and balance the following equations:
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1. Zn + HCl Zn +2 HCl ZnCl2 + H2
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2. Br2 + NaCl Br2 + NaCl No Reaction
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3. F2 + NaBr F2 + 2NaBr 2NaF + Br2
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4. Al + CuSO4 2Al + 3CuSO4 Al2(SO4)3 + 3Cu
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5. Cu + AgNO3 Cu + 2AgNO3 Cu(NO3)2 + 2Ag
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6. Cd + CuSO4 Cd + CuSO4 CdSO4 + Cu
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7. K + H2O 2K + 2H2O 2KOH + H2
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8. Mg + H2SO4 Mg + H2SO4 MgSO4 + H2
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9. Ag + HCl Ag + HCl No Rxn
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10. I2 + KCl I2 + KCl No Rxn
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11. Ca + H2O Ca + 2H2O Ca(OH)2 + H2
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12. Zn + H2O Zn + H2O No Rxn
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COMBUSTION REACTIONS
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In the presence of excess oxygen, most hydrocarbons and alcohols can undergo complete combustion reactions to form carbon dioxide and water. The only tricky part is balancing the reaction. Balance the C first, H second, and O third.
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Ex. Ethane (C2H6) burns in air.
2C2H6 + 7O2 4CO2 + 6H2O
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Ethanol (C2H5OH) burns C2H5OH + 3O2 2CO2 + 3H2O
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Complete and balance the reactions for the combustion of the following compounds:
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1. CH4 CH4 + 2O2 CO2 + 2H2O
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2. C2H2 2C2H2 + 5 O2 4CO2 + 2H2O
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3. CH3OH 2CH3OH + 3O2 2CO2 + 4H2O
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4. C6H12O6 C6H12O6 + 6O2 6CO2 + 6H2O
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5. C8H18 2C8H O2 16CO2 + 18H2O
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6. C3H8 C3H8 + 5O2 3CO2 + 4H2O
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7. C6H6 2C6H6 + 15O2 12CO2 + 6H2O
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8. C2H4 C2H4 + 3O2 2CO2 + 2H2O
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9. C35H72 C35H O2 35CO2 +36 H2O
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10. C3H7OH 2C3H7OH + 9O2 6CO2 + 8H2O
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SYNTHESIS AND DECOMPOSITION REACTIONS
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Complete and balance the following equations:
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1. Sr + O2 2Sr + O2 2SrO
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2. Na + O2 4Na + O2 2Na2O
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3. K + Cl2 2K + Cl2 2KCl
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4. Ca + F2 Ca + F2 CaF2
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5. sodium + iodine 2Na + I2 2NaI
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6. magnesium + oxygen 2Mg + O2 2MgO
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7. hydrogen + chlorine H2 + Cl2 2HCl
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8. silver + sulfur 2Ag + S Ag2S
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9. calcium oxide + water CaO + H2O Ca(OH)2
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10. sulfur trioxide + water
SO3 + H2O H2SO4
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11. MgBr2 MgBr2 Mg + Br2
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12. AlCl3 2AlCl3 2Al + 3Cl2
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13. H2O 2H2O 2H2 + O2
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14. KI 2KI 2K + I2
