General Chemistry CHM 1032 Final Review – Fall 2017Hannah SageDisclaimer: I have made this review to the best of my ability. It is not comprehensive and should only be used as an aid to your review, not as your only study tool.All the problems are from Tro, Nivaldo J. Introductory Chemistry. 2nd ed., Pearson/Prentice Hall, 2009.

1. What is the difference between a law and a theory?

2. Classify each as an observation, a law, or a theorya. When a metal is burned in a closed container, the mass of the container and its

contents does not changeb. Matter is made of atomsc. Matter is conserved in chemical reactionsd. When wood is burned in a closed container, its mass does not change

3. Perform the following calculations to the correct number of significant figuresa. 87.6 + 9.888 + 2.3 + 10.77

b. 43.7 * 2.341

c. 89.6 + (98.33 * 4.674)

d. (6.99 – 5.772) * 3.44

4. Perform each of the following conversions.a. 2.14 kg to grams

b. 6172 mm to meters

c. 1316 mg to kilograms

d. 0.0256 L to milliliters

e.5. Total U.S. farmland occupies 954 million acres. How many square miles is this?

(1 acre = 43,560 ft2, 1 mi = 5280 ft)6. Ethylene glycol (antifreeze) has a density of 1.11 g/cm3.

a. What is the mass in grams of 417 mL of this liquid?

b. What is the volume in liters of 4.1 kg of this liquid?

7. Classify each of the following as a pure substance or a mixture. If a pure substance, classify it as an element or a compound. If it is a mixture, classify it as homogeneous or heterogeneous.

a. Helium gasb. Clean airc. Rocky road ice creamd. Concrete

8. Determine whether each of the following changes is chemical or physical.a. A balloon filled with hydrogen gas explodes upon contact with a spark.

b. The liquid propane in a barbecue evaporates away because the user left the valve open.

c. The liquid propane in a barbecue ignites upon contact with a spark.

d. Copper metal turns green on exposure to air and water.

9. The coldest temperature ever measured in the U.S. was -80F in Prospect Creek, Alaska. Convert this temperature to degrees Celsius and Kelvin.

10. An unknown metal with a mass of 28 g absorbs 58 J of heat. Its temperature rises from 31.1C to 39.9C. Calculate the heat of capacity of the metal.

11. Predict the ion formed by each of the following:a. Rbb. Kc. Ald. O

12. Determine the number of protons, electrons, and neutrons in each of the following:a. 23

11Nab. 266

88Rac. 208

82Pb

d. 147N

13. Bromine has two naturally occurring isotopes (Br-79 and Br-81) and an atomic mass of 79.904 amu.

a. If the natural abundance of Br-79 is 50.69%, what is natural abundance of Br-81?

b. If the mass of Br-81 is 80.9163 amu, what is the mass of Br-79?

14. Classify each of the following compounds as ionic or molecular.a. CS2

b. CuOc. KId. PCl3

15. Write a formula for the ionic compound that forms from each of the following pairs of elements.

a. Sodium and sulfurb. Strontium and oxygenc. Aluminum and sulfurd. Magnesium and chlorine

16. Name each of the following compoundsa. CsClb. SrBr2

c. SnO2

d. PbI2

e. NH4If. CoSO4

17. Write a formula for each of the following ionic compoundsa. Copper (II) bromideb. Silver nitratec. Potassium hydroxided. Sodium sulfatee. Potassium hydrogen sulfatef. Sodium hydrogen carbonate

18. How many moles of tin atoms are in a pure tin cup with a mass of 38.1 g?

19. How many molecules are in each of the following?a. 3.5 mol H2O

b. 56.1 g N2

20. Which of the following contains the greatest number of moles of O?a. 2.3 mol H2O

b. 1.2 mol H2O2

c. 0.9 mol NaNO3

d. 0.5 mol Ca(NO3)2

21. A 1.912 g sample of calcium chloride is decomposed into its constituent elements and found to contain 0.690 g Ca and 1.222 g Cl. Calculate the mass percent composition of Ca and Cl in calcium chloride.

22. A compound containing nitrogen and oxygen is decomposed in the laboratory and produces 1.78 g of nitrogen and 4.05 g of oxygen. Calculate the empirical formula of the compound.

