Fuels and Energy PDF

FUELS AND ENERGY Engr. Clint R. Mohammed, MBA Fuel Fuel – repositories of energy Fuel Fuel – repositories of energy storage Fuel Fuel – repositories of energy Fuel – provides energy such as: A.) Heating Fuel Fuel – repositories of energy Fuel – pro...

FUELS AND ENERGY Engr. Clint R. Mohammed, MBA Fuel Fuel – repositories of energy Fuel Fuel – repositories of energy storage Fuel Fuel – repositories of energy Fuel – provides energy such as: A.) Heating Fuel Fuel – repositories of energy Fuel – provides energy such as: A.) Heating B.) Transportation Fuel Fuel – repositories of energy Fuel – provides energy such as: A.) Heating B.) Transportation C.) Electrical generation Fuel Fuel – repositories of energy Fuel – provides energy such as: A.) Heating B.) Transportation C.) Electrical generation Fuel – substances that undergoes combustion and will produce energy in the form of heat Fuel Fuel – repositories of energy Fuel – provides energy such as: A.) Heating B.) Transportation C.) Electrical generation Fuel – substances that undergoes combustion and will produce energy in the form of heat Fuel – usually contains carbon and hydrogen propane CH3CH2CH3  octane CH3CH2CH2CH2CH2CH2CH2CH3 anthracene C14H10 Fuel Classification of Fuels: 1.) Solid Fuels A.) Coal -remains of plants millions of years ago Fuel Classification of Fuels: 1.) Solid Fuels A.) Coal -remains of plants millions of years ago B.) Coke -carbonization of coal Fuel Classification of Fuels: 1.) Solid Fuels A.) Coal -remains of plants millions of years ago B.) Coke -carbonization of coal heating at high temperature in the absence of air remove impurities Fuel Classification of Fuels: 1.) Solid Fuels A.) Coal -remains of plants millions of years ago B.) Coke -carbonization of coal C.) Peat -partially decomposed plant matter; usually in a water-saturated environment Fuel Classification of Fuels: 1.) Solid Fuels E.) Wood -fibrous substance consisting basically of xylem Fuel Classification of Fuels: 1.) Solid Fuels E.) Wood -fibrous substance consisting basically of xylem F.) Charcoal -product of wood distillation Fuel Classification of Fuels: 1.) Solid Fuels E.) Wood -fibrous substance consisting basically of xylem F.) Charcoal -product of wood distillation G.) Solid wastes and biomass -plant material and animal waste Fuel “torrefaction” Classification of Fuels: 1.) Solid Fuels drying E.) Wood -fibrous substance consisting basically of xylem F.) Charcoal -product of wood distillation G.) Solid wastes and biomass -plant material and animal waste Fuel Classification of Fuels: 2.) Liquid Fuels A.) Liquid petroleum fuels -made from fractional distillation of crude petroleum Distillation Column Fuel Classification of Fuels: 2.) Liquid Fuels B.) Nonpetroleum liquid fuels i.) Tar sands -mixture of mostly sand, clay, water, and bitumen Fuel Classification of Fuels: 2.) Liquid Fuels B.) Nonpetroleum liquid fuels i.) Tar sands -mixture of mostly sand, clay, water, and bitumen ii.) Oil shale -rock containing kerosene Fuel Classification of Fuels: 3.) Gaseous Fuels A.) Natural gas -combustible gas that occurs in porous rocks of the Earth’s crust -also found with or near accumulation of crude oil Fuel Classification of Fuels: 3.) Gaseous Fuels A.) Natural gas -combustible gas that occurs in porous rocks of the Earth’s crust -also found with or near accumulation of crude oil B.) Hydrogen gas -industrially made by (1) steam reforming of natural gas, (2) thermal cracking of hydrocarbon, or (3) electrolysis Steam Reforming: CH4 + 2H2O 4H2 + CO2 Thermal Cracking: Fuel Classification of Fuels: 3.) Gaseous Fuels C.) Acetylene -alkyne; ethyne -one process in producing is from calcium carbide  CaC2 + 2H2O C2H2 + Ca(OH)2 calcium water acetylene calcium carbide hydroxide ENERGY GENERATION OF FUELS Energy Generation of Fuels Chemical energy: energy present between atomic elements Energy Generation of Fuels Chemical energy: energy present between atomic elements chemical bonds Energy Generation of Fuels Chemical energy: energy present between atomic elements When bonds between atoms changes, the energy between them can either be absorbed or released Net Energy = Σ(energy from bond breakage) - Σ(energy from bond formation) Energy Generation of Fuels CH4(g) + 2O2(g) CO2(g) + 2H2O(l) H O O H