Presentation on theme: "Section B: Petroleum as an Energy Source Man has used oil for over 5000 years First drilled in."— Presentation transcript:
http://www.sebosis.com/members/peter/teaching/chemincomm Section B: Petroleum as an Energy Source Man has used oil for over 5000 years First drilled in 1859 in PA Oil is used in almost every aspect of modern life: products, shipping, manufacturing, heating, transportation, etc
http://www.sebosis.com/members/peter/teaching/chemincomm B.1 Energy and Fossil Fuels: Overview Chemical energy, a form of Potential Energy, is stored in the bonds of compounds In an energy releasing chemical reaction bonds break and reactant atoms reorganize into new bonds Result has less chemical energy, but process released energy (heat and light)
http://www.sebosis.com/members/peter/teaching/chemincomm B.1 Energy and Fossil Fuels: Combustion of Methane Energy releasing reaction of burning methane CH 4 + 2 O 2 CO 2 + 2 H 2 O + energy 2 Steps: Bond breaking, then bond making
http://www.sebosis.com/members/peter/teaching/chemincomm B.1 Energy and Fossil Fuels: Combustion Breaking bonds requires energy: endothermic change (increases chemical energy) energy + CH 4 + 2 O 2 C + 4 H + 4 O The forming new bonds releases energy: exothermic change (decreases chemical energy [>]) C + 4 H + 4 O CO 2 + 2 H 2 O + energy Overall this is exothermic as more is released when reforming than is required to break bonds
http://www.sebosis.com/members/peter/teaching/chemincomm B.1 Energy and Fossil Fuels: Combustion (continued) Overall reaction maybe exothermic or endothermic: –if more energy is added to break bonds than produced when bond making then endothermic –opposite, like burning methane, is exothermic Generally, if a reaction is endothermic, then the reverse reaction is exothermic Actual reaction mechanism are more complex
http://www.sebosis.com/members/peter/teaching/chemincomm B.2 Energy Conversion Conversion makes energy more useful Hair dryer example: oil/potential - generate steam/thermal – spin turbine/kinetic - general electricity/electrical – transmit – thermal and kinetic in the hair dryer. Energy is not consumed, but changes form - Law of Conservation of Energy But some energy is lost to useful work.
http://www.sebosis.com/members/peter/teaching/chemincomm B.2 Energy Conversion (continued) Conversion of chemical energy into heat and then mechanical typically loses > 50% Minimizing conversion is essential to using fuel efficiently Solar cells (convert sunlight to electricity) and fuel cells (convert chemical energy to electricity) hold promise in adding efficiency of petroleum use.
http://www.sebosis.com/members/peter/teaching/chemincomm B.2 Energy Conversion – Automobile example Around 25% of the energy in gasoline contributes to powering the drive wheels. 75% is lost into the environment, mostly in the form of heat: 33% lost through exhaust, 30% through engine cooling, 6% pumping combustion air, 3% due to piston ring friction, …
http://www.sebosis.com/members/peter/teaching/chemincomm B.3 Combustion Lab: Background In this lab we measure how much thermal energy is released when burning a fuel. We burn a paraffin wax candle (long chain alkane) under a can of water and watch the water temperature increase. We will note the increase in temperature, while the mass of the candle decreases.
http://www.sebosis.com/members/peter/teaching/chemincomm B.3 Combustion Lab: Background Candle wax burning: (exothermic) C 25 H 52 (s) + 38 O 2 (g) 25 CO 2 (g) + 26 H 2 O (g) + E Paraffin wax Oxygen Carbon Dioxide water vapor ENERGY (Alkane)gasgasgas More energy is liberated by forming bonds of the CO 2 and H 2 O molecules than is required to break bonds of C 25 H 52 and O 2
http://www.sebosis.com/members/peter/teaching/chemincomm B.3 Combustion Lab: Background Specific heat capacity of a substance is the quantity of heat needed to raise the temperature of 1 gram of the substance by 1° C. The SHC of water is 4.2 J/(g·°C or joules per gram per degree Celsius ). To raise the temperature of 10 g water from 25°C to 30°C: 4.2 J * 10 g * 5°C = 210 J
http://www.sebosis.com/members/peter/teaching/chemincomm B.3 Combustion Lab: Background Heat of combustion is the quantity of thermal energy given off when a certain amount of substance is burned. This is usually measured when : –one gram or –one mole (molar heat of combustion) of substance is burned.
