Flashcards
CHEM 42 Test 2
Cards in this deck (94)
- 1combustionchemical reaction of a fuel with oxygen to release energy in the form of heat and light
-products CO2 and O2 - 2potential energystored energy
- 3kinetic energyenergy of motion
- 4photosynthesisprocess by which green plants and some bacteria capture the energy in sunlight to produce glucose and oxygen from carbon dioxide and water
-energy from sunlight converted into potential energy of oxygen and glucose - 5fuelsubstance that produces energy when burned
- 6fossil fuelhydrocarbon deposits derived from the remains of ancient plants and animals
- 7What is the first law of thermodynamics?energy is neither created nor destroyed; instead it is transformed
- 8What is the second law of thermodynamics?the entropy (random dispersion of energy) in the universe is increasing
- 9What are the formulas of the first 10 hydrocarbons?1. methane CH4
2. ethane C2H6
3. propane C3H8
4. butane C4H10
5. pentane C5H12
6, hexane C6H14
7. heptane C7H16
8. octane C8H18
9. nonane C9H20
10. decane C10H22 - 10What are some ways to represent hydrocarbon formulas?chemical (molecular) formula, structural (Lewis) formula, condensed structural formula
- 11How are fossil fuels, photosynthesis, and solar energy related?1. plants and some bacteria convert sun's energy to potential energy of glucose and oxygen
2. organisms die, decay, reverse photosynthesis process by releasing CO2 and H2O; sometimes O2 can't reach the organism so partial decay happens
3. transformation into fossil fuels
4. solar energy stored in remains as potential energy are burned as fuel - 12electronegativitymeasure of the attraction of an atom for an electron in a chemical bond
- 13polar covalent bondbond in which electrons are not equally shared but more close to the electronegative atom
- 14nonpolar covalent bondelectrons are shared equally or near equally between atoms
- 15intermolecular forceforce that occurs between two molecules
- 16hydrogen bondelectrostatic attraction of an H atom bonded to a highly electronegative (O, N, F) atom an da neighboring O, N, or F atom
- 17densitymass per unit volume
- 18specific heatamount of energy needed to increase temperature of 1 g of substance by 1 degree celsius
- 19solventsubstance capable of dissolving one or more substances
- 20solutesubstance that dissolves in a solvent
- 21solutionhomogenous mix of solute and solvent
- 22aqueous solutionsolution in which water is the solvent
- 23concentrationconcentration of amount of solute to amount of solution
- 24molarityunit of concentration represented as number of moles solute per liter of solution
- 25nonelectrolytenonconductive solute in an aqueous solution
- 26electrolyteconductive solute in an aqueous solution
- 27ionarom or group of atoms that has acquired an electric charge from gaining or losing electron(s)
- 28cationpositively charged ion
- 29anionnegatively charged ion
- 30ionic bondchemical bond formed when oppositely charged ions attract
- 31ionic compoundions that are present in fixed proportions and arranged in regular, geometric structure
- 32polyatomic ionstwo or more atoms covalently bonded together that have an overall positive or negative charge
- 33electronegativitymeasure of attraction of an atom for an electron in a chemical bond
- 34polar covalent bondbond in which electrons are not equally shared but rather more closer to the more electronegative atom
- 35nonpolar covalent bondelectrons are equally or nearly equally shared between two atoms
- 36intermolecular forceforce that occurs between molecules
-hydrogen bonding - 37hydrogen bondingelectrostatic attraction of an H atom bonded to a highly electronegative atom (F, O, N) and a neighboring F, O, or N atom either in the same molecule or a different one
- 38densitymass per unit volume
-g/cm3
-g/mL - 39specific heatquantity of heat energy that must be absorbed to raise the temperature of 1g of a substance by 1 degree celsius
-water=1.48J/g - 40percentparts per hundred
- 41parts per millionconcentration of one part out of a million
-10,000 times smaller that parts per hundred
