Chemistry Final Exam study guide by nuhman10

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									                                    Chemistry Final Exam
                                        Study Guide

1. A balanced equation allows one to determine the …
2. If one knows the mole ratio of a reactant and product in a chemical reaction, one can …
3. In the equation 2KClO3 → 2KCl + 3O2, how many moles of oxygen are produced when 3.0
    mol of KClO3 decompose completely?
4. For the reaction represented by the equation 2Fe + O2 → 2FeO, how many gram of iron(II)
    oxide are produced from 8.00 mol of iron in an excess of oxygen?
5. When two substances react to form products, the reactant which is used up is called the ____.
6. Provided with a balanced equation, the first step in most stoichiometry problem is to _____.
7. At STP, how many liters of oxygen are required to react completely with 5.5 liters of
    hydrogen to form water? 2H2(g) + O2 → 2H2O(g)
8. Why does a can collapse when a vacuum pump removes air from the can?
9. Why does the air pressure inside the tires of a car increase when the car is driven?
10. Convert the pressure 225 kPa to atm.
11. Standard pressure is exactly ________.
12. The volume of a gas is is 400.0 mL when the pressure is 1.00 atm. At the same temperature,
    what is the pressure at which the volume of the gas is 2.0 L?
13. According to Avogadro’s law, 1 L of H2(g) and 1 L of O2(g) at the same temperature and
    pressure have / contain …..
14. The ideal gas law is equivalent to Charles’s law when …
15. The standard molar volume of a gas is …
16. A gas is confined in a steel tank with a volume of 6.982 L. At 20.20 0C, the gas exerts a
    pressure of 8.532 atm. After heating the tank, the pressure of the gas increases to 10.406 atm.
    What is the temperature of the heated gas?
17. According to Gay-Lussac’s law …
18. The volume of a gas is 1.50 L at 30 0C and 1.00 atm. What volume will the gas occupy if the
    temperature is raised to 134.0 0C at constant pressure.
19. As the temperature of a gas in a balloon deceases, what happens to the volume, gas pressure
    and average kinetic energy of the gas?
20. According to VSEPR theory, the shape of an AB4 molecule is ….
21. How many valence electrons are in a sulfur atom?
22. When one atom contributes both bonding electrons in a single covalent bond, the bond is
    called an …
23. Why do atoms share electrons in covalent bonds?
24. What is a polar bond?
25. Identify an element that can form diatomic molecules held together by a single, double, and a
    triple covalent bond.
26. What are resonance structures?
27. Use VSEPR theory to predict the shape of carbon dioxide CO2.
28. Identify the electronegativity of F, H, N, O, and C
29. Explain why molecules that contain polar bonds may be nonpolar.
30. Define boiling point of a liquid
31. Define dipole force, intermolecular bond, dispersion force and hydrogen bond.
32. Explain the relationship between intermolecular attractions in liquid and the following
    a. viscosity, b. boiling point, c. surface tension, d. vapor pressure
33. The vapor pressure of methanol is 1 mm Hg at -440C; 10 mm Hg at -160C; 1520 mm Hg at
    840C. What is the boiling point of methanol?
34. What is the number of non-bonding electron pairs in a water molecule?
35. Identify the factor that accounts for the unusually high boiling point of water.
36. What is (are) the product(s) from the reaction of water and
        a. A metal oxide, b. nonmetal oxide, c. an active metal?
37. What are the products from the complete decomposition of hydrocarbon?
38. What are the products form the reaction of a strong acid with a strong base?
39. Predict the physical state of helium at 4 K (Bp = 4 K) and 1.1 atm pressure.
40. Apply the like dissolve like rule to predict liquids that are miscible with water.
41. Apply the like dissolve like rule to predict liquids that are miscible with liquid bromine, Br2.
42. Yeast and sugar are added to champagne to give the sparkle of carbonation. Under what
    conditions is carbon dioxide gas most soluble?
43. If 20.0 mL of blood plasma has a mass of 21.0 g and contains 0.870 g of protein, what is the
    mass/mass percent concentration of the sample?
44. What is the mass of solute dissolved in 10.0 g of a 5.00% sugar solution?
45. What is the molarity of a sucrose solution that contains 10.0 g of C12H22O11 (342.24 g/mol)
    dissolved in 100.0 mL of solution?
46. What is the mass of nickel(II) nitrate (182.71 g/mol) dissolved in 25.0 mL of 0.100 M
    Ni(NO3)2 solutions?
47. What is the volume of 12.0 M hydrochloric acid that contains 3.646 g of HCl solute (36.46
    g/mol)?
48. What volume of 18 M sulfuric acid must be diluted with distilled water to prepare 500.0 mL
    of 0.50 M H2SO4?
49. What is the molarity of aqueous potassium hydroxide if 35.5 mL of KOH reacts with 20.0 mL
    of 0.100 M H3PO4?

