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Chapter 4 Lecture Notes 1

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Chapter 4 Lecture Notes 1 Usual Atomic Charges of Main Group Elements +1 +2+3 +4 +5 +6 +7 -5 -4 -3 -2 -1 Examples SO3 sulfur trioxide CO2 carbon dioxide Al2O3 aluminum trioxide IF7 iodine heptafluoride Fig. 2-6, p.63 Chemical Equations A chemical equation—just like a mathematical equation—is a way to express, in symbolic form, the reactions occurring in a chemical system. Balancing chemical equations Reaction stoichiometry Reagents limiting the extent of reaction Acid-base reactions Oxidation states of reactants and products 1 Types of Chemical Reactions Combination Reactions: Atoms or molecules combine to form a new molecule → 2H2 + O2 2H2O → ClO + NO2 ClNO3 ClO + ClO → ClOOCl Types of Chemical Reactions Decomposition Reactions: A molecule breaks apart to form different molecules or atoms → NO2 + sunlight O + NO 2C7H5(NO2)3 + heat → 7CO(g) + 7C + 5H2O(g) + 3N2(g) 2 Types of Chemical Reactions Displacement Reactions: An atom or molecule displaces an atom or molecule in the reaction partner → H + Cl2 HCl + Cl → 2Na(s) + 2H2O(l) 2NaOH(aq) + H2(g) Types of Chemical Reactions Exchange Reactions: The components of two compounds are exchanged BaCl2(aq) + Na2SO4(aq) → BaSO4(s) + 2NaCl(aq) 3NaOH(aq) + H3PO4(aq) → Na3PO4(aq) + 3H2O(l) 3 Balancing Chemical Equations Remember Conservation of Mass rule—matter is neither created nor destroyed in a chemical reaction. A balanced chemical equation must have the same number of each type of atom on the reactant side as on the product side. Balancing Chemical Equations Process for balancing chemical equations: 1. Determine correct chemical formulas of all reactants and products 2. Start with “heavier” atoms—balance number of these on reactant and product sides of equation 3. If elements appear in equation as either reactants or products, balance these last 4. Electrical charge must be balanced 4 Balanced Chemical Equations Examples Write a balanced chemical equation for the reaction of Fe(III) with oxygen to form iron oxide → 1. Fe + O2 Fe2O3 → 2. 2 Fe + O2 Fe2O3 Fe is currently balanced → 3. 2 Fe + 3/2 O2 Fe2O3 O is now balanced coefficients must usually be integer numbers—multiply everything by 2 to remove 3/2 denominator: → 4 Fe + 3 O2 2 Fe2O3 Balanced Chemical Equations Examples Write a balanced chemical equation for the combustion of methane—combustion is reaction with oxygen producing a flame. Complete combustion produces only CO2 and H2O. 5 Balanced Chemical Equations Examples → 1. CH4 + O2 CO2 + H2O → 2a. CH4 + O2 CO2 + H2O C is now balanced → 2b. CH4 + O2 CO2 + 2 H2O H is now balanced → 3. CH4 + 2 O2 CO2 + 2 H2O O is now balanced → CH4 + 2 O2 CO2 + 2 H2O Balanced Chemical Equations Examples Combustion of propane, C3H8 → 1. C3H8 + O2 CO2 + H2O → 2a. C3H8 + O2 3 CO2 + H2O → 2b. C3H8 + O2 3 CO2 + 4 H2O → 3. C3H8 + 5 O2 3 CO2 + 4 H2O 4. No charges to balance → C3H8 + 5 O2 3 CO2 + 4 H2O 6 Balanced Chemical Equations Examples Reaction of ammonium perchlorate with aluminum → NH4ClO4(s) + Al(s) Al2O3(s) + N2(g) + HCl(g) + H2O(g) 2a. Balance N: 2 NH4ClO4(s) + Al(s) → Al2O3(s) + N2(g) + HCl(g) + H2O(g) 2b. Balance Cl: 2 NH4ClO4(s) + Al(s) → Al2O3(s) + N2(g) + 