stoichiometry Chemical Equations Balancing equations 1.The Eq. must represent the known facts. 2. The Eq. must contain the correct formulas for reactants and products. 3. The law of conservation of mass must be followed. 4. Balance atoms that appear once 1st. 5. Treat polyatomics as one unit if they appear on both sides the same way. 6. Balance other elements. 7. Balance H 8. Balance O last!! *NEVER CHANGE A SUBSCRIPT Chemical Reactions and Equations: Basic Concepts Topic 8 Balancing an Equation • The balanced equation tells us that when carbon and oxygen react, one unit of oxygen react with each molecule of carbon to form one unit of carbon dioxide Conservation of Mass and Balancing Equations Click in this box to enter notes. Go to Slide Show View (press F5) to play the video or animation. (To exit, press Esc.) This media requires PowerPoint® 2000 (or newer) and the Macromedia Flash Player (7 or higher). 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Example • Write and balance the reaction between sodium hydroxide and calcium bromide to give calcium hydroxide and sodium bromide NaOH + CaBr2 Ca(OH)2 + NaBr • 2 NaOH + CaBr2 Ca(OH)2 + 2NaBr Here are some more to balance: a) b) c) d) e) f) g) h) i) 2KNO3 2KNO2 + O2 2Pb(NO3)2 2PbO + 4NO2 + O2 P4 + 6I2 4PI3 3MgO + 2H3PO4 Mg3(PO4)2 + 3H2O Br2 + 2KI I2 + 2KBr Ca(OH)2 + 2HNO3 Ca(NO3)2 + 2H2O Bi2O3 + 3H2 2Bi + 3H2O 3Fe + 2O2 Fe3O4 2CaO + 5C 2CaC2 + CO2 Classification of Reactions • There are 5 major classifications of reactions: – Synthesis A + B → AB – Decomposition AB → A + B – Combustion Hydrocarbon + O2 → CO2 + H2O – Single Replacement AB + C → AC + B – Double Replacement AB + CD → AD + CB Chemical Reactions and Equations: Basic Concepts Topic 8 Major Classes of Reactions • In one type of reaction, two substances— either elements or compounds—combine to form a compound. • Whenever two or more substances combine to form a single product, the reaction is called a synthesis reaction. Chemical Reactions and Equations: Basic Concepts Topic 8 A Synthesis Reaction • When iron rusts, iron metal and oxygen gas combine to form one new substance, iron(III) oxide. • The balanced equation for this synthesis reaction shows that there is more than one reactant but only one product. Chemical Reactions and Equations: Basic Concepts Topic 8 A Synthesis Reaction Synthesis (Combination) • Synthesis – when 2 or more substances react to produce 1 product • Of the form: A + B AB • Examples: – 2 Fe + 3 Cl2 2 FeCl3 – 2 Na + Cl2 2NaCl – CaO + H2O Ca(OH)2 – 2Mg + O2 2MgO Synthesis # 1 1. Metal oxide + nonmetal oxide metal oxyanion a salt (Not Redox) • No Redox simply means that the oxidation numbers of the elements stays the same • Oxyanion = a polyatomic ion with oxygen Synthesis # 1 Example • Sulfur dioxide gas is passed over solid calcium oxide • SO2 + CaO • We know that we have to get a metal oxyanion. • So we either get CaSO4 or CaSO3 • We need to check the oxidation states on sulfur to see which one is the same. Synthesis # 1 Example • • • • • • • In SO2, the oxidation number of O is -2 So the oxidation number of S must be +4 Our product choices are CaSO3 or CaSO4 In CaSO3…S has an oxidation # of +4 In CaSO4…S has an oxidation # of +6 Therefore the product must be CaSO3 SO2 + CaO CaSO3 Chemical Reactions and Equations: Basic Concepts Topic 8 Major Classes of Reactions • In a decomposition reaction, a compound breaks down into two or more simpler substances. • The compound may break down into individual elements, such as when mercury(II) oxide decomposes into mercury and oxygen. Chemical Reactions and Equations: Basic Concepts Topic 8 Major Classes of Reactions • The products may be an element and a compound, such as when hydrogen peroxide decomposes into water and oxygen. • The compound may break down