http://www.sebosis.com/members/peter/teaching/chemincomm Hydrocarbon Table: Including Heat of Combustion Boiling ShortHeat ofMolar Heat of Name Point (C)#Carbon formula Combustion (kJ/g) Combustion (kJ/mol) Methane-1621 CH 4 55.6890 Ethane-88.62 C2H6C2H6 52.01560 Propane-42.13 C3H8C3H8 50.02200 Butane-0.54 C 4 H 10 49.32859 Pentane36.15 C 5 H 12 48.83510 Hexane68.76 C 6 H 14 48.24141 Heptane98.47 C 7 H 16 *** 48.24817 Octane125.78 C 8 H 18 47.85450
http://www.sebosis.com/members/peter/teaching/chemincomm B.3 Combustion Lab: Calculations 1.Mass of water in grams = volume of water (100mL) * 1.0 g/mL 2.Total rise in temperature = final temperature – initial temperature 3.Heat = mass * Specific heat of substance (water – 4.2J/(g·°C)) * change in temp. 4.Mass of burned wax = Mass of candle & card before burn – mass after burn 5.Heat of combustion of paraffin = #3 / #4
http://www.sebosis.com/members/peter/teaching/chemincomm B.4 Using Heats of Combustion Hydrocarbon + Oxygen gas Carbon dioxide+Water+??Thermal energy?? 2 C 2 H 6 + 7 O 2 4 CO 2 + 6 H 2 O + 3120 kJ (see the table with heat of combustion entry for ethane-C 2 H 6 ) Notice the table entry is for one mole, we have 2 here 2 C 2 H 6 so we multiply by 2. 12 g of octane would be: 12 * 47.8kJ = 574 kJ
http://www.sebosis.com/members/peter/teaching/chemincomm B.5 Altering Fuels: Overview Due to changes in demand various fractions of hydrocarbons vary in price over time. E.G: the gasoline fraction demand is growing more quickly than other types, such as kerosene Chemists and chemical engineers work innovate to maximize $ for crude oil, by maximizing the amount of the more valuable fractions while minimizing less valuable fractions of distillation.
http://www.sebosis.com/members/peter/teaching/chemincomm B.5 Altering Fuels: Cracking Due to cars becoming more popular in the early 1900s chemists invented cracking. Cracking - larger hydrocarbons are broken into smaller ones. E.G: C 16 => 2 C 8 s (kerosene into gasoline) Extra C 1-4 are burned to feed the cracking process > 1/3 of all crude is cracked, and catalysts are used such as aluminosilicates for efficiency (< tempature) Gasoline is mostly straight chain, but branched chains burn better in engines – less knocking. E.G: 2,2,4-trimethylpentane isomer of octane is works well
http://www.sebosis.com/members/peter/teaching/chemincomm B.5 Altering Fuels: Octane Rating Isooctane (2,2,4-trimethylpentane) by definition is 100 octane, straight chain heptane is 0. Gas is rated this way. (> isooctane > octane rating, > heptane < octane rating) Prior to the mid-1970, lead, was added to gasoline to inexpensively increase the octane rating by more slowly burning straight chain gasoline molecules, but the lead was found to be harmful to the environment, so eliminated.
http://www.sebosis.com/members/peter/teaching/chemincomm B.5 Altering Fuels: Oxygenated Fuels A fuel with an oxygen atom – added to gasoline to raise octane rating, introduced when lead was removed. (burns cleaner due to the oxygen) Methanol (methyl alcohol, CH 3 OH): > octane rating and produced from natural gas, coal, corn or wood MTBE (116 octane rating), first used in 70s as an octane booster then increased importance as an oxygenated additive. BUT is mixes readily with water, tastes bad, can be bad for you, and seeps into water from leaking tanks. (net: good for air, bad for water) Some states have eliminated the use, some others limiting use. MTHF (87 octane rating), is promising. Generated from renewable resources, also oxygenates fuel
http://www.sebosis.com/members/peter/teaching/chemincomm B.5 Altering Fuels: Oxygenated Fuels (continued) Octane ratings can also be boosted by isomerization – convert straight chain hydrocarbon molecules to branched chain Hydrocarbon vapor is heated with a catalyst to get branched chains. Branched C 6 H 14 can be added to gasoline fractions (C 5-12 ) to produce high-quality gas Isomerization and cracking add costs!