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Essential Questions: What are the parts of a chemical equation? What is a catalyst? Word Equations: Methane (g) + Oxygen (g) [Yield to produce]Carbon dioxide (g) + Water (l) Reactants Product Phases: Gas (g) Liquid (1) Solid (s) Other symbols are used in equations. Catalyst: • Substance that speeds up a rxn. • Written above the • Not a reactant or a product Ex. H202(g) H20(1) + 02(g) Essential Question: How do you balance a chemical equation? Balancing Equations: 1. Determine correct formulas for reactants/products. 2. Balance each compound using oxidation numbers. 3. Balance each compound using coefficients. 4. Make sure coefficients are in the lowest ratio. Exs: A. Solid zinc reacts with a water solution of hydrogen sulfate to produce hydrogen gas, a water solution of zinc sulfate, and heat. Zinc(sy + hydrogen sulfate (g) hydrogen (g) + zinc sulfate (g) Zn(s) + H2SO4 (g) H2 (g) + Zn+1SO4 therefore is balanced. B. Calcium hydroxide + Sulfuric acid Calcium sulfate + Water. Balance each compound using coefficients. Calcium hydroxide + Sulfuric acidCalcium sulfate + water Ca (OH)2 + H2S04Ca (SO4) + H2O Using Rule #4: Inspect the three equations below. Are they balanced? 2 CH4 + 4O22CO2 + 4H2O 6 CH4 + 12O26CO2 + 12H2O 1/2 CH4 + O21/2 CO2 + H2O The first two are balanced but are they in the smallest whole-numbers ratio? (Rule 4) *NO, it should be CH4 + 2O2CO2 + 2H2O Essential Questions: What are the four types of reactions? What is general formula for each type? What is the relationship of Table J to writing equations? Types of Reactions: Combination (synthesis) Decomposition Single replacement Double replacement Synthesis: • Two or more reactants combine to form a single product • General Formula: A +BAB H +Cl HCl Na + Cl NaCl Decomposition: • Reverse of synthesis • A single compound is broken down (decomposed into two or more simpler substances) • General Formula: ABA + B Exs: 2 H2O2(1)2 H2O(1) + O2 2 NH3(g)N2(g) + 3 H2(g) Single Replacement Single replacement: Rxn, in which one element replaces another element in a compound. General formula: A + BCAC + B ** Use table J to determine if rxn will occur. Exs: Zn (s) + CuS04 ZnS04(g) + Cu(s) Mg + 2 HClH2 + MgCl2 Table J ** Use table J to determine if rxn will occur. • A reactive metal will replace any other metal below it. Exs: a. Zn + Cu(NO3)2Cu + ZnNO3)2 b. Cu + Zn(NO3)2no rxn c. F2 + NaCl Cl2 + NaF d. C12 + NaFno rxn Double Replacement: • Chemical change involving an exchange of positive ions between two compounds. (Between two ionic compounds) • Generally occur in an aqueous solution. • Often produces a gas, precipitate or a molecular compound. (H2O) • General formula: AB + CDAD + CB Exs. Ag(NO3)(aq)+ NaCl (aq)NaNO 3(aq)+ AgCl(s) Ba(N03)2(aq)+ Na2SO4(aq)BaSO4(s)+ 2 Na(NO3) (aq) Essential Question: What are the three types of situation in which a double replacement reaction will occur? Three situations in which a double replacement will occur: 1 . One product is a solid (precipitate) Table F AgNO3(aq) + NaCl (aq)AgCl(s) + NaNO3(aq) NaCl is a solid (insoluble) NaNO3 is a soluble therefore, rxn occurs. 