1. In the area of nano-chemistry, particles defined as nanoparticles range in size from 1-2500 nm. 1 nm is equivalent to 1 × 10–9 m. A wavelength of red light is measured at 655 nm. What is this measurement in centimeters?
a.
6.55 cm
b.
0.00655 cm
c.
6.55 x 10−5 cm
d.
6.55 x 10−7 cm
e.
6.55 x 10−9 cm
2. The liquid 1,2-ethanedithiol is insoluble in water. If a 75.5-g sample of 1,2-ethanedithiol has a volume of 61.2 mL, what is its density, and would it float or sink if poured into a beaker containing water?
a.
1.23 g/mL and it would sink in water
b.
1.23 g/mL and it would float on water
c.
0.811 g/mL and it would sink in water
d.
0.811 g/mL and it would float on water
3. A general chemistry student found a chunk of metal in the basement of a friend’s house. She measured the mass of the metal to be 238.7 g. Then she dropped the metal into a graduated cylinder containing 35.0 mL of water, and the water level rose to 47.3mL. Of the following metals, which one did she use?
a.
Aluminum, d = 2.72 g/mL
b.
Silver, d = 10.50 g/mL
c.
Lead, d = 11.34 g/mL
d.
Tungsten, d = 19.38 g/mL
e.
Platinum, d = 21.46 g/mL
4. An empty Erlenmeyer flask weighs 241.3 g. When filled with water (density = 0.997 g/mL), the flask and its contents weigh 489.1 g. What volume of water does the flask hold?
a.
246. mL
b.
247. mL
c.
248. mL
d.
249. mL
e.
241. mL
5. What is the correct answer to the expression below?
=
a.
8.63 cm
b.
8.6369 cm
c.
8.6 cm
d.
8.636 cm
e.
8 cm
6. The specific heat of ice is 0.492 cal/(g × °C). How many calories of heat are required to raise 100.0 g of ice from -20.0 °C to -0.5 °C?
a. 2.52 cal
b. 10.4 cal
c. 49.2 cal
d. 959 cal
e. 3960 cal
7. An Indy race car can travel 111 m/s. What is the speed of the car in miles per hour? (Given: 1 mi = 1.61 km, and 1 h = 3600 s)
a. 111 mi/h
b. 178 mi/h
c. 248 mi/h
d. 400 mi/h
e. 643 mi/h
8. Calculate the length of a copper wire having a diameter of 0.200 cm and a mass of 15.620 g. The density of copper is 8.92 g/cm3. (Given: volume = πd2 L/4, where π = 3.14, d = diameter, and L = length)
a. 1.80 × 10-4 cm
b. 4.00 × 10-4 cm
c. 5.50 × 10-2 cm
d. 1.75 cm
e. 55.8 cm
9. At which of the following temperatures is it most economical to fill a gas tank?
a. 50 °C
b. 40 °C
c. 30 °C
d. 20 °C
e. 10 °C
10. Element Y has two natural isotopes: Y-63 (62.940 amu) and Y-65 (64.928 amu). Calculate the atomic mass of element Y given the abundance of Y-63 is 69.17%.
a. 63.55 amu
b. 64.00 amu
c. 64.32 amu
d. 107.85 amu
e. 108.46 amu
11. For the following reaction, 4.57 g of silver nitrate (Molar Mass = 169.88 g/mol) are mixed with excess copper. The reaction yields 2.29 g of copper(II) nitrate (Molar Mass = 187.57 g/mol). What is the percent yield for this reaction?
2 AgNO3(aq) + Cu(s) ? Cu(NO3)2 (aq) + 2 Ag(s)
a.
45.3%
b.
50.1%
c.
67.8%
d.
73.8%
e.
90.9%
12. How many grams of nickel are present in 3.89 g of nickel(II) iodide?
a.
0.138 g Ni
b.
0.731 g Ni
c.
1.23 g Ni
d.
1.30 g Ni
e.
2.07 g Ni
13. How many grams of silver will be formed when 27.9 g of copper reacts with
excess silver nitrate, according to the balanced equation below?
2AgNO3 + Cu ? Cu(NO3)2 + 2Ag
a.
8.22 g
b.
23.7 g
c.
32.9 g
d.
47.4 g
e.
94.7 g
14. What is the maximum amount of carbon dioxide which can be formed if 15.2 g of glucose, C6H12O6 (molar mass = 180.18 g/mol) is allowed to react with 22.5 g of oxygen, O2?
C6H12O6 + 6O2 ? 6CO2 + 6H2O
a.
19.2 g
b.
20.6 g
c.
22.3 g
d.
26.4 g
e.
30.9 g
15. 61.8 g of potassium hydroxide is allowed to react with 33.8 g of phosphoric acid, according to the following reaction:
3 KOH(aq) + H3PO4(aq) ? K3PO4(aq) + 3 H2O(l)
What is the theoretical yield of potassium phosphate for this reaction?
a.
15.6 g
b.
16.3 g
c.
73.2 g
d.
77.9 g
e.
233.8 g
16. An oxide of nitrogen contains 74.1% oxygen and has a molar mass of 108 g/mol. What is the molecular formula for this compound?
a.