into simpler compounds. Chemical Reactions and Equations: Basic Concepts Topic 8 A Decomposition Reaction • When ammonium nitrate is heated to a high temperature, it explosively breaks down into dinitrogen monoxide and water. • The decomposition reaction taking place is represented by a balanced equation that shows one reactant and more than one product. Chemical Reactions and Equations: Basic Concepts Topic 8 A Decomposition Reaction Decomposition • Decomposition – when a single compound breaks down into 2 or more compounds • Of the form: AB A + B • Note that this is the exact opposite of synthesis • Examples: – 2 Na3N 6 Na + N2 – NH4NO3 N2O + 2H2O – 2H2O 2 H2 + O2 Decomposition Synthesis Decomposition Redox Metal + Nonmetal salt Salt Metal + Nonmetal Non Redox Metal oxide + H2O base base Metal oxide + H 2O Nonmetal oxide + H2O acid acid Nonmetal oxide + H2O Metal oxide + Nonmetal oxide salt salt Metal oxide + Nonmetal oxide More Decomposition • • • • Metal chlorates metal chloride + O2 (NH4)2CO3 2NH3 + H2O + CO2 2H2O2 2H2O + O2 If you get any of these products…they decompose… – – – – NH4OH NH3 + H2O H2CO3 CO2 + H2O H2SO3 SO2 + H2O HNO2 NO + NO2 + H2O Chemical Reactions and Equations: Basic Concepts Topic 8 Major Classes of Reactions • A combustion reaction is one in which a substance rapidly combines with oxygen to form one or more oxides. Click box to view movie clip. Chemical Reactions and Equations: Basic Concepts Topic 8 Combustion • When welding is done with an acetylene torch, acetylene combines with oxygen to form carbon dioxide and water. • This combustion reaction is exothermic, and enough energy is released to melt metal. Chemical Reactions and Equations: Basic Concepts Topic 8 Combustion Combustion • Combustion – when O2 combines with a hydrocarbon to form CO2 and H2O • Of the form: hydrocarbon + O2 CO2 + H2O • For example: – CH4 + 2 O2 CO2 + 2H2O – 2CH3OH + 3O2 2CO2 + 4H2O Combustion 1. • • • Hydrocarbon + O2 CO2+ H2O (No ions) Combustion of methane CH4 + O2 CO2+ H2O CH4 + 2O2 CO2+ 2H2O When Balancing Combustion Reactions • Put a two in front of the hydrocarbon to start. • Balance them in the order C, H, O • Make sure your answer is in the lowest whole number ratio Chemical Reactions and Equations: Basic Concepts Topic 8 Major Classes of Reactions • In a single-displacement reaction, one element takes the place of another in a compound. • The element can replace the first part of a compound, or it can replace the last part of a compound. Chemical Reactions and Equations: Basic Concepts Topic 8 Single Displacement • If an iron nail is placed into an aqueous solution of copper(II) sulfate, the iron displaces the copper ions in solution, and copper metal forms on the nail. Chemical Reactions and Equations: Basic Concepts Topic 8 Single Displacement Single Replacement • Single Replacement – when the atoms of one element replace the atoms of another element in a compound • Of the form : A + BX B + AX • For example: – 2 Li + 2H2O 2 LiOH + H2 – Cu + 2AgNO3 2 Ag + Cu(NO3)2 Activity Series Page 286 TABLE 3 in your text book Single Replacement Reactions • In order for a single replacement reaction to occur, the element that is by itself must be strong enough to push the other element out of the way. • The activity series show you the relative pushing power of the elements. • In order for the reaction to occur, the lone element must be above the element in the compound • Otherwise…NO REACTION NR Single Replacement Reactions • You need to know which chart you are to look at…metals or halogens. • A metal can replace another metal • A halogen can replace another halogen Will these reactions occur? • Will the following reaction occur? If so, complete and balance the reaction. • Ag + Cu(NO3)2 • Ag + Cu(NO3)2 NR • No reaction because Ag