2 HCl(g) + H2O(g) Balanced Chemical Equations Examples Reaction of ammonium perchlorate with aluminum (con’t.) 2c. Balance H: 2 NH4ClO4(s) + Al(s) → Al2O3(s) + N2(g) + 2 HCl(g) + 3 H2O(g) 2d. Balance O: 2 NH4ClO4(s) + Al(s) → 5/3 Al2O3(s) + N2(g) + 2 HCl(g) + 3 H2O(g) 7 Balanced Chemical Equations Examples Reaction of ammonium perchlorate with aluminum (con’t.) 3a. Balance Al: 2 NH4ClO4(s) + 10/3 Al(s) → 5/3 Al2O3(s) + N2(g) + 2 HCl(g) + 3 H2O(g) 3b. Remove fractional coefficients (multiply by 3): 6 NH4ClO4(s) + 10 Al(s) → 5 Al2O3(s) + 3 N2(g) + 6 HCl(g) + 9 H2O(g) Balanced Chemical Equations Examples + → 2+ ℓ Mg(s) + H3O (aq) Mg (aq) + H2(g) + H2O( ) 1. As written, the only element out of balance is the hydrogen—balance H first: + → 2+ ℓ Mg(s) + 2 H3O (aq) Mg (aq) + H2(g) + 2 H2O( ) 2. Check charge balance: left-hand side has total charge of +2 (2 * 1+ charge on hydronium ion) Right-hand side has total charge of +2 (2+ charge on Mg ion) 8 Stoichiometry of Chemical Reactions For the generic chemical reaction aA + bB + … → xX + yY + … A, B, X, and Y represent the atoms or molecules reacting and forming, and the coefficients a, b, x, and y represent the stoichiometric coefficients—they tell how many moles of one substance reacts with another substance to form some number of moles of the products. Stoichiometry It is important to remember that the stoichiometric coefficients represent numbers of moles, not masses of reactants and products 9 Stoichiometry How much carbon dioxide is produced by burning one gallon of gasoline? Gasoline is composed of many hydrocarbons, but let’s assume they are all iso-octane (C8H18) -1 Isooctane has a density of 0.6980 g mL 1 gal = 3.785 L = 3785 mL Stoichiometry Mass of isooctane -1 (0.6980 g mL ) (3785 mL) = 2642 g C8H18 Molar mass: 8(12.011 g mol-1) + 18(1.0079 g mol-1) = 114.230 g mol-1 Moles C8H18: -1 (2642 g) / (114.230 g mol ) = 23.13 mol C8H18 10 Stoichiometry Balanced chemical equation: → 2 C8H18 + 25 O2 16 CO2 + 18 H2O Determine moles of CO2 produced: (16 mol CO2) (23.13 mol C8H18) = 185.0 mol CO2 (2 mol C8H18) Stoichiometry Determine mass of CO2: -1 (185.0 mol CO2) (44.009 g mol ) = 8142 g CO2 = 8.142 kg CO2 per gallon of gasoline consumed How much CO2 is emitted by CA every year? Californians consume ~1.4 x 1010 gallons of gasoline each year. 10 -1 (1.4 x 10 gal) (8.142 kg CO2 gal ) 11 = 1.1 x 10 kg CO2 11 Stoichiometry The following general expression applies to stoichiometry problems: (Coefficient B) Moles B = (Moles A) (Coefficient A) Limiting Reagents Suppose the amount of one the reactant in a chemical reaction is insufficient to allow the reaction to proceed to completion. That reactant is called the limiting reagent. The limiting reagent limits how much product can formed in a reaction. 12 Limiting Reagents 6 NH4ClO4(s) + 10 Al(s) → 5 Al2O3(s) + 3 N2(g) + 6 HCl(g) + 9 H2O(g) If we begin with 1.00 kg ammonium perchlorate and 0.100 kg aluminum, how many moles of gaseous product will be produced? 1. Which reactant will be consumed first? -1 (1000 g NH4ClO4)/(117.488 g mol ) = 8.51 mol NH4ClO4 (100 g Al)/(26.982 g mol-1) = 3.71 mol Al Limiting Reagents 1a. How much Al required for NH4ClO4 to react completely? (10 mol Al) (8.51 mol = 14.2 mol Al (6 mol NH4ClO4) NH4ClO4) Since we only have 3.71 mol Al, there is insufficient Al for the NH4ClO4 to react completely, so Al is the limiting reagent. 