O H H C H O C O O O H O H H C-H : 410 kJ/mol O=O : 494 kJ/mol C=O : 799 kJ/mol H-O : 460 kJ/mol Net = Σ(energy from bond breakage) - Σ(energy from bond formation) Energy Net = Energy Energy Generation of Fuels CH4(g) + 2O2(g) CO2(g) + 2H2O(l) H O O H O H H C H O C O O O H O H H C-H : 410 kJ/mol O=O : 494 kJ/mol C=O : 799 kJ/mol H-O : 460 kJ/mol Net = Σ(energy from bond breakage) - Σ(energy from bond formation) Energy Net = Σ(4 C-H bonds + 2 O=O bonds) Energy Energy Generation of Fuels CH4(g) + 2O2(g) CO2(g) + 2H2O(l) H O O H O H H C H O C O O O H O H H C-H : 410 kJ/mol O=O : 494 kJ/mol C=O : 799 kJ/mol H-O : 460 kJ/mol Net = Σ(energy from bond breakage) - Σ(energy from bond formation) Energy Net = Σ(4 C-H bonds + 2 O=O bonds) Energy Energy Generation of Fuels CH4(g) + 2O2(g) CO2(g) + 2H2O(l) H O O H O H H C H O C O O O H O H H C-H : 410 kJ/mol O=O : 494 kJ/mol C=O : 799 kJ/mol H-O : 460 kJ/mol Net = Σ(energy from bond breakage) - Σ(energy from bond formation) Energy Net = Σ(4 C-H bonds + 2 O=O bonds) - Σ(2 C=O bonds + 4 H-O bonds) Energy Energy Generation of Fuels CH4(g) + 2O2(g) CO2(g) + 2H2O(l) H O O H O H H C H O C O O O H O H H C-H : 410 kJ/mol O=O : 494 kJ/mol C=O : 799 kJ/mol H-O : 460 kJ/mol Net = Σ(energy from bond breakage) - Σ(energy from bond formation) Energy Net = Σ(4 C-H bonds + 2 O=O bonds) - Σ(2 C=O bonds + 4 H-O bonds) Energy Energy Generation of Fuels CH4(g) + 2O2(g) CO2(g) + 2H2O(l) H O O H O H H C H O C O O O H O H H C-H : 410 kJ/mol O=O : 494 kJ/mol C=O : 799 kJ/mol H-O : 460 kJ/mol Net = Σ(energy from bond breakage) - Σ(energy from bond formation) Energy Net = Σ(4 C-H bonds + 2 O=O bonds) - Σ(2 C=O bonds + 4 H-O bonds) Energy Net Energy = Generation Σ(4 C-H bonds +of Fuels 2 O=O bonds) - Σ(2 C=O bonds + 4 H-O bonds) Energy CH4(g) + 2O2(g) CO2(g) + 2H2O(l) Net EnergyH [ = Σ (4 mol) O O H O H H C H O O H O H H C-H : 410 kJ/mol O=O : 494 kJ/mol C=O : 799 kJ/mol H-O : 460 kJ/mol Net = Σ(energy from bond breakage) - Σ(energy from bond formation) Energy Net = Σ(4 C-H bonds + 2 O=O bonds) - Σ(2 C=O bonds + 4 H-O bonds) Energy Net Energy = Generation Σ(4 C-H bonds +of Fuels 2 O=O bonds) - Σ(2 C=O bonds + 4 H-O bonds) Energy CH4(g) + 2O2(g) CO2(g) + 2H2O(l) Net EnergyH [ = Σ (4 mol) 410 kJ 1 mol O O H O H H C H O O H O H C-H : 410 kJ/mol O=O : 494 kJ/mol C=O : 799 kJ/mol H-O : 460 kJ/mol Net = Σ(energy from bond breakage) - Σ(energy from bond formation) Energy Net = Σ(4 C-H bonds + 2 O=O bonds) - Σ(2 C=O bonds + 4 H-O bonds) Energy Net Energy = Generation Σ(4 C-H bonds +of Fuels 2 O=O bonds) - Σ(2 C=O bonds + 4 H-O bonds) Energy CH4(g) + 2O2(g) CO2(g) + 2H2O(l) [ Net EnergyH [ = Σ (4 mol) 410 kJ + (2 mol) 494 kJ 1 mol 1 mol O O H O H H C H O O H O H H C-H : 410 kJ/mol O=O : 494 kJ/mol C=O : 799 kJ/mol H-O : 460 kJ/mol Net = Σ(energy from bond breakage) - Σ(energy from bond formation) Energy Net = Σ(4 C-H bonds + 2 O=O bonds) - Σ(2 C=O bonds + 4 H-O bonds) Energy Net Energy = Generation Σ(4 C-H bonds +of Fuels 2 O=O bonds) - Σ(2 C=O bonds + 4 H-O bonds) Energy CH4(g) + 2O2(g) CO2(g) + 2H2O(l) [ Net EnergyH [ = Σ (4 mol) 410 kJ + (2 mol) 494 kJ 1 mol 1 mol O O H O H H C H [ - Σ (2 mol) 799 kJ O 1Cmol O O O H O H H C-H : 410 kJ/mol O=O : 494 kJ/mol C=O : 799 kJ/mol H-O : 460 kJ/mol Net = Σ(energy from bond breakage) - Σ(energy from bond formation) Energy Net = Σ(4 C-H bonds + 2 O=O bonds) - Σ(2 C=O bonds + 4 H-O bonds) Energy Net Energy = Generation Σ(4 C-H bonds +of Fuels 2 O=O bonds) - Σ(2 C=O bonds + 4 H-O bonds) Energy CH4(g) + 2O2(g) CO2(g) + 2H2O(l) [ Net EnergyH [ = Σ (4 mol) 410 kJ + (2 mol) 494 kJ 1 mol 1 mol O O H O H [ H C H [ - Σ (2 mol) 799 kJ + (4 mol) 460 kJ O 1Cmol O 1 mol O O H O H H C-H : 410 kJ/mol O=O : 494 kJ/mol C=O : 799 kJ/mol H-O : 460 kJ/mol Net = Σ(energy from bond breakage) - Σ(energy from bond formation) Energy Net = Σ(4 C-H bonds + 2 O=O bonds) - Σ(2 C=O bonds + 4 H-O bonds) Energy Net Energy = Generation Σ(4 C-H bonds +of Fuels 2 O=O bonds) - Σ(2 C=O bonds + 4 H-O bonds) Energy CH4(g) + 2O2(g) CO2(g) + 2H2O(l) [ Net EnergyH [ = Σ (4 mol) 410 kJ + (2 mol) 494 kJ 1 mol 1 mol O O H O H [ H C H Net [ - Σ (2 mol) 799 kJ + (4 mol) 460 kJ O 1Cmol O 1 mol EnergyH = -810 kJ O O H O H C-H : 410 kJ/mol O=O : 494 kJ/mol C=O : 799 kJ/mol H-O : 460 kJ/mol Net = Σ(energy from bond breakage) - Σ(energy from