Q Balance the following equations and state what reaction type is taking place: 1) C5H12 + O2 ???CO2 + H2O + heat Reaction type: 2) K3PO4 + BaCl2 ???Ba3(PO4)2 + KCl Reaction type: 3) Al(OH)3 + H2SO4 ???Al2(SO4)3 + H2O Reaction type: 4) HCl + K2CO3 ???CO2 + H2O + KCl Reaction type: 5) AgNO3 + Na2CO3 ???Ag2CO3 + NaNO3 Reaction type: 6) Al2O3 + heat ???Al + O2 Reaction type: 7) Al + HCl ???H2 + AlCl3 Reaction type: 8) Cu(OH)2 ???H2O + CuO Reaction type: Everett Community College Student Support Services Program WORKSHOP 4: Name: Writing and Balancing Equations Section _ Part 1: Write and balance the following word equations. Remember that hydrogen, oxygen, nitrogen, chlorine, and bromine are diatomic molecules. 1. Magnesium metal and oxygen gas yield magnesium oxide. 2. Potassium chlorate, when heated, decomposes to potassium chloride and oxygen. 3. Solid iron reacts with oxygen gas to produce rust (a combination of iron oxides with a formula of Fe3O4). 4. Magnesium metal and hydrochloric acid react to yield magnesium chloride and hydrogen gas. 5. Sodium metal reacts with water to produce sodium hydroxide and hydrogen gas. 6. Sulfur reacts with oxygen to form sulfur dioxide. 7. Solid zinc and sulfuric acid react to form zinc sulfate and hydrogen gas. 8. Carbon and oxygen gas react to produce carbon dioxide. 9. Hydrogen and oxygen react to yield water. 1. Solid aluminum reacts with hydrochloric acid to produce aluminum chloride and hydrogen gas. 11. Nitrogen and hydrogen are gases that react to form ammonia gas (NH3). 12. Fluorine gas reacts with water to give hydrogen fluoride and oxygen gas 1. Lead (II) nitrate decomposes, when heated, to yield lead (II) oxide, nitrogen monoxide gas, and oxygen gas 14. Aluminum and oxygen, when heated together, give aluminum oxide. 15. Phosphorus and bromine will react and form phosphorus tribromide. 16. Sodium hydrogen carbonate reacts with nitric acid to yield sodium nitrate and water and carbon dioxide. 17. Xenon gas and fluorine gas react over a platinum catalyst to form xenon hexafluoride. Name Section Part 2: Complete and balance the following double displacement reactions. Use the chart on page 62 to predict insoluble products. 1. Sodium chloride solution reacts with a silver nitrate solution. 1. Barium chloride solution reacts with sulfuric acid. 2. Sodium hydroxide reacts with hydrochloric acid. 3. Solutions of Iron (III) chloride and silver nitrate are mixed. 4. Phosphoric acid reacts with a solution of calcium hydroxide. 5. Potassium carbonate solution reacts with a solution of cobalt(II) bromide. 6. Bismuth(III) chloride solution reacts with hydrosulfuric acid. 7. Potassium acetate solution reacts with hydrochloric acid. 8. Sodium sulfite solution reacts with hydrochloric acid. Workshop 4, page 4 Single Replacement Reactions: Activity Series Li > K > Ba > Sr > Ca > Na > Mg > Al > Mn > Zn > Fe > Cd > Co > Ni > Sn > Pb The above elements all replace hydrogen from acids. The most active can replace H from water (Li – Na) . Mg can slowly react with hot water. Al – Pb react with acids but not with water. H > Cu > Ag > Hg > Au (Cu, Hg, Ag, do not replace H from acids) Predict whether the following will react, and what the products will be if they do. If no reaction is predicted, write NR. Balance the equations 9. H2 + CuO ? 10. Mg + MnCl2 ? 11. Mg + AgNO3 ? 12. K + Na2SiO3 ? 13. Cu + Fe2O3 ? Decomposition Reactions 14. Mg (OH)2 ? 15. H2CO3 ? 16. LiClO4 ? Combination reactions 17. P2O3 + H2O ? 18. SO2 + H2O ? Honors Chemistry Name Period Net Ionic Equation Worksheet READ THIS: When two solutions of ionic compounds are mixed, a solid may form. This type of reaction is called a precipitation reaction, and the solid produced in the reaction is known as the precipitate. You can predict whether a precipitate will form using a list of solubility rules such as those found in the table below. When a combination of ions is described as insoluble, a precipitate forms. There are three types of equations that are commonly written to describe a precipitation reaction. The molecular equation shows each of the substances in the reaction as compounds with physical states written next to the chemical formulas. The complete ionic equation shows each of the aqueous compounds as separate ions. Insoluble substances are not separated and these have the symbol (s) written next to them. Water is also not separated and it has a (l) written next to it. Notice that there are ions that are present on both sides of the reaction arrow –> that is, they do not react. These ions are known as spectator ions and they are eliminated from complete ionic equation by crossing them out. The remaining equation is known as the net ionic equation. For example: The reaction of potassium chloride and lead II nitrate Molecular Equation: 2KCl (aq) + Pb(NO3)2 (aq) -> 2KNO3 (aq) + PbCl2 (s) Complete Ionic Equation: 2K+ (aq) + 2Cl- (aq) + Pb2+ (aq) + 2NO3– (aq) -> 2K+ (aq) + 2NO3– (aq) + PbCl2 (s) Net Ionic Equation: 2Cl- (aq) + Pb2+ (aq) -> PbCl2 (s) Directions: Write balanced molecular, ionic, and net ionic equations for each of the following reactions. Assume all reactions occur in aqueous solution. Include states of matter in your balanced equation. 1. Sodium chloride and lead II nitrate Molecular Equation: Complete Ionic Equation: Net Ionic Equation: 2. Sodium carbonate and Iron II chloride Molecular Equation: Complete Ionic Equation: 3. Magnesium hydroxide and hydrochloric acid Molecular Equation: Complete Ionic Equation: Net Ionic Equation: 4. Potassium chromate and calcium chloride Molecular Equation: Complete Ionic Equation: Net Ionic Equation: 5. Ammonium phosphate and zinc nitrate Molecular Equation: Complete Ionic Equation: Net Ionic Equation: 6. Lithium hydroxide and barium chloride Molecular Equation: Complete Ionic Equation: 7. Sodium carbonate and hydrochloric acid produces sodium chloride, carbon dioxide and water Molecular Equation: Complete Ionic Equation: Net Ionic Equation: 8. Magnesium nitrate and sodium chromate Molecular Equation: Complete Ionic Equation: Net Ionic Equation: 9. Iron III chloride and magnesium metal Molecular Equation: Complete Ionic Equation: Net Ionic Equation: 10. Barium Bromide and sodium sulfate Molecular Equation: Complete Ionic Equation:

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