is below Cu in the Activity series of metals Will these reactions occur? • Will the following reaction occur? If so, complete and balance the reaction. • Mg + AlCl3 • 3Mg + 2AlCl3 3MgCl2 + 2 Al • The reaction WILL occur because Mg is above Al in the activity series Will these reactions occur? • Will the following reaction occur? If so, complete and balance the reaction. • Br2 + MgCl2 • Br2 + MgCl2 NR • This reaction will NOT occur because Br is not above Cl in the activity series of halogens Double Replacement • Double Replacement – a reaction involving the exchange of ions between 2 compounds • Of the form: AX + BY BX + AY Chemical Reactions and Equations: Basic Concepts Topic 8 Major Classes of Reactions • In double-displacement reactions, the positive portions of two ionic compounds are interchanged. • For a double-displacement reaction to take place, at least one of the products must be a precipitate or water. Chemical Reactions and Equations: Basic Concepts Topic 8 Double Displacement • When clear aqueous solutions of lead(II) nitrate and potassium iodine are mixed, a double-displacement reaction takes place and a yellow solid appears in the mixture. • This solid is lead(II) iodine, and it precipitates out because it is insoluble in water, unlike the two reactants and the other product. Chemical Reactions and Equations: Basic Concepts Topic 8 Double Displacement Double Replacement (Metathesis) • Double Replacement – a reaction involving the exchange of ions between 2 compounds • Of the form: AX + BY BX + AY • Examples: – Pb(NO3)2 + 2KI PbI2 + 2KNO3 – Na2CO3 + 2AgNO3 2NaNO3 + Ag2CO3 Double Replacement (Metathesis) • In order for a double replacement reaction to take place, one of 3 things must be formed: • Precipitate (solid) • Gas • Weak electrolyte – usually water Precipitation Reactions Click in this box to enter notes. Go to Slide Show View (press F5) to play the video or animation. (To exit, press Esc.) This media requires PowerPoint® 2000 (or newer) and the Macromedia Flash Player (7 or higher). [To delete this message, click inside the box, click the border of the box, and then press delete.] Copyright © Houghton Mifflin Company. All rights reserved. Solubility Rules!!! Double Replacement # 2 (Formation of a gas) 2. • • • • • • Formation of a gas (acid + sulfide, sulfite, carbonate, or bicarbonate…or ammonium salt + a strong base NH3(g), H2O, and a salt) Hydrobromic acid is added to a solution of potassium bicarbonate HBr + KHCO3 HBr + KHCO3 H2CO3 + KBr H2CO3 ALWAYS breaks down into CO2 + H2O HBr + KHCO3 CO2 + H2O + KBr H+ + HCO3- CO2 + H2O Double Replacement #4 (Acid Base neutralization) • Acid + base salt + water • Hydrogen sulfide gas is bubbled through excess potassium hydroxide solution • H2S + 2KOH 2HOH + K2S • H2S + 2K+ + 2OH- 2H2O + 2K+ + S-2 • H2S + 2OH- 2H2O + S-2 Proton Transfer Click in this box to enter notes. Go to Slide Show View (press F5) to play the video or animation. (To exit, press Esc.) This media requires PowerPoint® 2000 (or newer) and the Macromedia Flash Player (7 or higher). [To delete this message, click inside the box, click the border of the box, and then press delete.] Copyright © Houghton Mifflin Company. All rights reserved. Ionic Equations Equations • Molecular equations – show the complete chemical formulas. Does not indicate ionic character • Complete ionic equation – shows all ions. Actually how the particles exist in the solution Steps for Writing Ionic Equations 1. Write the balances molecular equation (balanced chemical equation) 2. Break every thing down into its ions EXCEPT the solid, gas, or water (complete ionic equation) 3. Cross out everything that is the same on both sides (spectator ions) 4. Write what is left (net ionic equation) Rules • When writing ionic equations, you must