bond formation) Energy Net = Σ(4 C-H bonds + 2 O=O bonds) - Σ(2 C=O bonds + 4 H-O bonds) Energy APPLICATION OF STOICHIOMETRY IN COMBUSTION REACTIONS Application of Stoichiometry in Combustion Reactions Combustion: reaction of a material with oxygen to produce oxides Combustion: commonly known as “burning” Combustion: release of energy Fuel w/ + O2(g) CO2(g) + H2O(l) carbon atom/s C3H8(g) + 5O2(g) 3CO2(g) + 4H2O(l) 2C4H8(g) + 13O2(g) 8CO2(g) + 10H2O(l) Application of Stoichiometry in Combustion Reactions Law of Conservation of Mass 100 g total 100 g total Fuel w/ + O2(g) CO2(g) + H2O(l) carbon atom/s C3H8(g) + 5O2(g) 3CO2(g) + 4H2O(l) 2C4H8(g) + 13O2(g) 8CO2(g) + 10H2O(l) Application of Stoichiometry in Combustion Reactions x mol total x=y y mol total Fuel w/ + O2(g) CO2(g) + H2O(l) carbon atom/s C3H8(g) + 5O2(g) 3CO2(g) + 4H2O(l) 2C4H8(g) + 13O2(g) 8CO2(g) + 10H2O(l) Application of Stoichiometry in Combustion Reactions 1.) What mass of carbon dioxide is produced when 105 g of methane burns completely in air? Given: Req’d: 105 g CH4 mCO2 Sol’n: CH4(g) + O2(g) CO2(g) + H2O(l) Last to balance: O Second to the last to balance: H Application of Stoichiometry in Combustion Reactions 1.) What mass of carbon dioxide is produced when 105 g of methane burns completely in air? Given: Req’d: 105 g CH4 mCO2 Sol’n: CH4(g) + O2(g) CO2(g) + H2O(l) Last to balance: O Second to the last to balance: H Application of Stoichiometry in Combustion Reactions 1.) What mass of carbon dioxide is produced when 105 g of methane burns completely in air? Given: Req’d: 105 g CH4 mCO2 Sol’n: CH4(g) + O2(g) CO2(g) + H2O(l) Last to balance: O Second to the last to balance: H Application of Stoichiometry in Combustion Reactions 1.) What mass of carbon dioxide is produced when 105 g of methane burns completely in air? Given: Req’d: 105 g CH4 mCO2 Sol’n: CH4(g) + O2(g) CO2(g) + H2O(l) Last to balance: O Second to the last to balance: H Application of Stoichiometry in Combustion Reactions 1.) What mass of carbon dioxide is produced when 105 g of methane burns completely in air? Given: Req’d: 105 g CH4 mCO2 Sol’n: CH4(g) + O2(g) CO2(g) + H2O(l) Last to balance: O Second to the last to balance: H Application of Stoichiometry in Combustion Reactions 1.) What mass of carbon dioxide is produced when 105 g of methane burns completely in air? Given: Req’d: 105 g CH4 mCO2 Sol’n: CH4(g) + O2(g) CO2(g) + 2H2O(l) Last to balance: O Second to the last to balance: H Application of Stoichiometry in Combustion Reactions 1.) What mass of carbon dioxide is produced when 105 g of methane burns completely in air? Given: Req’d: 105 g CH4 mCO2 4O Sol’n: CH4(g) + O2(g) CO2(g) + 2H2O(l) Last to balance: O Second to the last to balance: H Application of Stoichiometry in Combustion Reactions 1.) What mass of carbon dioxide is produced when 105 g of methane burns completely in air? Given: Req’d: 105 g CH4 mCO2 4O Sol’n: CH4(g) + 2O2(g) CO2(g) + 2H2O(l) Last to balance: O Second to the last to balance: H Application of Stoichiometry in Combustion Reactions 1.) What mass of carbon dioxide is produced when 105 g of methane burns completely in air? Given: Req’d: 105 g CH4 m mass mole mole mass CO2 MW SR MW Sol’n: CH4(g) + 2O2(g) CO2(g) + 2H2O(l) 16 g/mol 44 g/mol Application of Stoichiometry in Combustion Reactions 1.) What mass of carbon dioxide is produced when 105 g of methane burns completely in air? Given: Req’d: 105 g CH4 m mass mole mole mass CO2 MW SR MW Sol’n: CH4(g) + 2O2(g) CO2(g) + 2H2O(l) 16 g/mol 44 g/mol Application of Stoichiometry in Combustion Reactions 1.) What mass of carbon dioxide is produced when 105 g of methane burns completely in air? Given: Req’d: 105 g CH4 m mass mole mole mass CO2 MW SR MW Sol’n: CH4(g) + 2O2(g) CO2(g) + 2H2O(l) 16 g/mol 44 g/mol (105 g CH4) Application of Stoichiometry in Combustion Reactions 1.) What mass of carbon dioxide is produced when 105 g of methane burns completely in air? Given: Req’d: 105 g CH4 m mass mole mole mass CO2 MW SR MW Sol’n: CH4(g) + 2O2(g) CO2(g) + 2H2O(l) 16 g/mol 44 g/mol (105 g CH4) Application of Stoichiometry in Combustion Reactions 1.) What mass of carbon dioxide is produced when 105 g of methane burns completely in air? Given: Req’d: 105 g CH4 m mass mole mole mass CO2 MW SR MW Sol’n: CH4(g) + 2O2(g) CO2(g) + 2H2O(l) 16 g/mol 44 