Chemical Equations and StoichiometryChemical EquationsSlide 3Slide 4Slide 5Slide 6Slide 7Slide 8Slide 9Slide 10Slide 11Slide 12Slide 13Slide 14Slide 15Slide 16Slide 17Slide 18Slide 19Slide 20Slide 21Slide 22Slide 23Slide 24Slide 25Slide 26Slide 27Slide 28Slide 29Slide 30Slide 31Slide 32Slide 33Slide 34Slide 35Slide 36Slide 37Slide 38Slide 39Slide 40Slide 41Slide 42Slide 43Slide 44Slide 45Slide 46Slide 47Slide 48Slide 49Slide 50Slide 51Slide 52Slide 53Slide 54Chapter 4 1Chemical Equations and Chemical Equations and StoichiometryStoichiometryChapter 4Chapter 4Chapter 4 22H2(g) + O2(g)  2H2O(g)Chemical EquationsChemical EquationsChapter 4 32H2(g) + O2(g)  2H2O(g)•The materials you start with are called Reactants.Chemical EquationsChemical EquationsChapter 4 42H2(g) + O2(g)  2H2O(g)•The materials you start with are called Reactants.•The materials you make are called Products.Chemical EquationsChemical EquationsChapter 4 52H2(g) + O2(g)  2H2O(g)•The materials you start with are called Reactants.•The materials you make are called Products.•The numbers in front of the compounds (H2 and H2O) are called stoichiometric coefficients.–Coefficients are multipliers, in this equation 2 in front of the H2 indicates that there are 2 molecules of H2 in the equation.Chemical EquationsChemical EquationsChapter 4 62H2(g) + O2(g)  2H2O(g)•Notice that the number of hydrogen atoms and oxygen atoms on the reactant side and the product side is equal.Law of Conservation of Mass Matter cannot be created or lost in any chemical reaction.Chemical EquationsChemical EquationsChapter 4 7Balancing Chemical Reactions___NH4NO3(s)  ___N2O(g) + ___H2O(g)Chemical EquationsChemical EquationsChapter 4 8Balancing Chemical Reactions___NH4NO3(s)  ___N2O(g) + ___H2O(g)Chemical EquationsChemical EquationsReactants ProductsN 2 N 2H 4 H 2O 3 O 2Chapter 4 9Balancing Chemical Reactions___NH4NO3(s)  ___N2O(g) + _2_H2O(g)Chemical EquationsChemical EquationsReactants ProductsN 2 N 2H 4 H 2 4O 3 O 2 3Chapter 4 10Balancing Chemical Reactions___Mg3N2(s) + ___H2O(l)  ___Mg(OH)2(s) + ___NH3(aq)Chemical EquationsChemical EquationsReactants ProductsMg 3 Mg 1N 2 N 1H 2 H 5O 1 O 2Chapter 4 11Balancing Chemical Reactions___Mg3N2(s) + ___H2O(l)  _3_Mg(OH)2(s) + ___NH3(aq)Chemical EquationsChemical EquationsReactants ProductsMg 3 Mg 1 3N 2 N 1H 2 H 5 9O 1 O 2 6Chapter 4 12Balancing Chemical Reactions___Mg3N2(s) + ___H2O(l)  _3_Mg(OH)2(s) + _2_NH3(aq)Chemical EquationsChemical EquationsReactants ProductsMg 3 Mg 1 3N 2 N 1 2H 2 H 5 9 12O 1 O 2 6Chapter 4 13Balancing Chemical Reactions___Mg3N2(s) + _6_H2O(l)  _3_Mg(OH)2(s) + _2_NH3(aq)Chemical EquationsChemical EquationsReactants ProductsMg 3 Mg 1 3N 2 N 1 2H 2 12 H 5 9 12O 1 6 O 2 6Chapter 4 142 H2(g) + O2(g)  2 H2O(g)•The coefficients in a balanced equation represent both the number of molecules and the number of moles in a reaction.