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15. NaCl 2NaCl 2Na + Cl2
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16. nickel(II) chlorate Ni(ClO3)2 NiCl2 + 3O2
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SINGLE AND DOUBLE REPLACEMENT REACTIONS
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Write and balance the following reactions:
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Zn(s) + CuSO4(aq) ZnSO4(aq) + Cu(s)
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Cl2(g) + 2KI(aq) 2KCl(aq) + I2(s)
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Ni(s) + MgSO4(aq) No Reaction
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Br2(l) + CaCl2(aq) No Rxn
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5. zinc + copper(II) nitrate
Zn(s) + Cu(NO3)2(aq) Cu(s) + Zn(NO3)2(aq)
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6. calcium + hydrochloric acid
Ca(s) + 2HCl(aq) CaCl2(aq) + H2(g)
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7. copper(II) nitrate + silver
Cu(NO3)2(aq) + Ag(s) No Rxn
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8. sodium iodide + bromine
2NaI(aq) + Br2(l) 2NaBr(aq) + I2(s)
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2Na(s) + 2H2O(l) 2NaOH(aq) + H2(g)
9. sodium + water 2Na(s) + 2H2O(l) 2NaOH(aq) + H2(g)
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FeCl2(aq) + K2S(aq) FeS(s) + 2KCl(aq)
10. FeCl2 + K2S FeCl2(aq) + K2S(aq) FeS(s) + 2KCl(aq)
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ZnCl2(aq) + Pb(NO3)2(aq) Zn(NO3)2(aq) + PbCl2(s)
11. ZnCl2 + Pb(NO3)2 ZnCl2(aq) + Pb(NO3)2(aq) Zn(NO3)2(aq) + PbCl2(s)
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CaCl2(aq) + Na2CO3(aq) 2NaCl(aq) + CaCO3(s)
12. CaCl2 + Na2CO3 CaCl2(aq) + Na2CO3(aq) 2NaCl(aq) + CaCO3(s)
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(NH4)2SO4(aq) + BaCl2(aq) 2NH4Cl(aq) + BaSO4(s)
13. (NH4)2SO4 + BaCl2 (NH4)2SO4(aq) + BaCl2(aq) 2NH4Cl(aq) + BaSO4(s)
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14. sodium hydroxide + acetic acid
NaOH(aq) + HC2H3O2(aq) NaC2H3O2(aq) + H2O(l)
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15. copper(II) sulfate + ammonium sulfide
CuSO4(aq) + (NH4)2S(aq) CuS(s) + (NH4)2SO4(aq)
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MIXED EQUATION WORKSHEET #1 Complete the word equation, write the formula equation, balance it and identify the type of reaction. You many abbreviate as S, D, SR, DR, and C.
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1. Magnesium hydroxide + nitric acid
magnesium nitrate + water Mg(OH)2 + 2HNO3 Mg(NO3)2 + 2H2O DR
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2. Complete combustion of methane (CH4)
methane + oxygen carbon dioxide + water CH4 + 2O2 CO2 + 2H2O Combustion
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3. Chlorine + sodium bromide
bromine + sodium chloride Cl2 + 2NaBr Br2 + 2NaCl Single Replacement
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4. Aluminum + sulfuric acid
aluminum sulfate + hydrogen 2Al + 3H2SO4 Al2(SO4)3 + 3H2 Single replacement
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5. Sulfuric acid + sodium acetate
sodium sulfate + acetic acid H2SO4 + 2NaC2H3O2 Na2SO4 + 2HC2H3O2 Double replacement
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6. Heating calcium carbonate
calcium oxide + carbon dioxide CaCO3 CaO + CO2 Decomposition
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7. Heating mercuric oxide
mercury + oxygen 2HgO 2Hg + O2 Decomposition
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8. Zinc + silver nitrate Zinc + silver nitrate zinc nitrate + silver Zn + 2AgNO3 Zn(NO3)2 + 2Ag Single Replacement
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Sulfur + oxygen sulfur dioxide S + O2 SO2 synthesis
9. Burning sulfur Sulfur + oxygen sulfur dioxide S + O2 SO2 synthesis
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10. Heating sodium chlorate
sodium chloride + oxygen 2NaClO3 2NaCl + 3O2 Decomposition