g/mol (105 g CH4) Application of Stoichiometry in Combustion Reactions 1.) What mass of carbon dioxide is produced when 105 g of methane burns completely in air? Given: Req’d: 105 g CH4 m mass mole mole mass CO2 MW SR MW Sol’n: CH4(g) + 2O2(g) CO2(g) + 2H2O(l) 16 g/mol 44 g/mol ( ( (105 g CH4) 1 mol CH4 16 g CH4 MW Application of Stoichiometry in Combustion Reactions 1.) What mass of carbon dioxide is produced when 105 g of methane burns completely in air? Given: Req’d: 105 g CH4 m mass mole mole mass CO2 MW SR MW Sol’n: CH4(g) + 2O2(g) CO2(g) + 2H2O(l) 16 g/mol 44 g/mol ( ( (105 g CH4) 1 mol CH4 16 g CH4 MW Application of Stoichiometry in Combustion Reactions 1.) What mass of carbon dioxide is produced when 105 g of methane burns completely in air? Given: Req’d: 105 g CH4 m mass mole mole mass CO2 MW SR MW Sol’n: CH4(g) + 2O2(g) CO2(g) + 2H2O(l) 16 g/mol 44 g/mol ( ( (105 g CH4) 1 mol CH4 16 g CH4 MW Application of Stoichiometry in Combustion Reactions 1.) What mass of carbon dioxide is produced when 105 g of methane burns completely in air? Given: Req’d: 105 g CH4 m mass mole mole mass CO2 MW SR MW Sol’n: CH4(g) + 2O2(g) CO2(g) + 2H2O(l) 16 g/mol 44 g/mol ( ( (105 g CH4) 1 mol CH4 16 g CH4 MW Application of Stoichiometry in Combustion Reactions 1.) What mass of carbon dioxide is produced when 105 g of methane burns completely in air? Given: Req’d: 105 g CH4 m mass mole mole mass CO2 MW SR MW Sol’n: CH4(g) + 2O2(g) CO2(g) + 2H2O(l) 16 g/mol 44 g/mol ( ( ( ( (105 g CH4) 1 mol CH4 1 mol CO2 16 g CH4 1 mol CH4 MW stoichiometric ratio Application of Stoichiometry in Combustion Reactions 1.) What mass of carbon dioxide is produced when 105 g of methane burns completely in air? Given: Req’d: 105 g CH4 m mass mole mole mass CO2 MW SR MW Sol’n: CH4(g) + 2O2(g) CO2(g) + 2H2O(l) 16 g/mol 44 g/mol ( ( ( ( (105 g CH4) 1 mol CH4 1 mol CO2 16 g CH4 1 mol CH4 MW stoichiometric ratio Application of Stoichiometry in Combustion Reactions 1.) What mass of carbon dioxide is produced when 105 g of methane burns completely in air? Given: Req’d: 105 g CH4 m mass mole mole mass CO2 MW SR MW Sol’n: CH4(g) + 2O2(g) CO2(g) + 2H2O(l) 16 g/mol 44 g/mol ( ( ( ( (105 g CH4) 1 mol CH4 1 mol CO2 16 g CH4 1 mol CH4 MW stoichiometric ratio Application of Stoichiometry in Combustion Reactions 1.) What mass of carbon dioxide is produced when 105 g of methane burns completely in air? Given: Req’d: 105 g CH4 m mass mole mole mass CO2 MW SR MW Sol’n: CH4(g) + 2O2(g) CO2(g) + 2H2O(l) 16 g/mol 44 g/mol ( ( ( ( ( ( (105 g CH4) 1 mol CH4 1 mol CO2 44 g CO2 16 g CH4 1 mol CH4 1 mol CO2 MW stoichiometric ratio MW Application of Stoichiometry in Combustion Reactions 1.) What mass of carbon dioxide is produced when 105 g of methane burns completely in air? Given: Req’d: 105 g CH4 m mass mole mole mass CO2 MW SR MW Sol’n: CH4(g) + 2O2(g) CO2(g) + 2H2O(l) 16 g/mol 44 g/mol ( ( ( ( ( ( (105 g CH4) 1 mol CH4 1 mol CO2 44 g CO2 16 g CH4 1 mol CH4 1 mol CO2 mCO2 = 288.75 g MW stoichiometric ratio MW Application of Stoichiometry in Combustion Reactions 2.) How many grams of ethanol is needed to produce 150 g of water when it is subjected to complete combustion? Given: Req’d: 150 g H2O mEtOH Sol’n: C2H5OH(l) + 3O2(g) 2CO2(g) + 3H2O(l) Last to balance: O Second to the last to balance: H Application of Stoichiometry in Combustion Reactions 2.) How many grams of ethanol is needed to produce 150 g of water when it is subjected to complete combustion? Given: Req’d: 150 g H2O mEtOH Sol’n: C2H5OH(l) + 3O2(g) 2CO2(g) + 3H2O(l) Last to balance: O Second to the last to balance: H Application of Stoichiometry in Combustion Reactions 2.) How many grams of ethanol is needed to produce 150 g of water when it is subjected to complete combustion? Given: Req’d: 150 g H2O mEtOH Sol’n: C2H5OH(l) + 3O2(g) 2CO2(g) + 3H2O(l) Last to balance: O Second to the last to balance: H Application of Stoichiometry in Combustion Reactions 2.) How many grams of ethanol is needed to produce 150 g of water when it is subjected to complete combustion? Given: Req’d: 150 g H2O mEtOH Sol’n: C2H5OH(l) + 3O2(g) 2CO2(g) + 3H2O(l) Last to balance: O Second to the last to balance: H Application of Stoichiometry in Combustion Reactions 2.) How many grams of ethanol is needed to produce 150 g of water when it is subjected to complete