Spring Semester Review - Honors Chemistry

Honors Chemistry Semester II Review
Behavior of Gases and States of Matter (Ch 12 & 13)
1. What are the major assumptions of the kinetic theory?
2. Theoretically, at _____ K, all motion stops.
3. What is standard air pressure in the following units?
__________ torr
__________ atmospheres
__________ mm Hg
__________ kPa
__________ inches of Hg
4. An open manometer is filled with water and connected to a container of neon gas. The water
level is 578 mm higher in the open arm. The barometric pressure is exactly 101.325 kPa.
What is the pressure, in mm Hg, of the neon?
5. Make the following temperature conversions:
a. 516 K to ºC b. 421 ºC to K
6. A nitrogen molecule has a velocity of 500.0 m/s at room temperature and pressure. What is
the velocity of a helium molecule at the same temperature and pressure?

*** Match the law with the description:
a. Boyle’s Law d. Combined Law
b. Charles' Law e. Graham’s Law
c. Dalton’s Law f. Gay-Lussac
_____ 7. The effect of temperature and pressure on volume.
_____ 8. The velocity of a gas is inversely related to the square root of its mass.
_____ 9. The effect of pressure on volume.
_____ 10. P T = P 1 + P 2 + P 3 …
_____ 11. The effect of temperature on volume.
_____ 12. The effect of temperature on pressure.
13. Correct the following gas volumes from the initial conditions listed to the new conditions.
Assume that the pressure or temperature is constant if not given.
a. 95.0 mL at STP to 24.0C and 91.5 kPa b. 245 mL at 5.0C and 92.0 kPa to
40.0C and 785 mm Hg
14. From the volume, temperature and pressure data given, calculate the number of moles and the
mass in grams for each gas listed:
a. 2000.0 mL NH 3 at 10.0ºC and 105.0 kPa b. 5.00 dm 3 SO 2 at 21.0ºC and 100.0 kPa
15. Calculate the volume each gas will occupy under the conditions listed.
a. 5.00 mol CH 4 at 27.0ºC and 97.2 kPa b. 200.0 g NH 3 at 12.0º C and 777 mm Hg
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16. What happens to pressure if:
a. the volume decreases to ¼ V?
b. the temperature increases to 1.5 T?
c. the number of moles increases to 3 times the moles?
17. How many mL of hydrogen gas can be produced when 6.05 g HCl reacts with 5.15 g of Mg
at STP?
18. Calculate the volume that 0.881 mol of gas will occupy at STP.
19. What is the density of CO 2 at STP?
20. Ammonia is synthesized from its elements. If 5.00 L of nitrogen gas reacts with excess
hydrogen gas, what volume of ammonia can be produced at STP?
Miscellaneous Info about Water and Aqueous Systems
1. In a closed, insulated system, ice is floating in water. The temperature is 0.0ºC. Will all of
the water freeze? Why?
2. Water is boiling at 100ºC. The hot plate's surface temperature is increased. Will the water
now boil at a higher temperature?
3. Is the vapor pressure of the liquid phase and the vapor pressure of the gas phase equal at the
boiling point?
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4. Are the attractive forces between the particles strong or weak when the vapor pressure of a
substance is high?
5. When hydrogen is bonded to a highly electronegative element, what intermolecular attractive
force results?
6. How much energy is required to raise the temperature of 175 g H 2 O from 11.0ºC to 140.0ºC?
7. What happens to the solubility of a solid if the temperature of the solution increases?
8. What happens to the solubility of a gas if the temperature of the solution increases?
9. How is a colloid different from a solution?
Solutions (Ch 14)
1. Calculate the molarity of the following solutions:
a. 500.0 cm 3 that contains 82.0 g b. 250.0 mL that contains 50.0 g
calcium nitrate
copper II sulfate pentahydrate
2. Calculate the mass of solute needed for the following:
a. 255 mL of 2.00 M Na 2 SO 4 7H 2 O b. 1.500 dm 3 of 0.0240 M KH 2 PO 4
3. Calculate the molality of the following solutions:
a. 15.0 g ethanol dissolved in 250.0 g water b. 1.20 x 10 23 molecules acetic acid
dissolved in 1500.0 g water
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4. Describe how you would make the following solutions:
a. 2.50 m solution of glucose containing 2000.0 g water
b. 1.25 m solution of NaCl containing 26.0 g NaCl
5. Determine the mass of ethylene glycol C 2 H 4 (OH) 2 , which must be dissolved in 2500.0 g water
to make a 4.00 m solution.
6. Calculate the mole fraction of methanol, CH 3 OH, when 3.20 g of methanol is dissolved in 4.61
g of ethanol, CH 3 CH 2 OH.
7. What is a colligative property?
8. What are the freezing and boiling points of a solution that contains 10.0 g naphthalene, C 10 H 8 ,
dissolved in 50.0 g water?
9. How many grams of an organic compound (molecular mass 75.0g/mol) must be dissolved in
500.0 g water to lower the freezing point of the solution to –2.57 ˚C?