N2O5
b.
N2O3
c.
N2O4
d.
N2O0
e.
N2O2
17. Butyric acid, found in rancid butter, has a molar mass of 88 g/mol. If butyric acid is 54.5% C, 9.09% H and 36.4% O, what is the molecular formula?
a.
C4H8O2
b.
C8H12O4
c.
C2H4O
d.
C12H6O
e.
CHO2
18. When 2.34 g of pure iron is allowed to react with an excess of oxygen, 3.35 g of the final compound is produced. Determine the formula of the compound.
a.
Fe2O3
b.
FeO2
c.
FeO4
d.
FeO3
e.
FeO
19. You need to make an aqueous solution of 0.139 M aluminum nitrate, Al(NO3)3, for an experiment in the lab, using a 300. mL volumetric flask. How much solid aluminum nitrate (Molar Mass = 213.012 g/mol) should you add?
a.
0.0101 g
b.
0.0417 g
c.
1.96 g
d.
8.88 g
e.
98.7 g
20. How many grams of Ag2CO3 (Molar mass = 275.75 g/mol) will precipitate when excess (NH4)2CO3 is added to 75.0 mL of 0.742 M AgNO3 solution?
2 AgNO3(aq) + (NH4)2CO3(aq) ? Ag2CO3(s) + 2 NH4NO3(aq)
a.
0.202 g
b.
3.87 g
c.
7.67 g
d.
13.6 g
e.
15.3 g
21. In the laboratory you dissolved 19.7 g of barium nitrate, Ba(NO3)2, in a volumetric flask and added water to a total volume of 125 mL. What is the concentration of the nitrate ion in solution?
a.
0.0754 M
b.
0.603 M
c.
0.791 M
d.
1.21 M
e.
1.58 M
22. You wish to make a 0.339 M H2SO4 solution from a stock solution of 12.0 M H2SO4. How much concentrated acid must you add to obtain a total volume of 100.00 mL of the dilute solution?
a.
0.708 mL
b.
1.77 mL
c.
2.83 mL
d.
3.54 mL
e.
5.65 mL
23. A helium-filled weather balloon has a volume of 652 L at 18 oC and 756 mm Hg. It is released and rises to an altitude of 6.55 km, where the pressure is 398 mm Hg and the temperature is –22 oC. The volume of the balloon at this altitude is
a.
1070 L
b.
1220 L
c.
1260 L
d.
1440 L
e.
1510 L
24. A sample of carbon dioxide gas at 291 K and 1.26 atm occupies a volume of 3.60 L. If the gas is allowed to expand to a larger volume, while at the same time it is heated to a higher temperature, the final gas pressure
a.
will be 1.26 atm.
b.
will be higher than 1.26 atm.
c.
will be lower than 1.26 atm.
d.
could be higher or lower than 1.26 atm depending on the final volume and temperature.
25. A 2.00-L glass soda bottle filled only with air is tightly capped at 24 °C and 720.0 mm Hg. If the bottle is placed in water at 89 °C, what is the pressure in the bottle?
a.
194 mm Hg
b.
878 mm Hg
c.
2670 mm Hg
d.
591 mm Hg
e.
414 mm Hg
26. How many propane molecules are in 22.4 liters of C3H8 gas at STP?
a. 1.20 × 1024
b. 1.35 × 1025
c. 1.81 × 1024
d. 6.02 × 1023
e. 2.69 × 1022
27. A common name for galactose is cerebrose, or brain sugar. What is the molecular formula of galactose if the empirical formula is CH2O, and the approximate molar mass is 180 g/mol?
a. CHO
b. CH2O
c. CH2O6
d. C6H12O6
e. C12H22O11
28. The insulating and packing material Styrofoam is a polymer of styrene. Find the molecular formula of styrene given its percent composition: 92.25% C, 7.75% H. The approximate molar mass of styrene is 104 g/mol.
a. CH
b. CH8
c. CH12
d. C8H8
e. C12H
29. Starting with 1.56 g of salicylic acid, a student prepares 1.75 g of aspirin. If the calculated mass of aspirin is 1.88 g, what is the percent yield?
a. 83.0%
b. 89.1%
c. 93.1%
d. 107%
e. 121%
30. The reaction for plant photosynthesis of glucose sugar and oxygen gas is:
__CO2(g) + __H2O(l) __C6H12O6(s) + __O2(g)
What is the volume of oxygen gas at STP produced from 2.20 g of CO2?
a. 0.187 L
b. 1.12 L
c. 1.60 L
d. 4.32 L
e. 6.72 L
31. A sample of laughing gas, N2O, occupies 0.250 L at 14.7 psi and -80.0 °C. If the volume of the gas is 0.375 L at 25.0 °C, what is the pressure?
a. 6.35 psi
b. 14.3 psi
c. 15.1 psi
d. 31.4 psi
e. 34.0 psi
32. An unknown gas occupies a volume of 4.75 L at 1227 °C and 5.00 atm. If the mass is 5.45 g, what is the molar mass of the gas? (R = 0.0821 atm?L/mol?K)
a. 21.5 g/mol
b. 23.8 g/mol
c. 28.3 g/mol
d. 141 g/mol
e. 344 g/mol
33. A sample of helium gas is at a temperature of 100 K. If both the volume and pressure each double, what is the final Kelvin temperature?