combustion? Given: Req’d: 150 g H2O mEtOH Sol’n: C2H5OH(l) + 3O2(g) 2CO2(g) + 3H2O(l) Last to balance: O Second to the last to balance: H Application of Stoichiometry in Combustion Reactions 2.) How many grams of ethanol is needed to produce 150 g of water when it is subjected to complete combustion? Given: Req’d: 150 g H2O mEtOH Sol’n: C2H5OH(l) + 3O2(g) 2CO2(g) + 3H2O(l) Last to balance: O Second to the last to balance: H Application of Stoichiometry in Combustion Reactions 2.) How many grams of ethanol is needed to produce 150 g of water when it is subjected to complete combustion? Given: Req’d: 150 g H2O mEtOH Sol’n: C2H5OH(l) + 3O2(g) 2CO2(g) + 3H2O(l) Last to balance: O Second to the last to balance: H Application of Stoichiometry in Combustion Reactions 2.) How many grams of ethanol is needed to produce 150 g of water when it is subjected to complete combustion? Given: Req’d: 150 g H2O mEtOH 3O Sol’n: C2H5OH(l) + 3O2(g) 2CO2(g) + 3H2O(l) Last to balance: O Second to the last to balance: H Application of Stoichiometry in Combustion Reactions 2.) How many grams of ethanol is needed to produce 150 g of water when it is subjected to complete combustion? Given: Req’d: 150 g H2O mEtOH 3O 7O Sol’n: C2H5OH(l) + 3O2(g) 2CO2(g) + 3H2O(l) Last to balance: O Second to the last to balance: H Application of Stoichiometry in Combustion Reactions 2.) How many grams of ethanol is needed to produce 150 g of water when it is subjected to complete combustion? Given: Req’d: 150 g H2O mEtOH 1O 7O Sol’n: C2H5OH(l) + 3O2(g) 2CO2(g) + 3H2O(l) Last to balance: O Second to the last to balance: H Application of Stoichiometry in Combustion Reactions 2.) How many grams of ethanol is needed to produce 150 g of water when it is subjected to complete combustion? Given: Req’d: 150 g H2O mEtOH 1O 7O Sol’n: C2H5OH(l) + 3O2(g) 2CO2(g) + 3H2O(l) Last to balance: O Second to the last to balance: H Application of Stoichiometry in Combustion Reactions 2.) How many grams of ethanol is needed to produce 150 g of water when it is subjected to complete combustion? Given: Req’d: 150 g H2O m mass mole mole mass EtOH MW SR MW Sol’n: C2H5OH(l) + 3O2(g) 2CO2(g) + 3H2O(l) 46 g/mol 18 g/mol Application of Stoichiometry in Combustion Reactions 2.) How many grams of ethanol is needed to produce 150 g of water when it is subjected to complete combustion? Given: Req’d: 150 g H2O m mass mole mole mass EtOH MW SR MW Sol’n: C2H5OH(l) + 3O2(g) 2CO2(g) + 3H2O(l) 46 g/mol 18 g/mol Application of Stoichiometry in Combustion Reactions 2.) How many grams of ethanol is needed to produce 150 g of water when it is subjected to complete combustion? Given: Req’d: 150 g H2O m mass mole mole mass EtOH MW SR MW Sol’n: C2H5OH(l) + 3O2(g) 2CO2(g) + 3H2O(l) 46 g/mol 18 g/mol (150 g H2O) Application of Stoichiometry in Combustion Reactions 2.) How many grams of ethanol is needed to produce 150 g of water when it is subjected to complete combustion? Given: Req’d: 150 g H2O m mass mole mole mass EtOH MW SR MW Sol’n: C2H5OH(l) + 3O2(g) 2CO2(g) + 3H2O(l) 46 g/mol 18 g/mol (150 g H2O) Application of Stoichiometry in Combustion Reactions 2.) How many grams of ethanol is needed to produce 150 g of water when it is subjected to complete combustion? Given: Req’d: 150 g H2O m mass mole mole mass EtOH MW SR MW Sol’n: C2H5OH(l) + 3O2(g) 2CO2(g) + 3H2O(l) 46 g/mol 18 g/mol (150 g H2O) Application of Stoichiometry in Combustion Reactions 2.) How many grams of ethanol is needed to produce 150 g of water when it is subjected to complete combustion? Given: Req’d: 150 g H2O m mass mole mole mass EtOH MW SR MW Sol’n: C2H5OH(l) + 3O2(g) 2CO2(g) + 3H2O(l) 46 g/mol 18 g/mol ( ( (150 g H2O) 1 mol H2O 18 g H2O MW Application of Stoichiometry in Combustion Reactions 2.) How many grams of ethanol is needed to produce 150 g of water when it is subjected to complete combustion? Given: Req’d: 150 g H2O m mass mole mole mass EtOH MW SR MW Sol’n: C2H5OH(l) + 3O2(g) 2CO2(g) + 3H2O(l) 46 g/mol 18 g/mol ( ( (150 g H2O) 1 mol H2O 18 g H2O MW Application of Stoichiometry in Combustion Reactions 2.) How many grams of ethanol is needed to produce 150 g of water when it is subjected to complete combustion? Given: Req’d: 150 g H2O m mass mole mole mass EtOH MW SR MW Sol’n: C2H5OH(l) + 3O2(g) 2CO2(g) + 3H2O(l) 46 g/mol 18 g/mol ( ( ( ( (150 g