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11. Zinc chloride + ammonium sulfide
zinc sulfide + ammonium chloride ZnCl2 + (NH4)2S ZnS + 2NH4Cl double replacement
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12. Aluminum hydroxide + hydrochloric acid
Aluminum hydroxide + hydrochloric acid aluminum chloride + water Al(OH)3 + 3HCl AlCl3 + 3H2O Double replacement
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13. Calcium + steam Calcium + steam calcium hydroxide + hydrogen Ca + 2H2O Ca(OH)2 + H2 Single replacement
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carbonic acid water + carbon dioxide H2CO3 H2O + CO2 Decomposition
14. Heating carbonic acid carbonic acid water + carbon dioxide H2CO3 H2O + CO2 Decomposition
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15. Electrolysis of sodium chloride
sodium + chlorine 2NaCl 2Na + Cl2 Decomposition
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16. Combustion of propane (C3H8)
Propane + oxygen Carbon dioxide + water C3H8 + 5O2 3CO2 +4 H2O Combustion
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17. Bromine + potassium iodide
Iodine + potassium bromide Br2 + 2KI I2 + 2KBr Single Replacement
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18. Magnesium + hydrochloric acid
magnesium chloride + hydrogen Mg + 2HCl MgCl2 + H2 Single replacement
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19. Sodium hydroxide + acetic acid
sodium acetate + water NaOH + HC2H3O2 NaC2H3O2 + H2O Double replacement
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20. Burning hydrogen hydrogen + oxygen water 2H2 + O2 2H2O Synthesis or combustion
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zinc sulfate + hydrogen Zn + H2SO4 ZnSO4 + H2 single replacement
21. Zinc + sulfuric acid Zinc + sulfuric acid zinc sulfate + hydrogen Zn + H2SO4 ZnSO4 + H2 single replacement
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22. Heating magnesium carbonate
magnesium oxide + carbon dioxide MgCO3 MgO + CO2 Decomposition
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Sodium + chlorine sodium chloride 2Na + Cl2 2NaCl Synthesis
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24. Lead(II) nitrate + sodium iodide
lead (II) iodide + sodium nitrate Pb(NO3)2 + 2NaI PbI2 + 2NaNO3 Double replacement
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25. Silver nitrate + sodium sulfide
silver sulfide + sodium nitrate 2AgNO3 + Na2S Ag2S + 2NaNO3 Double replacement
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26. Iodine + potassium chloride
No Reaction
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27. Magnesium oxide + water
magnesium hydroxide MgO + H2O Mg(OH)2 synthesis
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MIXED EQUATION WORKSHEET #2
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Complete the word equation, write the formula equation, balance it and identify the type of reaction. You many abbreviate as S, D, SR, DR, and C.
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1. sodium hydrogen carbonate + hydrochloric acid
sodium hydrogen carbonate + hydrochloric acid sodium chloride + water + carbon dioxide NaHCO3 + HCl NaCl + H2O + CO2 double replacement
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2. Complete combustion of ethanol (C2H5OH)
Ethanol + oxygen carbon dioxide + water C2H5OH + 3O2 2CO2 + 3H2O Combustion
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3. sulfurous acid + magnesium hydroxide
water + magnesium sulfite H2SO3 + Mg(OH)2 2H2O + MgSO3 double replacement
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4. carbonic acid + lithium hydroxide
water + lithium carbonate H2CO3 + 2LiOH 2H2O + Li2CO3 Double replacement
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5. gold + sulfuric acid gold + sulfuric acid No Reaction
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6. aluminum + fluorine aluminum + fluorine aluminum fluoride 2Al + 3F2 2AlF3 Synthesis
