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Semester II Review

Semester II Review. SM II Review. Name the compounds H 2 SO 3 Sulfurous Acid H 2 S Hydrosulfuric acid H 3 PO 4 Phosphoric acid HCN Hydrocyanic acid H 3 P Hydrophosphoric acid HBr Hydrobromic acid HClO Hypochlorous acid. SM II Review.

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Semester II Review

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  1. Semester II Review

  2. SM II Review • Name the compounds • H2SO3 Sulfurous Acid • H2S Hydrosulfuric acid • H3PO4 Phosphoric acid • HCN Hydrocyanic acid • H3P Hydrophosphoric acid • HBr Hydrobromic acid • HClO Hypochlorous acid

  3. SM II Review • Give the formula for the following compounds • hydrofluoric acid HF • hydroselenic acid H2Se • carbonic acid H2CO3 • nitrous acid HNO2 • sulfuric acid H2SO4 • hydrobromic acid HBr • Chlorous acid HClO2

  4. SM II Review • Antimony tribromide SbBr3 • Silicon difluoride SiF2 • Tetracarbon octahydride C4H8 • Dinitrogen monoxide N2O • Pentaphosphorous decoxide P5O10 • Sulfur hexachloride SF6

  5. SM II Review • P2O5Diphosphorous pentoxide • SO2Sulfur dioxide • NO2 Nitrogen dioxide • AsCl3 Arsenic trichloride • P4H8 Tetraphosphorous octahydride

  6. Semester II Review • For the following compound, draw its Lewis structure, give the electron tally, hybridization, name of shape, determine if it is polar or not, and identify the Intermolecular Forces. • SO2 e tally = 2BA 1LP, Hybrid = sp2, Shape = Bent, Polar, IMF= Dipole

  7. Semester II Review • For the following compound, draw its Lewis structure, give the electron tally, hybridization, name of shape, determine if it is polar or not, and identify the Intermolecular Forces. • NH3 e tally = 3BA 1LP, Hybrid = sp3, Shape = Trigonal Pyrmidal, Polar, IMF= H-Bonds

  8. Semester II Review • For the following compound, draw its Lewis structure, give the electron tally, hybridization, name of shape, determine if it is polar or not, and identify the Intermolecular Forces. • SO42- e tally = 4BA 0LP, Hybrid = sp3, Shape = Tetrahedral, Nonpolar, IMF(Ion)

  9. Semester I Review • Balance and classify the reactions • _2_ C8H18 + _25_ O2 _16_ CO2 + _18_ H2O • ____ FeCl3 + _3__ NaOH  ____ Fe(OH)3 + _3__NaCl • _4__ P + __5_O2 _2__P2O5 • _2__ Na + _2__ H2O  __2_ NaOH + ____H2 • _2__ Ag2O  _4__ Ag + ____O2 • ____ S8 + _12_ O2 _8__ SO3

  10. SM II Review • Complete, Balance, and Classify each Rxn • 2Al + 3S  Al2S3 Synthesis • NaCl + AgNO3 AgCl + NaNO3 D.R. • C3H8 + 5O2 3CO2 + 4H2O Combustion • 2H2O  2H2 + O2Decomposition • 2Li + Na2CO3 2Na + Li2CO3 S.R. • In every chemical reaction, what item(s) is/are conserved? Mass and Atoms

  11. SM II Review • For a given chemical reaction, the theoretical yield is generally more than the actual yield • The first step in most stoichiometry problems is to balance the equation.

  12. SM II Review • Hydrogen gas reacts with nitrogen gas to form ammonia gas. • Write and balance the equation • 3H2 + N2  2NH3 • Determine the Limiting reactant if 3.50 g of hydrogen reacts with 42.0 g of nitrogen. • What is the theoretical yield of the above problem? 39.4 g NH3 • What is the % yield if the reaction produced 15.3 g of ammonia. 38.8 % • Calculate the amount of grams of excess reactant leftover at the end of the reaction 25.8 g N2 Leftover

  13. SM II Review • What is the empirical formula of a compound that is 32.37 % Na, 22.58 % S, and 45.05 % O. Na2SO4 • If the molecular formula molar mass is 284.10, what is the molecular formula of the above compound. Na4S2O8 • What is the percent composition of FeO? 77.73% Fe and 22.27% O

  14. SM II Review • Calculate the specific heat of an unknown metal, given that 25.0g of the metal lost 3570 J of energy during a temperature change from 100.0oC to 25.0oC • c = -3570J / (25.0g)x(-75.0oC) • c = 1.90 J/goC

  15. Identify each of the letters on the graph and explain what is occurring. C = solid warming/cooling D = Phase change solid to liquid or vice versa E = liquid warming/cooling F = phase change liquid to gas or vice versa G = gas warming/cooling G F E D C SM II Review

  16. Label the solid, liquid, and gas regions on the graph. Label the triple point and critical point At 600oC and 90 atm, what phase is yummygum in? Liquid SM II Review Critical point liquid solid Triple point gas

  17. SM II Review • Calculate the amount of heat released if 25.0g of steam is cooled from 150.0 oC to (-15.0 oC) • Phase 1 = -2537.5 J • Phase change = -56500 J • Phase 2 = -10460 J • Phase change = -8350 J • Phase 3 = -753.75 J • Total Energy = -78600 J

  18. SM II Review • If the volume of a container holding a gas is reduced, what will happen to the pressure within the container? Increase • What happens to the temperature of a gas when it is compressed? Increases • What happens to the pressure of a gas inside a container, if the temperature of the gas is lowered? Decreases • The volume of a gas is doubled while the temperature is held constant. How does the gas pressure change? Decreases by 2 times

  19. SM II Review • Boyle’s law states that PV = K, inverse proportion. • Charles’ law states that V/T = K, direct proportion. • Gay-Lussac’s law states that P/T = K, direct proportion. • Avogadro’s law states that V/n = K, direct proportion. • Dalton's Law states that sum of all the pressures = the total pressure.

  20. Semester II Review • How many grams of CO2 are produced when 34.6 L of CH4 combusts with oxygen at a pressure of 1.78 atm and a temperature of 28oC. • Balance the equation first. (combustion of hydrocarbon) • CH4 + 2O2 CO2 + 2H2O • 2.49 mol CH4 will produce 110. g CO2

  21. SM II Review • A gas confined in a 305 mL container exerts a pressure of 1.07 atm at 38.6°C. At what Celsius temperature will it exert a pressure of 2.75 atm if it is placed into a 644 mL container? • 1506 K - 273 = 1233 °C

  22. SM II Review • What is the pressure inside a 3.0 L flask if 30.5 g of Carbon Monoxide is held at a temperature of 105.2 oC? • 11 atm or 1100 kPa

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