a. 25 K
b. 50 K
c. 100 K
d. 200 K
e. 400 K
34. Ammonia gas decomposes according to the equation:
2NH3(g) → N2(g) + 3H2(g)
If 15.0 L of nitrogen is formed at STP, how many liters of hydrogen will be produced (also measured at STP)?
a. 15.0 L
b. 30.0 L
c. 45.0 L
d. 90.0 L
e. not enough information
35. If the solubility of sodium acetate (Molar mass = 82 g/mol) is 76 grams per 100 grams of water, which of the following solutions would be considered supersaturated?
a. 8.5 moles of sodium acetate dissolved in 1 L of water
b. 5.5 moles of sodium acetate dissolved in 500 mL of water
c. 1.8 moles of sodium acetate dissolved in 300 mL of water
d. 1.2 moles of sodium acetate dissolved in 200 mL of water
e. none of the above
36. How many grams of a 23.4% by mass NaF solution is needed if you want to have of NaF?
a. 55.9
b. 31.1
c 13.1
d. 239
e. none of the above
37. What mass of a 29.0% by mass glucose, C6H12O6, solution contains 60.0 g of glucose?
a.
52.2 g
b.
207 g
c.
17.4 g
d.
96.7 g
e.
60.0 g
38. The Olympic Games shot put field event uses a 16 pound (lb) shot. Identify the correct solution map to convert from pounds to kilograms using prefix multipliers and the given conversions of 16 0z = 1 lb and
453.6 g = 16 oz.
a. 16 lb × × ×
b. 16 lb × × ×
c. 16 lb × × ×
d. 16 lb × × ×
39. From the following list of substances and heat capacities, choose the one that will have the lowest temperature after absorbing 100.0 kJ of heat. Assume identical masses of each substance start at the same initial temperature.
a. lead-0.128 J/g?°C
b. copper-0.385 J/g?°C
c. ethanol-2.42 J/g?°C
d. water-4.18 J/g?°C
e. not enough information
40. You have 10.0 g each of Na, C, Pb, Cu and Ne. Which contains the smallest number of moles?
a. Na
b. C
c. Pb
d. Cu
e. Ne
41. Which of the following contains 9.02 × 1023 atoms?
a. 4.00 g H2
b. 9.00 g H2O
c. 28.0 g N2
d. 32.0 g O2
e. none of the above
42. The mineral mimetite has the formula Pb5(AsO4)3Cl. What mass percent of oxygen does it contain?
a.
38.70 %
b.
16.34 %
c.
50.32 %
d.
12.90 %
e.
1.08 %
43. Which of the following is a product of α decay of U?
a.
Th
b.
Np
c.
Pa
d.
U
e.
Pu
44. If Pb undergoes a beta decay and the product of this decay undergoes another beta decay, which nuclide is produced?
a.
Bi
b.
Pb
c.
Po
d.
Bi
e.
Pb
45. Identify the missing particle in the following nuclear equation: Am + He → __________ + 2 n
a.
Bk
b.
Bk
c.
Bk
d.
Bk
e.
Bk
46. The I-131 nuclide has a half-life of 8.0 days. If you originally have a 1.8-kg sample on May 1st of a certain year, approximately how much will you have on June 1st of the same year?
a.
95 g
b.
56 g
c.
225 g
d.
113 g
e.
less than 50 g
47. What is the best answer to report for ?
a.
3.236
b.
3.2361
c.
3.2
d.
3.24
e.
3.23615
48. A car averages 25.0 miles per gallon of gasoline. How many liters of gasoline will be needed for a trip of 575 km? Some conversion factors that may be helpful are the following:
1 qt = 0.946 L 1 mile = 1.609 km 4 qt = 1 gal (exact) 1 ft = 12 in (exact)
a.
5 × 101 L
b.
6 × 103 L
c.
2 × 103 L
d.
1 × 102 L
e.
3 × 104 L
49. An irregularly shaped metal was weighed by the following difference:
Watch glass + metal = 56.7813 g Watch glass = 35.4725 g
The volume of the metal was determined by placing the metal in a graduated cylinder that had water in it and measuring the volume difference.
Graduated cylinder + water + metal = 14.15 mL
Graduated cylinder + water = 11.25 mL
The density should be reported as
a.
7.348 g/mL.
b.
7.35 g/mL.
c.
7.4 g/mL.
d.
7.3 g/mL.
e.
7.3479 g/mL.
50. Which of the following sequence of conversions will yield the correct number of scruples in 66.1 lb? Some equivalents that may be helpful are given below:
1.00 scruple = 20.0 grains 1.00 g = 15.4 grains 1.00 grain = 0.0648 g 1.00 lb = 453.6 g
1.00 kg = 2.205 lb
a.
b.
c.
d.
e.
¾
¾
¾
¾
¾
¾
®
¾
l
chlorophyl
/
UV