For chapter 15, please use the following (chapter 15 study guide) to review for the final exam

                                 Chapter 15 Acids and Bases
                                        Study Guide

   Know the general properties of acids and bases
   Know the concept of Arrhenius acid and Arrhenius base
   Be able to identify an Arrhenius acid and an Arrhenius base
   Be able to differentiate strong and weak Arrhenius acids and bases
   Be able to differentiate strong and weak acids and bases by their pH
   Know that acid base reaction is a subset of double replacement reaction
   Know the products of acid base reactions
   Know the concept of Bronsted-Lowry acid and Bronsted-Lowry base
   Be able to identify Bronsted-Lowry acids and bases in a chemical reaction
   Know the color of the acid-base indicators with focus on phenolphthalein
   Know the process of acid base titration
   If 10.0 mL of 0.100 M HCl is tritrated with 0.200 M NaOH, what volume of sodium
    hydroxide solution is required to neutralize the acid?
   If 25.0 mL of 0.100 M HCl is titrated with 0.150 M Ba(OH)2, what volume of barium
    hydroxide is required to neutralize the acid?
   Be able to write simple chemical reaction of an acid base reaction.
   Be able to balance chemical reaction to ensure proper stoichiometry of reaction
      An ammonia solution is 6.00 M and the density is0.950 g/mL. What is the mass/mass percent
       concentration of NH3
      What is the molarity of a nitric acid solution if 25.00 mL of HNO3 is required to neutralize
       0.424 g of sodium carbonate (105.99 g/mol)?(aq)
      If a 0.200 g sample of sodium hydroxide (40.00 g/mol) is completely neutralized with 0.100
       M H2SO4, what volume of sulfuric acid is required?
      Know the chemical equation for the collision of water
      Know the chemical equation for the ionization of water
      Know the ionization constant expression for water
      Given an aqueous solution in which the [H+] = 2.0 x 10-5, what is the molar hydroxide ion
       concentration? What is the pH of the solution?
      What is the pH of an aqueous solution if the [H+] = 0.000000075 M?
      What is the [OH-] in an ammonia solution if the pH is 10.20?

The following are from chapter 16 which we will complete by June 4.

   50. Identify the factors that increases the collision frequency of molecules
   51. Identify the factors that influences the rate of a chemical reaction
   52. Identify the factors that influences on the amount of product produced.
   53. Identify the reaction profile and the equation of reaction of an endothermic reaction, and an
       exothermic reaction.
   54. Understand the concept of the rate of forward reaction and the rate of reverse reactions and
       the state of chemical equilibrium
   55. Write the equilibrium constant expression for a reversible reaction
   56. Calculate the equilibrium constant, Keq from experimental data
   57. What is the general equilibrium constant expression, Keq, for the following reversible
       reaction: 2 A + 3 B ↔ 4 C + D
   58. What is the equilibrium constant expression for the following reaction?
       2 CH4(g) + O2(g) ↔ 2 CO(g) + 4 H2(g)
   59. Ultraviolet light converts oxygen in the upper atmosphere to ozone. Calculate the equilibrium
       constant for the reaction given the equilibrium concentrations at 200C: [O2] = 9.38 x 10-3 and
       [O3] = 3.40 x 10-15.
   60. Which of the changes to the reactant or the products below will shift the equilibrium to the
       right for the following reversible reaction in aqueous solution?
       HNO2(aq) ↔ H+(aq) + NO2-(aq)

								
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