10. What is the molecular mass of an organic compound if 16.0 g of the compound, when
dissolved in 225.0 g water, increased the boiling point by 8.56 C?
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11. Which substance forms the better electrolyte and WHY? 3 M NaCl or 4 M sucrose?
12. How would you make a supersaturated solution?
13. If the solubility of a gas in water is 5.25 g/100 mL when the pressure above the gas is 105.7
kPa, what is the solubility when the pressure is 101.3 kPa?
14. If the % (M/V) concentration for the solute is 5.0 % and the volume of the solution is 500.0
mL, what is the mass of the solute?
Acids and Bases (Ch 18)
1. Define an acid according to the following theories:
a. Arrhenius
b. Bronsted-Lowry
c. Lewis
2. What are the products of a neutralization reaction? What is the difference between a strong
and a weak acid?
3. Name the following acids and bases:
a. H 2 S d. H 3 PO 4 g. H 2 SO 3
b. H 2 SO 4 e. HClO 3 h. HI
c. Mg(OH) 2 f. Al(OH) 3 i. KOH
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4. Label the acid, base, conjugate acid, and conjugate base in the following reactions:
a. HSO 4
- (aq) + Cl - (aq) SO 4
2- (aq) + HCl (aq)
b. OH - (aq) + CH 3 COOH (aq) CH 3 COO - (aq) + H 2 O (l)
5. The approximate pH of some common substances is listed below. Calculate the pOH, [H 3 O+],
and the [OH-].
a. vinegar, 2.90 b. soft drink, 3.00 c. egg, 7.80
6. How many cm 3 of 0.500 M NaOH are required to completely neutralize 20.00 cm 3 of each of
the following acids:
a. 0.150 M HNO 3 b 0.450 M H 3 PO 4
7. How many moles of aluminum hydroxide are required to neutralize 3 moles of phosphoric
acid?
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Organic Chemistry (Ch 21 & 22)
1. A chain compound in which all carbon-carbon bonds are single is called a(n) _____________
or a ________________________.
2. The boiling point of the alkanes (increases or decreases) with more branches.
3. With increasing molecular mass of compounds within a homologous series, the boiling point
______________________. The smallest alkanes are _________________ at room temperature.
4. Name the following compounds:
a. C 5 H 12 b. C 8 H 18 c.C 8 H 16 d. C 4 H 6
5. Draw structural formulas for the following:
a. Benzene b. cyclohexane c. 4-ethyl-2,3-dimethyloctane
d. 2-butene e. 1-hexyne f. Heptanoic acid
6. Name the following molecules:
a. b.
c. d.
7. ____________________ are substances with the same formula but different arrangements.
8. Draw three structural isomers of C 6 H 14 :
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9. Draw and label structures that are examples of each of the following types of isomers: cis,
trans, positional, functional, and optical isomers.
10. Draw structural formulas and predict the products of the following:
a. 2-butene + hydrogen iodide
b. bromine + ethene
c. complete combustion of ethane
d. elimination of water from 1-pentanol
e. benzene + chlorine gas
f. ethanoic acid + ethanol
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Nuclear Chemistry (Ch 24)
1. Sodium-24 has a half-life of 15.0 hours. How much sodium-24 will remain from a 18.0 g
sample after 33.5 hours?
2. What happens when a neutron beaks down?
3. Write nuclear equations for these reactions:
a. the alpha decay of Po-218:
b. the beta decay of Pb-210:
c. the electron capture by Be-7:
d. the positron emission of F-19:
4. Complete the following transmutation reactions:
a. Li-6 reacts with a neutron to form an alpha particle plus one other particle. What is
the missing particle?
b. U-235 is bombarded with a neutron to form Rb-90 and Cs-144. What are the missing
particles?
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5. An artifact is found to contain 0.73 times the C-14 found in a living plant. What is the
approximate age of the plant?
6. Calculate the binding energy of an N-14 atom (mass = 14.00307 amu):
Thermochemistry (Ch 15)
1. What is the amount of heat required to raise the temperature of 200.0 g of aluminum by
10ºC?
2. What is the specific heat of a substance a 2.78 g sample of the material absorbs 241 J of
energy when its temperature increases by 175ºC.
3. A student mixed 100.0 mL of water at 47.2ºC with 35.0 g lead at 112ºC. What was the
final temperature of the mixture?
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4. Use Hess’s Law and the following thermochemical equations to produce the
thermochemical equation for the following reaction:
C (s, diamond) C(s, graphite)
What is the H for the reaction?
C (s, graphite) + O 2 (g) CO 2 (g)
C (s, diamond) + O 2 (g) CO 2 (g)
H = -394 kJ
H = -396 kJ
5. Calculate G system for each process and state whether the process is spontaneous or
nonspontaneous:
a) H system = 145 kJ, T = 293 K, S system = 195 J/K
b) H system = -232 kJ, T = 273 K, S system = 138 J/K
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