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Chem 1151 Review

Chem 1151 Review. Chapters 1-4. Chap 1. The edge of a cube is 39.3 cm. What is the volume in cm 3 ? m 3 ? gal? Note SF 1 in = 2.54 cm and 1 gal = 231 in 3 (56.1 – 51.1)/6.58 = Convert 3.18 μ s to ms Pt has a density of 21.4 g/cm 3 . What is the mass of a Pt sample of volume 5.0 in 3 ?

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Chem 1151 Review

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  1. Chem 1151 Review Chapters 1-4

  2. Chap 1 • The edge of a cube is 39.3 cm. What is the volume in cm3? m3? gal? Note SF 1 in = 2.54 cm and 1 gal = 231 in3 • (56.1 – 51.1)/6.58 = • Convert 3.18 μs to ms • Pt has a density of 21.4 g/cm3. What is the mass of a Pt sample of volume 5.0 in3? • 0.00015 x 54.6 + 1.002 =

  3. Chap 1 • Memorize T 1.2 from kilo to pico • 1 cm3 = 1 mL • Density of water = 1 g/cm3

  4. Chap 2 • Nuclide symbol for the species with 14 p+ and 14 n0. • Nuclide symbols for ions • Atomic wt for this element  • Write the formulas for and name • Co2+ and Br - • Na+ and PO43- • Cr 3+ and O2- • Ca2+ and HCO3- • Cs+ and S2-

  5. Chap 2 • Write formulas for • Nitrogen tribromide, oxygen difluoride, dichlorine pentoxide, dinitrogen tetrafluoride • Laws: conservation of mass, def proportions, multiple proportions • Theory: Dalton’s Atomic Theory • Memorize T2.5, Fig 2.22, strong acids, bases • Nomenclature rules (Types I, II, III)

  6. Chap 3 • Balance chem eqns • Conversions from g to mol to # atoms • Convert 0.15 mol Na to g to # Na atoms • Convert 2.78 g Hg(NO3)2 to # O atoms • Convert 10.0E20 N atoms in Hg(NO3)2 to mol molecule • # Ca2+ in 2 mol Ca3(PO4)2 • Determine empirical formula for 50.0% C, 5.6% H, 44.4% O

  7. Chap 3 • 3TiO2 +4C + 6Cl2 3TiCl4 + 2CO2 + 2CO • Calc g CO if 100 g TiO2 reacts w/xs C and Cl2 • Calculate g C needed to produce 1.0 kg TiCl4 • If the reaction yield is 70%, how many g C are needed in previous question? • If you start with 4.15g TiO2 and 6.78g Cl2 and xs C, how many g of TiCl4 will be produced? • How many g of the xs reagent (not counting C) will remain at the end of the rxn?

  8. Chap 4 • Memorize solubility rules, OX# rules, balancing redox rxn rules, defn of molarity • Predict solubility of aqueous solns of PbS, Na2CO3, Li3P, AgBr, BaSO4, NH4Br, Fe(OH)2, PbS, • Write the net ionic eqn for aq solns of • Silver nitrate + sodium bromide • Lead(II) nitrate + potassium sulfate • Hydrobromic acid + strontium hydroxide • Sodium carbonate + magnesium iodide

  9. Chap 4 • What is the molarity of a 50.0 mL solution containing 0.798 g KMnO4? • What volume of 0.120 M CuSO4 contains 0.150 mol solute? • Prepare 1.50 L of a 0.50 M solution of HCl from 12.4 M HCl stock soln. • What is the molarity of sodium ions in a 0.33 M soln of sodium phosphate?

  10. Chap 4 Na2CO3(aq) + Ca(OH)2(aq)  CaCO3(s) + 2NaOH(aq) • What volume of 0.350M Na2CO3 is required to react with 49.8 mL of 0.150M Ca(OH)2? • How many g of CaCO3 will be produced when 33.0 mL of 0.250M Na2CO3 reacts with 57.0 mL of 0.200M Ca(OH)2?

  11. Chap 4 • Determine the OX# of N in NO, NO2, N2O, NH2-, N2, N2O5, NO2-, N2O4 • Br2 + SO2 Br- + SO42- balance in acid • MnO4- + I-  MnO2 + IO3- bal in base • In the reactions above, what is oxidized?, reduced? What is the RA?, OA? #e- transferred?

  12. Chap 4 KI(aq) + AgNO3(aq)  KNO3(aq) + AgI(s) • Excess silver nitrate was added to a 10.0 mL sample of KI soln. If 2.183 g AgI was produced, what is the molarity of the KI soln? • If the rxn above has an 80% yield, what is the molarity of the KI soln?

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