-equivalent to 1mg solute/L water - 42parts per billionconcentration of 1 part out of a billion
-1000 times less than ppm - 43molaritymoles solute/liter solution
- 44atomic massthe mass (in g) of the same number of atoms found in exactly 12 grams of carbon 12
- 45Avogadro's numbernumber of atoms in exactly 12 grams of carbon 12 6.02x10^23
- 46molecontaining 6.02x10^23 number of objects
- 47molar massmass of one mole, or Avogadro's number, of whatever particles are specified
- 48combustionreaction of fuel and oxygen to release energy in the form of heat and light
- 49% net efficiency formulaelectrical energy produced/heat from fuel (100)
- 50calorieamount of heat needed to raise the temperature of 1 g of water 1 degree celsius
1000 cal = 1 Cal - 51Jouleenergy required to lift a 1 kg book 10 cm against the force of gravity
1J = 0.239 cal - 52entropymeasure of how much energy gets dispersed in a given process
- 53hydrocarbonscompounds made up of only hydrogen and carbon
- 54alkaneshydrocarbons with only single bonds between carbon atoms
- 55distillationseparation method in which a solution is heated to its boiling point and the vapors are condensed and collected
- 56temperaturemeasure of average kinetic energy of the atoms/molecules in a substance
- 57heatkinetic energy that flows from hotter object to colder one
- 58calorimetermeasures quantity of heat released in a combustion reaction
- 59heat of combustionquantity of heat energy given off when a specified amount of substance burns with oxygen
- 60exothermicchemical or physical change accompanied by the release of heat
-products have lower potential energy - 61endothermicchemical or physical change that absorbs energy
-products have higher potential energy - 62bond energyenergy that must be absorbed to break a certain bond
- 63thermal crackingprocess that breaks large hydrocarbon molecules into smaller ones by heating them to a high temperature
- 64catalytic crackingcatalysts used to crack larger hydrocarbons into smaller hydrocarbons at lower temperatures
- 65catalytic reformingatoms within a molecule are rearranged
- 66isomersmolecules with the same molecular formula but different chemical structures and properties
- 67oxygenated gasolinesa blend of petroleum derived hydrocarbons and oxygen containing compounds such as MTBE, ethanol or methanol
- 68activation energyenergy necessary to initiate a chemical reaction
- 69biofuelsrenewable fuel derived from a biological source
- 70alcoholhydrocarbon substituted with one or more OH group bonded to its carbon atoms
- 71functional groupdistinctive arrangement of atoms that imparts characteristic properties to the molecules that contain the group
- 72complete combustionproduction of CO2 is not offset by some natural process such as photosynthesis
- 73glucose formulac6h12o6
- 74ethanol formulac2h5oh
- 75methanolch3oh
- 76glycerolc3h8oh
- 77What are some examples of biofuels?-cellulosic ethanol from plant containing cellulose
-ethanol formed from starch
-biodiesel from oil or fats (triglycerides)
-glycerol - 78What do biofuels have in common?-all contain oxygen so release less energy than hydrocarbons
- 79ethanol vs gasolinefigure this out
- 80hydrogen fuel benefits and concerns-releases large amount of energy per gram as it burns
-explosive and highly reactive - 81acidcompound that releases hydrogen H+ ions in an aqueous solution
- 82strong acidacid that dissociates completely in aqueous soluitons
-eg HCl - 83weak acidacid that dissociates to small extent in aqueous solutions
-eg. CO2 - 84basecompound that releases hydroxide OH- ions into an aqueous solution
-eg ammonia NH3 - 85strong basesbases that dissociate completely in water
-eg. NaOH - 86weak basesdissociate to only a small extent in aqueous solutions
- 87ocean acidificationlowering of ocean pH due to rising atmospheric CO2 levels
- 88sulfuric acidH2SO4
- 89acetic acidCH3COOH
- 90carbonic acidH2CO3
- 91nitric acidHNO3
- 92hydrochloric acidHCl
- 93phosphoric acidH3PO4
- 94—
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- Chemistry Flashcards on CHEM 42 Test 2, created by Sabrina Paredes on 31/10/2016.
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