23. A compound containing carbon and hydrogen has a molar mass of 56.11 g/mol and an empirical formula of CH2. Find its molecular formula.

24. Balance each of the following chemical equations.a. O2 (g) + HCl(aq) Cl2(g) + H2O (l)b. O2 (g) + H2 (g) H2O (l)c. Co(NO3)3 (aq) + (NH4)2S(aq) Co2S3(s) + NH4NO3 (aq)

25. Determine whether each of the following compounds is soluble or insoluble. For the soluble compounds, write the ions present in the solution.

a. RbNO3

b. NiCO3

c. (NH4)2Sd. Sn(C2H3O2)2

26. Complete and balance each of the following equations. If no reaction occurs, write NO REACTION.

a. KI(aq) + BaS (aq)

b. K2SO4 (aq) + BaBr2 (aq)

c. NaCl (aq) + Hg2(C2H3O2)2 (aq)

d. NaC2H3O2 (aq) + Pb(NO3)2 (aq)

27. Aqueous potassium sulfide reacts with aqueous lead (II) nitrate. Write the balanced complete and net ionic equations.

28. Complete and balance the following equation for an acid-base reaction.a. HCl(aq) + Ba(OH)2 (aq)

29. Complete and balance each of the following equations for combustion reactions.a. C2H6(g) + O2(g) b. C3H8O(l) + O2 (g)

30. Classify each of the following chemical reactions as a synthesis, decomposition, single-displacement, or double-displacement reaction.

a. K2S(aq) + Co(NO3)2 (aq) 2KNO3(aq) + CoS(s)b. 3H2(g) + N2(g) 2 NH3(g)c. Zn(s) + CoCl2 (aq) ZnCl2 + Co(s)d. CH3Br(g) CH3(g) + Br(g)

31. For the reaction shown, calculate how many moles of NO2 form when 5.8 mol N2O5 reacts completely.

2 N2O5(g) 4 NO2(g) + O2(g)

32. For the reaction shown, calculate how many grams of oxygen form when 3.87 mg HgO reacts completely.

2 HgO(s) 2Hg(l) + O2(g)

33. For the reaction shown, find the limiting reactant for each of the following initial conditions

2K(s) + Cl2(g) 2KCl(s)a. 1 mol K; 1 mol Cl2

b. 2.2 mol K; 1 mol Cl2

34. Consider the following equation for the combustion of acetone (C3H6O), the main ingredient in nail polish remover. If a bottle of nail polish remover contains 155 g of acetone, how much heat would be released by its complete combustion.

C3H6O(l) + 4 O2(g) 3CO2(g) + 3 H2O(g) Hrxn = -1790 kJ

35. Rank the following types of electromagnetic radiation in order of increasing energy per photon.

a. Radio wavesb. Microwavesc. Infraredd. Ultraviolet

36. Write full orbital diagrams for each of the following elements and indicate the number of valence electrons and core electrons in each.

a. B

b. F37. Write noble gas electron configurations for each of the following elements.

a. Gab. Asc. Sn

38. Choose the element with the higher ionization energy from each of the following pairs.a. As or Bib. As or Br

39. Write a Lewis structure for each of the following compounds.a. NaF

b. SrBr2

c. SCl2

d. CO3 2-

40. Determine the electron and molecular geometries of each of the following molecules.a. N2O (oxygen is terminal)

b. SO2

c. H2S

d. PF3

41. A balloon with an initial volume of 3.2 L at a temperature of 299 K is warmed to 376 K. What is the volume at the final temperature?

42. A sample of gas with an initial volume of 32.5 L at a pressure of 755 mmHg and a temperature of 315 K is compressed to a volume of 15.8 L and warmed to a temperature of 395 K. What is the final pressure of the gas?

43. A cylinder contains 11.8 L of air at a total pressure of 43.2 psi and a temperature of 25C. How many moles of gas does the cylinder contain?

44. How many liters of hydrogen gas are formed from the complete reaction of 1.07 mol of C? Assume that the hydrogen gas is collected at a pressure of 1.0 atm and temperature of 315 K.

C(s) + H2O(g) CO(g) + H2(g)