H2O) 1 mol H2O 1 mol EtOH 18 g H2O 3 mol H2O MW stoichiometric ratio Application of Stoichiometry in Combustion Reactions 2.) How many grams of ethanol is needed to produce 150 g of water when it is subjected to complete combustion? Given: Req’d: 150 g H2O m mass mole mole mass EtOH MW SR MW Sol’n: C2H5OH(l) + 3O2(g) 2CO2(g) + 3H2O(l) 46 g/mol 18 g/mol ( ( ( ( (150 g H2O) 1 mol H2O 1 mol EtOH 18 g H2O 3 mol H2O MW stoichiometric ratio Application of Stoichiometry in Combustion Reactions 2.) How many grams of ethanol is needed to produce 150 g of water when it is subjected to complete combustion? Given: Req’d: 150 g H2O m mass mole mole mass EtOH MW SR MW Sol’n: C2H5OH(l) + 3O2(g) 2CO2(g) + 3H2O(l) 46 g/mol 18 g/mol ( ( ( ( (150 g H2O) 1 mol H2O 1 mol EtOH 18 g H2O 3 mol H2O MW stoichiometric ratio Application of Stoichiometry in Combustion Reactions 2.) How many grams of ethanol is needed to produce 150 g of water when it is subjected to complete combustion? Given: Req’d: 150 g H2O m mass mole mole mass EtOH MW SR MW Sol’n: C2H5OH(l) + 3O2(g) 2CO2(g) + 3H2O(l) 46 g/mol 18 g/mol ( ( ( ( ( (150 g H2O) 1 mol H2O 1 mol EtOH 18 g H2O 3 mol H2O ( 46 g EtOH 1 mol EtOH MW stoichiometric ratio MW Application of Stoichiometry in Combustion Reactions 2.) How many grams of ethanol is needed to produce 150 g of water when it is subjected to complete combustion? Given: Req’d: 150 g H2O m mass mole mole mass EtOH MW SR MW Sol’n: C2H5OH(l) + 3O2(g) 2CO2(g) + 3H2O(l) 46 g/mol 18 g/mol ( ( ( ( ( (150 g H2O) 1 mol H2O 1 mol EtOH 18 g H2O 3 mol H2O ( 46 g EtOH 1 mol EtOH mEtOH = 127.78 g MW stoichiometric ratio MW Application of Stoichiometry in Combustion Reactions 3.) How many grams of carbon dioxide is produced if 10 grams of butane burns with 10 grams of oxygen? Given: Sol’n: 10 g C4H10 2C4H10(l) + 13O2(g) 8CO2(g) + 10H2O(l) 10 g O2 Req’d: mCO2 Application of Stoichiometry in Combustion Reactions 3.) How many grams of carbon dioxide is produced if 10 grams of butane burns with 10 grams of oxygen? Given: Sol’n: 10 g C4H10 2C4H10(l) + 13O2(g) 8CO2(g) + 10H2O(l) 10 g O2 Req’d: mCO2 Application of Stoichiometry in Combustion Reactions 3.) How many grams of carbon dioxide is produced if 10 grams of butane burns with 10 grams of oxygen? Given: Sol’n: 10 g C4H10 2C4H10(l) + 13O2(g) 8CO2(g) + 10H2O(l) 10 g O2 Req’d: mCO2 Application of Stoichiometry in Combustion Reactions 3.) How many grams of carbon dioxide is produced if 10 grams of butane burns with 10 grams of oxygen? Given: Sol’n: 10 g C4H10 2C4H10(l) + 13O2(g) 4CO2(g) + 10H2O(l) 10 g O2 Req’d: mCO2 Application of Stoichiometry in Combustion Reactions 3.) How many grams of carbon dioxide is produced if 10 grams of butane burns with 10 grams of oxygen? Given: Sol’n: 10 g C4H10 2C4H10(l) + 13O2(g) 4CO2(g) + 10H2O(l) 10 g O2 Req’d: mCO2 Application of Stoichiometry in Combustion Reactions 3.) How many grams of carbon dioxide is produced if 10 grams of butane burns with 10 grams of oxygen? Given: Sol’n: 10 g C4H10 2C4H10(l) + 13O2(g) 4CO2(g) + 10H2O(l) 10 g O2 Req’d: mCO2 Application of Stoichiometry in Combustion Reactions 3.) How many grams of carbon dioxide is produced if 10 grams of butane burns with 10 grams of oxygen? Given: Sol’n: 10 g C4H10 2C4H10(l) + 13O2(g) 4CO2(g) + 15H2O(l) 10 g O2 Req’d: mCO2 Application of Stoichiometry in Combustion Reactions 3.) How many grams of carbon dioxide is produced if 10 grams of butane burns with 10 grams of oxygen? Given: Sol’n: 10 g C4H10 2C4H10(l) + 1313O2(g) 4CO2(g) + 15H2O(l) 10 g O2 2 Req’d: 13 O mCO2 Application of Stoichiometry in Combustion Reactions 3.) How many grams of carbon dioxide is produced if 10 grams of butane burns with 10 grams of oxygen? Given: Sol’n: 10 g C4H10 2 2C4H10(l) + 13 [ 10 g O2 [ 13O2(g) 2 4CO2(g) + 15H2O(l) Req’d: mCO2 Application of Stoichiometry in Combustion Reactions 3.) How many grams of carbon dioxide is produced if 10 grams of butane burns with 10 grams of oxygen? Given: Sol’n: 10 g C4H10 2C4H10(l) + 1313O2(g) 8CO2(g) + 10H2O(l) 10 g O2 Req’d: mCO2 Application of Stoichiometry in Combustion Reactions 3.) How many grams of carbon dioxide is produced if 10 grams of butane burns with 10 grams of oxygen? Given: Sol’n: 10 g C4H10 2C4H10(l) + 1313O2(g) 8CO2(g) + 10H2O(l) 10 g O2 10 g 10 g Req’d: 58 g/mol 32 g/mol mCO2 Limiting