2. Determine moles of each gaseous product formed in reaction: 13 Limiting Reagents (3 mol N2) (3.71 mol Al) = 1.11 mol N (10 mol Al) 2 (6 mol HCl) (3.71 mol Al) = 2.23 mol HCl (10 mol Al) (9 mol H2O) (3.71 mol Al) = 3.34 mol H O (10 mol Al) 2 Total gas phase product = 6.68 mol Limiting Reagents Example Ammonia reacts with nitric oxide to form nitrogen gas and water: → NH3 + NO N2 + H2O If 71.4 g NH3 reacts with 168.6 g NO, how much N2 and H2O will be produced? Step 1: Balance the chemical equation 14 Limiting Reagents → Example (con’t.): NH3 + NO N2 + H2O Step 1: Balance the chemical equation → 2 NH3 + NO N2 + 3 H2O H balanced → 2 NH3 + 3 NO N2 + 3 H2O O balanced → 2 NH3 + 3 NO 5/2 N2 + 3 H2O N balanced → 4 NH3 + 6 NO 5 N2 + 6 H2O remove fractional coefficient Limiting Reagents → Example (con’t.): NH3 + NO N2 + H2O Step 2: Determine moles of reactants 71.4 g NH 3 = 4.19 mol NH w 17.031 g /mol 3 168.6 g NO = 5.62 mol NO 30.006 g/mol Step 3: Determine which is limiting reagent (4 mol NH3) = NO is limiting (5.62 mol NO) 3.75 mol NH3 (6 mol NO) reagent 15 Limiting Reagents → Example (con’t.): NH3 + NO N2 + H2O Step 4: Determine amount of products ( 5 mol N ) (5.62 mol NO) 2 = 4.68 mol N (6 mol NO) 2 = (4.68 mol N2 ) (28.014 g/mol) 131 g N2 (6 mol H O) (5.62 mol NO) 2 = 5.62 mol H O (6 mol NO) 2 = (5.62 mol H2O) (18.0152 g/mol) 101 g H2O Limiting Reagents Example Ca5(PO4)3F + 5 H2SO4 + 10 H2O → 3 H3PO4 + 5 CaSO4·2H2O + HF compound initial mass initial moles Ca5(PO4)3F 1000. g 1.983 mol H2SO4 200.0 g 2.039 mol H2O 100.0 g 5.551 mol Determine mass of all products formed 16 Limiting Reagents Example: Ca5(PO4)3F + 5 H2SO4 + 10 H2O → 3 H3PO4 + 5 CaSO4·2H2O + HF Step 1: Determine limiting reagent—examine Ca5(PO4)3F (5 mol H2SO 4 ) = (1.983 mol Ca5 ...) 9.915 mol H2SO4 for complete rxn (1 mol Ca5 ...) (10 mol H2O) = (1.983 mol Ca5 ...) 19.83 mol H2O for complete rxn (1 mol Ca5 ...) Not enough H2SO4 or H2O to react completely with Ca5(PO4)3F ∴ Ca5(PO4)3F is not limiting reagent Limiting Reagents Example: Ca5(PO4)3F + 5 H2SO4 + 10 H2O → 3 H3PO4 + 5 CaSO4·2H2O + HF Step 1: Determine limiting reagent—examine H2SO4 (10 mol H2O) = (2.039 mol H2SO 4 ) 4.078 mol H2O for complete rxn (5 mol H2SO4 ) H2O is in excess relative to the amount needed to react completely with H2SO4 ∴ H2SO4 is limiting reagent 17 Limiting Reagents Example: Ca5(PO4)3F + 5 H2SO4 + 10 H2O → 3 H3PO4 + 5 CaSO4·2H2O + HF Step 2: Determine amount of product formed (3 mol H3PO4 ) = (2.039 mol H2SO 4 ) 1.223 mol H3PO 4 w (5 mol H2SO4 ) = (1.223 mol H3PO 4 ) ( 97.995 g/mol) 119.8 g H3PO4 Limiting Reagents Example: Ca5(PO4)3F + 5 H2SO4 + 10 H2O → 3 H3PO4 + 5 CaSO4·2H2O + HF Step 2: Determine amount of product formed ⋅ (5 mol CaSO4 2H2O) = (2.039 mol H2SO 4 ) 2.039 mol CaSO4 (5 mol H2SO4 ) ⋅ = ⋅ (2.039 mol CaSO4 2H2O) (172.17 g/mol) 351.1 g CaSO4 2H2O (1 mol HF) = (2.039 mol H2SO 4 ) 0.4078 mol HF (5 mol H2SO4 ) (0.4078 mol HF) (20.006 g/mol) = 8.158 g HF 18 Product Yields Example: Ca5(PO4)3F + 5 H2SO4 + 10 H2O → 3 H3PO4 + 5 CaSO4·2H2O + HF For each kg of Ca5(PO4)3F that reacts, 400.
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