•The coefficients can also be used to derive ratios between any two substances in the chemical reaction.2 H2 : 1 O22 H2 : 2 H2O1 O2 : 2 H2OQuantitative InformationQuantitative Information•The ratios can be used to predict•The amount of product formed•The amount of reactant neededChapter 4 15Quantitative InformationQuantitative InformationChapter 4 16Quantitative InformationQuantitative Information 2 C4H10(l) + 13 O2(g)  8 CO2(g) + 10 H2O(g)How many grams of CO2 are formed if 1.00g of butane (C4H10) is allowed to react with excess oxygen?Chapter 4 17Quantitative InformationQuantitative Information 2 C4H10(l) + 13 O2(g)  8 CO2(g) + 10 H2O(g)How many grams of CO2 are formed if 1.00g of butane (C4H10) is allowed to react with excess oxygen?1. Moles of C4H10F.W. 58.124ggmolgHCmoles124.58100.1104Chapter 4 18Quantitative InformationQuantitative Information2 C4H10(l) + 13 O2(g)  8 CO2(g) + 10 H2O(g)How many grams of CO2 are formed if 1.00g of butane (C4H10) is allowed to react with excess oxygen?1. Moles of C4H10F.W. 58.124gmolgmolgHCmoles 0172.0124.58100.1104Chapter 4 19Quantitative InformationQuantitative Information 2 C4H10(l) + 13 O2(g)  8 CO2(g) + 10 H2O(g)How many grams of CO2 are formed if 1.00g of butane (C4H10) is allowed to react with excess oxygen?2. Ratio of C4H10:CO22 C4H10 : 8 CO2or104228HCCOChapter 4 20Quantitative InformationQuantitative Information2 C4H10(l) + 13 O2(g)  8 CO2(g) + 10 H2O(g)How many grams of CO2 are formed if 1.00g of butane (C4H10) is allowed to react with excess oxygen?3. Set-up ratio and proportion between known and unknown quantitiesChapter 4 21Quantitative InformationQuantitative Information2 C4H10(l) + 13 O2(g)  8 CO2(g) + 10 H2O(g)How many grams of CO2 are formed if 1.00g of butane (C4H10) is allowed to react with excess oxygen?3. Set-up ratio and proportion between known and unknown quantities10410420172.028HCmolxHCCOChapter 4 22Quantitative InformationQuantitative Information2 C4H10(l) + 13 O2(g)  8 CO2(g) + 10 H2O(g)How many grams of CO2 are formed if 1.00g of butane (C4H10) is allowed to react with excess oxygen?3. Set-up ratio and proportion between known and unknown quantities210410420688.00172.028COmolxHCmolxHCCOChapter 4 23Quantitative InformationQuantitative Information2 C4H10(l) + 13 O2(g)  8 CO2(g) + 10 H2O(g)How many grams of CO2 are formed if 1.00g of butane (C4H10) is allowed to react with excess oxygen?4. Convert the moles of unknown substance into the desired unitsChapter 4 24Quantitative InformationQuantitative Information2 C4H10(l) + 13 O2(g)  8 CO2(g) + 10 H2O(g)How many grams of CO2 are formed if 1.00g of butane (C4H10) is allowed to react with excess oxygen?4. Convert the moles of unknown substance into the desired unitsFW of CO2: 44.011g/mol  molgmolCOg /011.440688.02Chapter 4 25Quantitative InformationQuantitative Information2 C4H10(l) + 13 O2(g)  8 CO2(g) + 10 H2O(g)How many grams of CO2 are formed if 1.00g of butane (C4H10) is allowed to react with excess oxygen?4. Convert the moles of unknown substance into the desired unitsFW of CO2: 44.011g/mol gmolgmolCOg 03.3/011.440688.02Chapter 4 26“What runs out first”2 C8H18 + 25 O2  16 CO2 + 18 H2O•If you have 2 moles of C8H18 and 20 moles of O2all the O2 will be used and the reaction will stop•O2 is call the limiting reagent (reactant)Limiting Reactant – The reagent present in the smallest