and Excess Application of Stoichiometry in Combustion Reactions 3.) How many grams of carbon dioxide is produced if 10 grams of butane burns with 10 grams of oxygen? Given: Sol’n: 10 g C4H10 2C4H10(l) + 1313O2(g) 8CO2(g) + 10H2O(l) 10 g O2 10 g 10 g Req’d: 58 g/mol 32 g/mol mCO2 Limiting and Excess Application of Stoichiometry in Combustion Reactions 3.) How many grams of carbon dioxide is produced if 10 grams of butane burns with 10 grams of oxygen? Given: Sol’n: 10 g C4H10 2C4H10(l) + 1313O2(g) 8CO2(g) + 10H2O(l) 10 g O2 10 g 10 g Req’d: 58 g/mol 32 g/mol 44 g/mol mCO2 Limiting and Excess Application of Stoichiometry in Combustion Reactions 3.) How many grams of carbon dioxide is produced if 10 grams of butane burns with 10 grams of oxygen? Given: Sol’n: 10 g C4H10 2C4H10(l) + 13 13O2(g) 8CO2(g) + 10H2O(l) 10 g O2 10 g 10 g Req’d: 58 g/mol 32 g/mol 44 g/mol mCO2 for C4H10: ( ( ( ( (10 g C4H10) 1 mol C4H10 8 mol CO2 = 0.6897 mol CO 58 g C4H10 2 mol C4H10 2 Application of Stoichiometry in Combustion Reactions 3.) How many grams of carbon dioxide is produced if 10 grams of butane burns with 10 grams of oxygen? Given: Sol’n: 10 g C4H10 2C4H10(l) + 13 13O2(g) 8CO2(g) + 10H2O(l) 10 g O2 10 g 10 g Req’d: 58 g/mol 32 g/mol 44 g/mol mCO2 for C4H10: ( ( for O2: ( ( (10 g C4H10) 1 mol C4H10 8 mol CO2 = 0.6897 mol CO 58 g C4H10 2 mol C4H10 2 ( ( ( 32 g O2( (10 g O2) 1 mol O2 8 mol CO2 = 0.1923 mol CO 13 mol O2 2 Application of Stoichiometry in Combustion Reactions 3.) How many grams of carbon dioxide is produced if 10 grams of butane burns with 10 grams of oxygen? Given: Sol’n: 10 g C4H10 2C4H10(l) + 13 13O2(g) 8CO2(g) + 10H2O(l) 10 g O2 10 g 10 g Req’d: 58 g/mol 32 g/mol 44 g/mol mCO2 for C4H10: ( ( for O2: ( ( (10 g C4H10) 1 mol C4H10 8 mol CO2 = 0.6897 mol CO 58 g C4H10 2 mol C4H10 2 ( ( ( 32 g O2( (10 g O2) 1 mol O2 8 mol CO2 = 0.1923 mol CO 13 mol O2 2 Application of Stoichiometry in Combustion Reactions 3.) How many grams of carbon dioxide is produced if 10 grams of butane burns with 10 grams of oxygen? Given: Sol’n: 10 g C4H10 2C4H10(l) + 1313O2(g) 8CO2(g) + 10H2O(l) 10 g O2 Req’d: 44 g/mol mCO2 for O2: ( ( ( (10 g O2) 1 mol O2 32 g O2 ( 8 mol CO2 13 mol O2 = 0.1923 mol CO2 Application of Stoichiometry in Combustion Reactions 3.) How many grams of carbon dioxide is produced if 10 grams of butane burns with 10 grams of oxygen? Given: Sol’n: 10 g C4H10 2C4H10(l) + 1313O2(g) 8CO2(g) + 10H2O(l) 10 g O2 Excess Limiting Req’d: Reactant Reactant 44 g/mol mCO2 for O2: ( ( ( (10 g O2) 1 mol O2 32 g O2 ( 8 mol CO2 13 mol O2 = 0.1923 mol CO2 Application of Stoichiometry in Combustion Reactions 3.) How many grams of carbon dioxide is produced if 10 grams of butane burns with 10 grams of oxygen? Given: Sol’n: 10 g C4H10 2C4H10(l) + 1313O2(g) 8CO2(g) + 10H2O(l) 10 g O2 Excess Limiting 8.46 g Req’d: Reactant Reactant 44 g/mol mCO2 ( ( ( 32 g O2 ( (10 g O2) 1 mol O2 8 mol CO2 = 0.1923 mol CO 13 mol O2 2 ( ( (0.1923 mol CO2) 44 g CO2 1 mol CO2 = 8.46 g CO2 Application of Stoichiometry in Combustion Reactions 4.) How many grams of carbon dioxide and water is produced if 10 grams of butane burns with 10 grams of oxygen? Given: Sol’n: 10 g C4H10 2C4H10(l) + 13 13O2(g) 8CO2(g) + 10H2O(l) 10 g O2 Excess Limiting Req’d: Reactant Reactant 44 g/mol mH2O ( ( ( 32 g O2 ( (10 g O2) 1 mol O2 8 mol CO2 = 0.1923 mol CO 13 mol O2 2 ( ( (0.1923 mol CO2) 44 g CO2 1 mol CO2 = 8.46 g CO2 Application of Stoichiometry in Combustion Reactions 4.) How many grams of carbon dioxide and water is produced if 10 grams of butane burns with 10 grams of oxygen? Given: Sol’n: 10 g C4H10 2C4H10(l) + 1313O2(g) 8CO2(g) + 10H2O(l) 10 g O2 Excess Limiting 8.46 g Req’d: Reactant Reactant 18 g/mol mH2O Application of Stoichiometry in Combustion Reactions 4.) How many grams of carbon dioxide and water is produced if 10 grams of butane burns with 10 grams of oxygen? Given: Sol’n: 10 g C4H10 2C4H10(l) + 1313O2(g) 8CO2(g) + 10H2O(l) 10 g O2 Excess Limiting 8.46 g 4.33 g Req’d: Reactant Reactant 18 g/mol mH2O ( ( ( ( ( ( (10 g O2) 1 mol O2 10 mol H2O 18 g H2O 32 g O2 13 mol O2 1 mol H2O = 4.33 g H2O Application of Stoichiometry in Combustion Reactions 4.) How many grams of carbon dioxide and water is produced if 10 grams of butane burns with 10 grams of oxygen? Given: Sol’n: 10 g C4H10 2C4H10(l) + 