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WWU CHEM 121 - Climate Change

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Climate ChangeSlide 2Greenhouse effectEffects The effects of climate change are already visible – melting glaciers, the migration of plant and animal species, and an increase in severe storms, to name a few. What will happen next? No one can say for sure, but here are some possibilities:Carbon CalculatorConvert your average CO2 consumption into gramsContents and ConceptsSlide 8Slide 9Figure 3.3: Reaction of zinc and iodine causing iodine to vaporize. Photo courtesy of James Scherer.Slide 11The MoleSlide 13Slide 14Figure 3.2: One mole each of various substances. Photo courtesy of American Color.Slide 16Slide 17Slide 18Slide 19Slide 20Slide 21Slide 22Slide 23Slide 24Slide 25Slide 26Slide 27Slide 28Slide 29Slide 30Slide 31Slide 32Slide 33Slide 34Slide 35Slide 36Slide 37Slide 38Climate Change•Climate change is a significant shift in temperature and weather patterns around the world. While some changes are normal, the vast majority of scientists agree that our activities are causing dramatic changes to the Earth’s climate.A little bit of carbon dioxide is a good thing – it keeps the planet warm and habitable. Now, however, we are putting so much carbon dioxide into the atmosphere that the planet is getting too warm. This problem is also called the greenhouse effect . Over the last three hundred years we have radically increased our use of energy sources like oil, coal and natural gas. Burning these fuels releases carbon dioxide into the atmosphere.Greenhouse effectmoduleEffects The effects of climate change are already visible – melting glaciers, the migration of plant and animal species, and an increase in severe storms, to name a few. What will happen next? No one can say for sure, but here are some possibilities:•Rising sea levels destroy coastal areas •Frequent and intense heat waves •More droughts and wildfires •Extinction of millions of species •Spreading of weather-sensitive diseaseCarbon Calculator•Estimate your personal carbon usage!!•Here's a different sort of calculator•Low Impact Living•My footprintConvert your average CO2 consumption into grams•There are 2000 lb/ton•There are 454 g/lbContents and ConceptsMass and Moles of SubstancesHere we will establish a critical relationship between the mass of a chemical substance and the quantity of that substance (in moles).• Molecular Mass and Formula Mass• The Mole ConceptDetermining Chemical FormulasExplore how the percentage composition andmass percentage of the elements in a chemicalsubstance can be used to determine thechemical formula.3.Mass Percentages from the Formula4.Elemental Analysis: Percentages of C, H, and O5.Determining FormulasStoichiometry: Quantitative Relations in Chemical Reactions•Develop a molar interpretation of chemical•equations, which then allows for calculation•of the quantities of reactants and products.6. Molar Interpretation of a Chemical Equation7. Amounts of Substances in a Chemical Equation8. Limiting Reactant: Theoretical and Percentage YieldFigure 3.3: Reaction of zinc and iodine causing iodine to vaporize. Photo courtesy of James Scherer.Counting Objects of Fixed Relative Mass12 red marbles @ 7g each = 84g12 yellow marbles @4e each=48g55.85g Fe = 6.022 x 1023 atoms Fe32.07g S = 6.022 x 1023 atoms S•The Mole is based upon the definition:•The amount of substance that contains as many elementary parts (atoms, molecules, or other?) as there are atoms in exactly •12 grams of carbon -12.•1 Mole = 6.022045 x 1023 particlesThe MoleMole - Mass Relationships of ElementsElement Atom/Molecule Mass Mole Mass Number of Atoms1 atom of H = 1.008 amu 1 mole of H = 1.008 g = 6.022 x 1023 atoms1 atom of Fe = 55.85 amu 1 mole of Fe = 55.85 g = 6.022 x 1023 atoms1 atom of S = 32.07 amu 1 mole of S = 32.07 g = 6.022 x 1023 atoms1 atom of O = 16.00 amu 1 mole of O = 16.00 g = 6.022 x 1023 atoms1 molecule of O2 = 32.00 amu 1 mole of O2 = 32.00 g = 6.022 x 1023 molecule1 molecule of S8 = 2059.52 amu 1 mole of S8 = 2059.52 g = 6.022 x 1023 moleculesCaCO3 100.09 gOxygen 32.00 gCopper 63.55 gWater 18.02 gOne Mole of Common SubstancesFigure 3.2: One mole each of various substances.Photo courtesy of American Color.•Molecular Mass•The sum of the atomic masses of all the atoms in a molecule of the substance•Formula Mass•The sum of the atomic masses of all atoms in a formula unit of the compound, whether molecular or notMolecular Mass - Molar Mass ( M )The Molecular mass of a compound expressed in amu is numerically the same as the mass of one mole of the compound expressed in grams. For water: H2O Molecular mass = (2 x atomic mass of H ) + atomic mass of O = 2 ( 1.008 amu) + 16.00 amu = 18.02 amu Mass of one molecules of water = 18.02 amu Molar mass = ( 2 x atomic mass of H ) + atomic mass of O = 2 ( 1.008 g ) + 16.00 g = 18.02 g 18.02 g H2O = 6.022 x 1023 molecules of water = 1 mole H2O•Calculate the formula weight of the following compounds from their formulas. Report your answers to three significant figures.–calcium hydroxide, Ca(OH)2–methylamine, CH3NH23 significant figures74.1 amu3 significant figures31.1 amuTotal 74.0952 O 2(16.00) = 32.00 amuCa(OH)21 Ca 1(40.08) = 40.08 amu2 H 2(1.008) = 2.016 amuCH3NH21 C 1(12.01) = 12.01 amu5 H 5(1.008) = 5.040 amu1 N 1(14.01) = 14.01 amuTotal 31.060Information Contained in the Chemical Formula of Glucose C6H12O6 ( M = 180.16 g/mol)Carbon (C) Hydrogen (H) Oxygen (O)Atoms/moleculeof compoundMoles of atoms/mole of compoundAtoms/mole ofcompoundMass/moleculeof compoundMass/mole of compound6 atoms 12 atoms 6 atoms6 moles of 12 moles of 6 moles of atoms atoms atoms 6(6.022 x 1023) 12(6.022 x 1023) 6(6.022 x 1023) atoms atoms atoms6(12.01 amu) 12(1.008 amu) 6(16.00 amu) =72.06 amu =12.10 amu =96.00 amu72.06 g 12.10 g 96.00 g•What is the mass in grams of the nitric acid molecule, HNO3?First, find the molar mass of HNO3:1 H 1(1.008) = 1.0081 N 1(14.01) = 14.013 O 3(16.00) = 48.00 63.018(2 decimal places)63.02 g/molmolecules10x6.02 mol1 x molg 63.0223g 10x41.0468438522figures)tsignifican(3g 10x1.05 is molecule HNO one of mass The223.Next, convert this mass of one mole to one molecule using Avogadro’s


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