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7. calcium oxide + water calcium oxide + water calcium hydroxide CaO + H2O Ca(OH)2 Synthesis
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8. acetic acid + sodium hydroxide
water + sodium acetate HC2H3O2 + NaOH H2O +NaC2H3O2 Double replacement
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9. potassium chloride + lead(II) nitrate
potassium nitrate + lead(II) chloride 2KCl + Pb(NO3)2 2KNO3 + PbCl2 Double replacement
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10. carbon monoxide + oxygen
carbon dioxide 2CO + O2 2CO2 Synthesis
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sodium + chlorine sodium chloride 2Na + Cl2 2NaCl Synthesis
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12. dinitrogen pentoxide + water
nitric acid N2O5 + H2O H2N2O6 2HNO3 Synthesis
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13. bromine + sodium chloride
No rxn
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14. potassium chloride + mercury(I) nitrate
potassium nitrate + mercury(I) chloride 2KCl + Hg2(NO3)2 2KNO3 + Hg2Cl2 Double replacement
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15. sulfur dioxide + water
sulfurous acid SO2 + H2O H2SO3 Synthesis
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lithium oxide + water lithium hydroxide Li2O + H2O 2LiOH Synthesis
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17. heating zinc carbonate
zinc oxide + carbon dioxide ZnCO3 ZnO + CO2 Decomposition
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18. silver nitrate + sodium chloride
silver chloride + sodium nitrate AgNO3 + NaCl AgCl + NaNO3 Double replacement
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19. heating beryllium chlorate
beryllium chloride + oxygen Be(ClO3)2 BeCl2 + 3O2 Decomposition
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20. electrolysis of water
water hydrogen + oxygen 2H2O 2H2 + O2 Decomposition
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21. complete combustion of butane (C4H10)
Butane + oxygen carbon dioxide + water 2C4H O2 8CO2 + 10H2O Combustion
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22. iron(II) sulfate + ammonium sulfide
iron(II) sulfide + ammonium sulfate FeSO4 + (NH4)2S FeS + (NH4)2SO4 Double replacement
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23. lithium + water lithium + water lithium hydroxide + hydrogen 2Li + 2H2O 2LiOH + H2 Single replacement
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24. potassium oxide + water
potassium hydroxide K2O + H2O 2KOH Synthesis
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25. silver + sulfur silver + sulfur silver sulfide 2Ag + S Ag2S Synthesis
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26. sodium + water sodium + water sodium hydroxide + hydrogen 2Na + 2H2O 2NaOH + H2 Single replacement
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27. calcium hydroxide + ammonium sulfate
calcium sulfate + ammonia + water Ca(OH)2 + (NH4)2SO4 CaSO4 + 2NH3 + 2H2O Double replacement
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NET IONIC EQUATIONS
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Net ionic equations show only the species actually involved in the reaction. As you first learn to write net ionic equations, you will write three different equations for each reaction.
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Steps in writing net ionic equations:
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1. Write the complete molecular equation
1. Write the complete molecular equation. (This is the type of equation that you are accustomed to writing.)
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2. Write the complete ionic equation
2. Write the complete ionic equation. To do this, you must ionize everything that is soluble and ionized in solution. Everything else is left together. Do not ionize solids, gases or weak electrolytes.
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3. Write the net ionic equation