keep together the solid, gas, or water • Spectator ions – ions that appear on both sides of the equation. They have very little to do with the chemical reaction Example • Write the balanced chemical equation, the complete ionic equation, and the net ionic equation for the reaction between lead (II) nitrate and potassium iodide. Solid potassium iodide will be formed. Example • • • • • Write the balanced chemical equation Pb(NO3)2 + 2 KI PbI2 + 2 KNO3 You MUST identify the solid, gas, or water Pb(NO3)2 + 2 KI PbI2 (s) + 2 KNO3 Balanced chemical equation Example • Now break every thing except the solid, gas, or water into its ions • Remember ions are things with charges • Everything will be broken down into one positive charge and one negative charge Example • Pb(NO3)2 + 2 KI PbI2 (s) + 2 KNO3 • Pb+2 + 2NO3-1 + 2K+1 + 2 I -1 PbI2 (s) + 2K+1 + 2NO3-1 • Complete ionic Equation Example • Now cross out everything that is the same on both sides (spectator ions) • Pb+2 + 2NO3-1 + 2K+1 + 2 I -1 PbI2 (s) + 2K+1 + 2NO3-1 • Pb+2 + 2NO3-1 + 2K+1 + 2 I -1 PbI2 (s) + 2K+1 + 2NO3-1 • Now write what is left • Pb+2 + 2 I -1 PbI2 (s) • Net ionic equation Another Example • Write the balanced chemical equation, complete ionic equation, and net ionic equation for the reaction between calcium chloride and sodium carbonate. Solid calcium carbonate will be formed. Another Example • Balanced chemical equation • CaCl2 + Na2CO3 CaCO3 (s) + 2NaCl • Complete ionic equation • Ca+2 + 2Cl -2 + 2Na +1 + CO3 -2 CaCO3 (s) + 2Na +1 + 2Cl -1 • Net Ionic Equation • Ca+2 + 2Cl -2 + 2Na +1 + CO3 -2 CaCO3 (s) + 2Na +1 + 2Cl -1 • Ca+2 + CO3 -2 CaCO3 (s) What if water is formed? • Write the balanced chemical equation, complete ionic equation, and net ionic equation for the reaction between Calcium hydroxide and nitric acid Example with water • Balanced chemical equation • Ca(OH)2 + 2 HNO3 Ca(NO3)2 + 2 HOH • Complete ionic equation • Ca+2 + 2(OH) -1 + 2H+1 + 2NO3 -1 Ca+2 + 2NO3 -1 + 2 HOH • Net Ionic Equation • Ca+2 + 2(OH) -1 + 2H+1 + 2NO3 -1 Ca+2 + 2NO3 -1 + 2 HOH • 2(OH) -1 + 2H+1 2 HOH Stoichiometry • Using the methods of stoichiometry, we can measure the amounts of substances involved in chemical reactions and relate them to one another. Stoichiometry Rules • 1. Balance the equation. • 2. convert all units to moles • 3. use a molar ratio from the balanced equation to compare what is given to what you want. • 4. convert back from moles to the unit the question asks for. • Always no matter what unit you are given convert it to moles before you make a comparison. Coefficients • Coefficients in a balanced chemical RXN can represent any of the following • 1. moles • 2. molecules of a compound • 3. volume of a gas at STP. (22.7 L=1mol) • * they never represent mass. Mole – Mole Relationship • 4 Fe + 3O2 2Fe2O3 • 4 mol Fe / 3 mol O2 • 4 mol Fe / 2 mol Fe2O3 • 3mol O2 / 2 mol Fe2O3 Mole – Mole Relationship • How many moles of Fe2O3 will I form from 5.0 mol of Fe? • 5.0 mole Fe x 2 mol Fe2O3 4 mol Fe • 2.5 mol Fe2O3 Conversion Factor # 3 # Moles A # Moles B The #’s in from if A & B MUST come from the balanced chemical equation Mass – Mole Relationship • How many g of NaCl will be produced from 1.25 mol of chlorine gas reacting with sodium? • Write the reaction • Na + Cl2 NaCl • Balance the reaction • 2Na + Cl2 2NaCl Mass – Mole Relationship • Work the problem • 1.25 mol Cl2 x 2 mol NaCl x 58.44 g NaCl • 1 mol Cl2 1 mol NaCl • 146 g NaCl Mass – Mass Relationships • Ammonium nitrate decomposes into dinitrogen monoxide gas and water. Determine that amount of water produced if 25.0 g of ammonium nitrate decomposes. • NH4NO3 N2O + H2O • NH4NO3 N2O + 2 H2O Mass – Mass Relationships • 25.0 g NH4NO3 x 1 mol NH4NO3 x 2 mol H2O x 18.02 g H2O 80.04 g NH4NO3 1 mol NH4NO3 1 mol H2O • 11.2 g H2O