1313O2(g) 8CO2(g) + 10H2O(l) 10 g O2 10 g 10 g 8.46 g 4.33 g Req’d: mH2O 20 g 12.79 g Application of Stoichiometry in Combustion Reactions 4.) How many grams of carbon dioxide and water is produced if 10 grams of butane burns with 10 grams of oxygen? Given: Sol’n: 10 g C4H10 2C4H10(l) + 1313O2(g) 8CO2(g) + 10H2O(l) 10 g O2 10 g 10 g 8.46 g 4.33 g Req’d: Excess Limiting mH2O Reactant Reactant Application of Stoichiometry in Combustion Reactions 4.) How many grams of excess reactant remains if 10 grams of butane burns with 10 grams of oxygen? Given: Sol’n: 10 g C4H10 2C4H10(l) + 1313O2(g) 8CO2(g) + 10H2O(l) 10 g O2 10 g 10 g 8.46 g 4.33 g Req’d: Excess Limiting mH2O Reactant Reactant Application of Stoichiometry in Combustion Reactions 5.) How many grams of excess reactant remains if 10 grams of butane burns with 10 grams of oxygen? Given: Sol’n: 10 g C4H10 2C4H10(l) + 13 13O2(g) 8CO2(g) + 10H2O(l) 10 g O2 10 g 10 g 8.46 g 4.33 g Req’d: Excess Limiting mx’s Reactant Reactant 12.79 g ( ( ( ( ( ( (10 g O2) 1 mol O2 2 mol C4H10 58 g C4H10 32 g O2 13 mol O2 1 mol C4H10 mbutane consumed = 2.79 g C4H10 12.79 g mx’s = mbutane of Application fedStoichiometry in Combustion Reactions - mbutane consumed 5.) mx’sHow many = 10 g - grams 2.79 gof excess reactant remains if 10 grams of butane burns with 10 grams of oxygen? Given: Sol’n: 10 g C4H10 2C4H10(l) + 13 13O2(g) 8CO2(g) + 10H2O(l) 10 g O2 10 g 10 g 8.46 g 4.33 g Req’d: Excess Limiting mx’s Reactant Reactant ( ( ( ( ( ( (10 g O2) 1 mol O2 2 mol C4H10 58 g C4H10 32 g O2 13 mol O2 1 mol C4H10 mx’s = 7.21 g mbutane consumed = 2.79 g C4H10 Application of Stoichiometry in Combustion Reactions 5.) How many grams of excess reactant remains if 10 grams of butane burns with 10 grams of oxygen? Given: Sol’n: 10 g C4H10 2C4H10(l) + 1313O2(g) 8CO2(g) + 10H2O(l) 10 g O2 10 g 10 g 8.46 g 4.33 g Req’d: mx’s mx’s = 7.21 g Application of Stoichiometry in Combustion Reactions 5.) How many grams of excess reactant remains if 10 grams of butane burns with 10 grams of oxygen? Given: Sol’n: 10 g C4H10 2C4H10(l) + 1313O2(g) 8CO2(g) + 10H2O(l) 10 g O2 10 g 10 g 8.46 g 4.33 g Req’d: mx’s x’s = 7.21 g 20 g 20 g Application of Stoichiometry in Combustion Reactions 6.) Calculate for the mass in grams of carbon dioxide that is produced when a butane gas contained in a 20-liter container at 5 atm and 25 0C, burned completely with excess oxygen. Given: Sol’n: Vbut = 20 L Pbut = 5 atm Tbut = 25 0C Req’d: mCO2 Assumption: ideal gas Application of Stoichiometry in Combustion Reactions 6.) Calculate for the mass in grams of carbon dioxide that is produced when a butane gas contained in a 20-liter container at 5 atm and 25 0C, burned completely with excess oxygen. Given: Sol’n: Vbut = 20 L 2C4H10(l) + 13O2(g) 8CO2(g) + 10H2O(l) Pbut = 5 atm Tbut = 25 0C Req’d: mCO2 Assumption: ideal gas Application of Stoichiometry in Combustion Reactions 6.) Calculate for the mass in grams of carbon dioxide that is produced when a butane gas contained in a 20-liter container at 5 atm and 25 0C, burned completely with excess oxygen. Given: Sol’n: Vbut = 20 L 2C4H10(l) + 13O2(g) 8CO2(g) + 10H2O(l) Pbut = 5 atm Limiting Excess Tbut = 25 0C Reactant Reactant Req’d: mCO2 mass butane = ? mole butane = ? Assumption: ideal gas Application of Stoichiometry in Combustion Reactions 6.) Calculate for the mass in grams of carbon dioxide that is produced when a butane gas contained in a 20-liter container at 5 atm and 25 0C, burned completely with excess oxygen. Given: Sol’n: Vbut = 20 L 2C4H10(l) + 13O2(g) 8CO2(g) + 10H2O(l) Pbut = 5 atm Limiting Excess Tbut = 25 0C Reactant Reactant Req’d: PV = nRT mCO2 ( Assumption: ideal gas ( (5 atm)(20 L) = (n) 0.08206 L atm (25+273.15)K mol K nbut = 4.09 mol Application of) Stoichiometry 44ing CO ( Combustion ( Reactions (4.09 mol C4H10 ( 8 mol CO2 6.) Calculate for the ( massC4inH10 2 mol 2 grams of carbon 1 mol = 719.84 g CO2 dioxide that is produced when a butane gas contained in a 20-liter container at 5 atm and 25 0C, burned completely mwith CO2 =excess 719.84oxygen. g Given: Sol’n: Vbut = 20 L 2C4H10(l) + 13O2(g) 8CO2(g) + 10H2O(l) Pbut = 5 atm Limiting Excess 0 Tbut = 25 C Reactant Reactant 44 g/mol Req’d: PV = nRT mCO2 ( Assumption: ideal gas ( (5 atm)(20 L) = (n) 0.08206 L atm (25+273.15)K mol K nbut = 4.09 mol