3. Write the net ionic equation. To do this, cancel out all ions that are not participating in the reaction (spectator ions) and rewrite the equation.
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Sodium chloride + silver nitrate
1. NaCl(aq) + AgNO3(aq) NaNO3(aq) + AgCl(s) 2. Na+ + Cl- + Ag+ + NO3- Na+ + NO3- + AgCl(s) 3. Cl- + Ag+ AgCl
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Ex. HCl + Ba(OH)2 1. 2HCl + Ba(OH)2 2H2O + BaCl2
3. 2H+ + 2OH- 2H2O H+ + OH- H2O
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Write net ionic equations for the following reactions:
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1. KCl(aq) + Pb(NO3)2(aq) 2KCl(aq) + Pb(NO3)2(aq)
2KNO3(aq) + PbCl2(s) 2K+ + 2Cl- + Pb2+ + 2NO3- 2K+ + 2NO3- + PbCl2 Pb2+ + 2Cl- PbCl2
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2. HCl(aq) + CaSO3(s) 2HCl(aq) + CaSO3(s)
H2O(l) + SO2(g) + CaCl2(aq) 2H+ + 2Cl- + CaSO3 H2O + SO2 + Ca2+ + 2Cl- 2H+ + CaSO3 H2O + SO2 + Ca2+
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3. Zn(s) + O2(g) 2Zn(s) + O2(g) 2ZnO(s)
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4. Li(s) + H2O(l) 2Li(s) + 2H2O(l) 2LiOH(aq) + H2(g)
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5. Na2SO4(aq) + BaBr2(aq) Na2SO4(aq) + BaBr2(aq)
2NaBr(aq) + BaSO4(s) 2Na+ + SO42- + Ba2+ + 2Br- 2Na+ + 2Br- + BaSO4 SO42- + Ba2+ BaSO4
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6. MgCO3(s) MgCO3(s) MgO(s) + CO2(g)
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7. AgNO3(aq) + Na2CO3(aq) 2AgNO3(aq) + Na2CO3(aq)
Ag2CO3(s) + 2NaNO3(aq) 2Ag+ + 2NO3- + 2Na+ + CO32- Ag2CO3 + 2Na+ + 2NO3- 2Ag+ + CO32- Ag2CO3
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8. Na2S(aq) + HCl(aq) Na2S(aq) + 2HCl(aq) 2NaCl(aq) + H2S(g)
2Na+ + S2- + 2H+ + 2Cl- 2Na+ + 2Cl- + H2S S2- + 2H+ H2S
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9. H2SO3(aq) H2SO3(aq) H2O(l) + SO2(g)
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10. Cl2(g) + NaI(aq) Cl2(g) + 2NaI(aq) I2(s) + 2NaCl(aq) Cl2 + 2Na+ + 2I- I2 + 2Na+ + 2Cl- Cl2 + 2I- I2 + 2Cl-
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EXTRA EQUATION WORKSHEET PRE-AP CHEMISTRY
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Complete the word equation, write the formula equation, balance it and identify the type of reaction. You many abbreviate as S, D, SR, DR, and C.
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1. heating magnesium carbonate
magnesium oxide + carbon dioxide MgCO3 MgO + CO2 Decomposition
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2. complete combustion of propanol (C3H7OH)
propanol + oxygen carbon dioxide + water 2C3H7OH + 9O2 6CO2 + 8H2O Combustion
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S + O2 SO2 Synthesis 3. sulfur + oxygen
sulfur + oxygen sulfur dioxide S + O2 SO2 Synthesis
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4. sulfuric acid + cadmium
cadmium sulfate + hydrogen H2SO4 + Cd CdSO4 + H2 Single Replacement
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5. sulfur dioxide + water
sulfurous acid SO2 + H2O H2SO3 Synthesis
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6. hydrochloric acid(aq) + calcium carbonate(s)
carbon dioxide(g) + water(l) + calcium chloride(aq) 2HCl + CaCO3 CO2 + H2O + CaCl2 Double replacement
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7. net ionic equation for #6
1. 2HCl(aq) + CaCO3(s) CO2(g) + H2O(l) + CaCl2(aq) 2. 2H+ + 2Cl- + CaCO3 CO2 + H2O + Ca2+ + 2Cl- 3. 2H+ + CaCO3 CO2 + H2O + Ca2+
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8. silver nitrate (aq)+ hydrochloric acid (aq)
silver chloride(s) + nitric acid(aq) AgNO3 + HCl AgCl + HNO3 Double replacement
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9. net ionic equation for #8
1. AgNO3(aq) + HCl(aq) AgCl(s) + HNO3(aq) 2. Ag+ + NO3- + H+ + Cl- AgCl(s) + H+ + NO3- 3. Ag+ + Cl- AgCl(s)
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10. barium nitrate(aq) + potassium sulfate (aq)