2. A rxn in which a gas is produced NaS(g) + 2 HCl(aq)H2S(g) + 2 NaCl(aq) 3. A rxn in which a molecular substance is formed(H2O) NaOH (aq) + HCl (aq)H2O(l) + NaOH (aq) Essential Questions: What is a mole? What is Avogadro’s number? Mole: Is a specific number of particles 1 mole of any substance = 6.02 x1023particles (Avogadro’s number) **A mole of any substance contains Avogadro's number of particles (6.02 x l023) ** 1 mole of 1 mole of 1 mole of 1 mole of Ag = 6.02 x1023 atoms of Ag CO2 = 6.02 x1023 molecules of CO2 Ca ions = 6.02 x1023 ions N2 = 6.02 xl023 molecules of N2 Types of Mole Problems: Atoms -Moles Moles-Atoms Grams-Moles Moles-Grams Mole-Mole (equations) Mass—Mass (equations) Mass-Volume (equations) Volume-Volume (equations) # of Particles (equations) 1. Atoms-Mole: Ex. Magnesium is a light metal used in the manufacture of aircraft, automobile wheels, tools, and garden furniture. How many moles of magnesium are in 1.25x10 23 atoms of magnesium? a. List knows/unknowns: Known: Unknown: 1 mole Mg = 6.02x1023 atoms Mg # of moles of Mg # of atoms Mg = 1.25 x l023 atoms atoms Mgmoles Mg b. Solve problem: 1.25 xl 023 atoms Mg x 1 mole Mg 6.02xlO23atomsMg =1.25xl023x lmoleMg 6.02x1023 =2.08 x lO-1 mole Mg =.208 mole Mg B. How many moles are 2.08 x 1023 atoms of silicon? a. List known/unknown: Known: Unknown: 1 mole Si =6.02xl023 atoms moles of Si 2.80x1023= # of atoms Atoms Si mole Si b. Solve 2.80xl023 atoms Si x 1 mole Si 6.02x1023atoms Si =4.65 mole Si 2. MolesAtoms : How many atoms are in a mole of CO2? a. List known/unknown Known : Unknown: 1 mole CO2=6.02xl023 molecules #of atoms of CO2 CO2= 1 atom C 2 atoms O Therefore 3 atoms in CO2 b. Solve: 1 mole CO2 x 3(6.02x10 23 atoms CO2) 1 Mole CO2 =18.06xlO23atoms B. Propane is a gas used for cooking and heat. How many atoms are in 2.12 moles of propane (C3H8)? a. List Known/Unknown Known: Unknown: 2.12 moles of C3H8 atoms of C3H8 1 mole of C3H8 = 6.02x1023 molecules C3H8 (3C and 8H) 2.12moles C3H8 x 11(6.02 x 1023) 1mole C3H8 =1.4039 x l025 atoms C3H8 =1.40 x l025atoms C3H8 3. Grams Moles: Formula Mass- the sum of masses of all the atoms in a given formula Find the formula mass of O2 A. O2 = 2 atoms x 16amu=32 amu(formula mass) *1 mole of any substance = formula mass therefore, 1 mole of O2= 32g/mole B. Find the formula mass of CuSO4 Cu=l atom x 63.55amu=63.55amu S= 1 atom x 32.07amu= 32.07 amu O= 4 atom x 16amu = 64.00 amu 159.62 amu Gram Formula Mass- The formula mass expressed in grams. ** 1 mole of any substance= Formula mass Ex. How many moles are equivalent to 4.75g NaOH? a. Known Unknown 4.75g NaOH moles of NaOH b. Calculate GFM (gram formula mass) of NaOH Na=23amu O=16 amu H=l amu 40amu= 40g/mole NaOH C. Solve: 4.75g NaOH x 1 mole NaOH 40gNaOH =0.119 moles of NaOH 4. MolesGrams: Ex. How many grams are present in 40.5 moles of H2SO4? A. Known Unknown 40.5 moles H2SO4 # grams ofH2SO4 B Calculate GFM: H= 2amu x 2 =4 S= 32amu O= 16amu x 4 = 64 =98 amu= 98 g/mole Solve: 40.5 mole H2SO4 x 98gH2SO4 1 mole H2SO4 =3970g H2SO4 5. MoleMole a. In the equation N2 + 3H22NH3, how many moles of N2 are needed to produce 5.0 moles of NH3? Moles NH3 moles of N2 5.0 mole NH3 x 1 mole N2 2 Moles NH3 = 2.5 mole N2 b. In the equation 2NO + O2 2 NO2, How many moles of O2 are needed to produce 3.5 moles of NO2? Moles of NO2 Moles of O2 3.5 moles of NO2 x 1 mole O2 2 moles NO2 = 1.75 mole O2 Mole Mass: a. In the equation: 4Al +3O22 A12O3, how many grams of aluminum will combine with 1.50 moles of oxygen? Mole Grams 1.50 mole O2 x 4 mole Al x 27g Al 3 mole O2 1 mole Al =54 g Al b. Based on the previous equation, how many moles of O2 are needed to produce 51.0 g of Al2O3? GramsMoles 51 .O g A12O3 x 1 mole Al2O3 x 3 mole O2 102g Al2O3 2 moleAl2O3 =.75 mole O2 8. MassMass: a. In the equation, CH4 + 2 O2 2 H2O, how many grams of CO2 are formed when 8.0g of CH4 reacts with an excess of CO2? 8.0g CH4 x 1 mole CH4 x 1 mole CO2 x 44 g CO 16gCH4 1 mole CH4 1 mole CO2 = 22g C02 b. In the equation 2 H2O22H2O+ O2, how many grams of 02 will be formed from the decomposition of 17.0g of H2O2? 17.0g H2O2 x 1 mole H2O2 x 1 mole O2 x 32O2 34g H2O2 2 mole H2O2 1 mole O2 =8.0g O2 9. MassVolume: **1 mole of any substance = 22.4L(STP) a. In the equation: 2 CO (g) + O2 (g) 2 CO2 (g), how many liters of CO2, at STP are produced by the reaction of 64.0g of O2 (g) 64g O2 x 1 mole O2x 2 mole CO2_ x 22.4L CO2 32g O2 1 mole O2 1 mole CO2 = 89.6 L CO2 b. In the equation: 2 CO(g) + O2 (g) 2 CO2 (g) How many liters of O2 (g) at STP are able to react with 28.0g of CO(g)? 28.0gCO x 1 mole CO2 x 1 mole O2x 22.4L O2 28gCO 2 mole CO 1 moleO2 = 11.2 L O2 10. VolumeVolume: In the equation 4 NH3 (g) + 5 O2(g)4NO(g) + 6 H20(l). How many liters of NH3 (g) at STP are needed to react with 200 L of O2 (g) at STP? 2.0 L O2 x 1 mole O2 x 4 mole NH3 x 22.4 L NH3 22.4 L O2 5 mole O2 1 mole NH3 =160L NH3 b. In the equation: 4 NH3 (g) + 5 O2 (g) 4 NO(g) + 6 H2O(l) How many liters of NH3 (g) at STP are needed to produce 1000 L of NO(g) at STP? 1OOL NO x l mole NO x 4 mole NH3 x 22.4LNH3 22.4L NO 4 mole NO 1 mole NH3 = 1,OOOL NH3 Number of particles : a. In the equation: 2 C2H6+ 7 O2 4 CO2 + 6 H2O, how many molecules of C2H6 are needed to produce 27.Og of H2O? 27.0g H2O x 1 mole H2O x 2 mole C2H6 x 18gH2O 6moleH2O 6.02xl023 mole 1 mole C2H6 = 3.01xl023 molecules of C2H6 b. in the equation 2 C2H6 + 7 O2 4 CO2 + 6 H2O, how many molecules of CO2 are produced when 3.5 moles of O2 react? 3.5 mole O2 x 4 mole CO2 x 6.02x1023 molecules of CO2 7 mole O2 1 mole CO2 =12.04x 1023 molecules of C02 =1.204x 1024 molecules of C02 Limiting Reactant (regent)- a reactant that limits the amount of production of product formed in a reaction.