barium sulfate(s) + potassium nitrate(aq) Ba(NO3)2 + K2SO4 BaSO4 + 2KNO3 Double Replacement
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11. net ionic equation for #10
1. Ba(NO3)2 (aq) + K2SO4(aq) BaSO4(s) + 2KNO3(aq) 2. Ba2+ + 2NO3- + 2K+ + SO42- BaSO4 + 2K+ + 2NO3- 3. Ba2+ + SO42- BaSO4
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12. sodium hydroxide + phosphoric acid
sodium phosphate + water 3NaOH + H3PO4 Na3PO4 + 3H2O Double replacement
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13. iodine + rubidium chloride
iodine + rubidium chloride No Rxn
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14. magnesium(s) + copper(II) sulfate(aq)
magnesium sulfate(aq) + copper(s) Mg + CuSO4 MgSO4 + Cu Single replacement
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15. net ionic equation for #14
1. Mg(s) + CuSO4(aq) MgSO4(aq) + Cu(s) 2. Mg + Cu2+ + SO42- Mg2+ +SO42- + Cu 3. Mg + Cu2+ Mg2+ + Cu
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16. ammonium nitrate(aq) + sodium hydroxide(aq)
ammonium nitrate(aq) + sodium hydroxide(aq) ammonia (g)+ water (l) + sodium nitrate (aq) NH4NO3 + NaOH NH3 + H2O + NaNO3 Double replacement
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17. net ionic equation for #16
1. NH4NO3(aq) + NaOH(aq) NH3(g) + H2O(l) + NaNO3(aq) 2. NH4+ + NO3- + Na+ + OH- NH3 + H2O + Na+ + NO3- 3. NH4+ + OH- NH3 + H2O
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18. potassium(s) + water(l)
potassium hydroxide(aq) + hydrogen(g) 2K + 2H2O 2KOH + H2 Single Replacement
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19. net ionic equation for #18
1. 2K(s) + 2H2O(l) 2KOH(aq) + H2(g) 2. 2K + 2H2O 2K+ + 2OH- + H2
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20. sodium bromide(aq) + chlorine(g)
sodium chloride + bromine 2NaBr + Cl2 2NaCl + Br2 Single replacement
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21. net ionic equation for #20
1. 2NaBr(aq) + Cl2(g) 2NaCl(aq) + Br2(l) 2. 2Na+ + 2Br- + Cl2 2Na+ + 2Cl- + Br2 3. 2Br- + Cl2 2Cl- + Br2
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aluminum + nitrogen aluminum nitride 2Al + N2 2AlN Synthesis
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23. sodium sulfide(aq) + hydrochloric acid(aq)
sodium sulfide(aq) + hydrochloric acid(aq) sodium chloride (aq) + hydrogen sulfide (g) Na2S + 2HCl 2NaCl + H2S Double replacement
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24. net ionic equation for #23
1. Na2S(aq) + 2HCl(aq) 2NaCl(aq) + H2S(g) 2. 2Na+ + S2-+ 2H+ + 2Cl- 2Na+ + 2Cl-+ H2S 3. S2-+ 2H+ H2S
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25. heating magnesium sulfate heptahydrate
magnesium sulfate + water MgSO4.7H2O MgSO4 + 7H2O Decomposition
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26. heating mercury(II) oxide
mercury + oxygen 2HgO 2Hg + O2 Decomposition
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27. bromine + strontium chloride
bromine + strontium chloride No Rxn
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1. Dilute hydrochloric acid is added to a solution of potassium sulfite.
2HCl(aq) +K2SO3(aq) H2O(l) + SO2(g) +2KCl(aq) 2H+ + 2Cl- +2K+ + SO32- H2O(l) + SO2(g) +2K+ +2Cl- 2H+ + SO32- H2O(l) + SO2(g)
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2. A solution of sodium sulfide is added to a solution of zinc nitrate.
Na2S(aq) + Zn(NO3)2(aq) 2NaNO3(aq) + ZnS(s) 2Na+ + S2- + Zn2+ + 2NO3- 2Na+ + 2NO3- + ZnS S2- + Zn2+ ZnS
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3. Chlorine gas is bubbled into a solution of potassium iodide.
Cl2(g) + 2KI(aq) 2KCl(aq) + I2(s) Cl2 + 2K+ + 2I- 2K+ + 2Cl- + I2 Cl2 + 2I- -> 2Cl- + I2
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4. Magnesium metal is burned in nitrogen gas.
3Mg(s) + N2(g) Mg3N2(s)
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5. Solid sodium oxide is added to water.
Na2O(s) + H2O(l) 2NaOH(aq) Na2O(s) + H2O(l) 2Na+(aq) + 2OH-(aq)
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