Name: __________________________ Date: _____________
1. A cylindrical glass tube with 12.7 cm in length is filled with mercury (density = 13.6
g/mL). The mass of mercury needed to fill the tube is 105.5 g. Calculate the inner
diameter of the tube (volume of a cylinder of radius r and length h is Vcylinder = r2h).
A)
B)
C)
D)
E)
0.882 cm
0.774 cm
0.536 cm
0.533 cm
0.500 cm
2. What is the total coefficients when the following reaction is balanced using
whole-number coefficients?
TiO2 +
C +
Cl2 →
TiCl4 +
CO2 +
CO
A)
B)
C)
D)
E)
14
12
15
13
16
3. Find the empirical formula of an organic compound from the following composition
34.62 % C, 3.88 % H and 61.50 % O.
Then, determine how many moles of CO2(g) will be produced when one mole of this
compound reacts with excess O2(g).
A)
B)
C)
D)
E)
3
2
1
1.5
4
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4. A 15.00 mL solution of NaCl was diluted to 125.0 mL. A 25.00 mL of this solution
was diluted further to 1.000 L. The concentration of the final solution is 0.00383 M.
Calculate the concentration of the original solution.
A)
B)
C)
D)
E)
1.28 M
0.153 M
1.53 M
0.168 M
2.25 M
5. A 32.65 g sample of a solid is placed in a flask. Toluene, in which the solid is
insoluble, is added to the flask so that the total volume of solid and liquid together is
50.00 mL. The solid and solution weigh 58.58 g. The density of toluene is 0.864
g/mL. What is the density of the solid?
A)
B)
C)
D)
E)
1.63 g/cm3
0.432 g/cm3
0.864 g/cm3
1.22 g/cm3
2.21 g/cm3
6. Convert 31 picometer (pm) to nanometer (nm).
A)
B)
C)
D)
E)
3.1 x 10-2
3.1 x 10-3
3.1 x 10-9
3.1 x 10+3
3.1 x 10+9
7. Which of the following is an illustration of the law of definite propotion?
A)
B)
C)
D)
E)
Water is 11% hydrogen and 89% oxygen by mass.
Water boils at 100 °C at 1 atm pressure.
Water can be separated into other substances by a chemical process.
Water and salt have different boiling points.
Water consists hydrogen and oxygen molecules.
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8. For the following calculation:
(12.67 + 19.2)(3.99) / (1.36 + 11.366) = ________
the correct answer (reported to the correct number of significant figures) is
A)
B)
C)
D)
E)
1.00 × 10
9.99224
9.9922
9.992
1
1.0 × 10
1
9. Which one of the following compounds can be considered non-electrolyte?
A)
B)
C)
D)
E)
Ethanol(CH3CH2OH)
Ethyl amine (C2H5NH2)
Hydrofluoric acid (HF)
Acetic Acid (CH3COOH)
Ammonia (NH3)
10. Give the net ionic equation for the reaction (if any) that occurs when aqueous solutions
of lithium sulfide and copper (II) nitrate are mixed.
A)
B)
C)
D)
E)
2+
2-
Cu (aq) + S (aq) → CuS(s)
No reaction occurs
2+
Li+(aq) + S (aq) + Cu+(aq) + NO3-(aq) → CuS(s) + Li (aq) + NO3 (aq)
Li+(aq) + S-(aq) + Cu+(aq) + NO3 (aq) → CuS(s) + LiNO3(aq)
22Li+(aq) + S (aq) → Li2S(s)
11. Citric acid has the molecular formula C6H8O7. A 0.250 g sample of citric acid
dissolved in 25.0 mL of water requires 37.2 mL of 0.105 M NaOH for complete
neutralization. What number of acidic hydrogens per molecule does citric acid have?
A)
B)
C)
D)
E)
3
2
1
4
8
Page 3
12. Rust [Fe2O3(s)] can be removed by oxalic acid. Calculate the number of grams of
Fe2O3(s) which can be removed by 1.00 x 102 mL of a 0.150 M solution of oxalic acid
H2C2O4.
Fe2O3(s) + 6H2C2O4(aq) → 2Fe(C2O4)33-(aq)+ 3H2O +6H+(aq)
A)
B)
C)
D)
E)
0.399 g
2.40 g
16.0 g
7.99 g
0.160 g
13. What is the formula for the ionic compound formed by aluminum and sulfide
ions?
A)
B)
C)
D)
E)
Al2S3
AlS3
AlSO4
Al2(SO3)3
Al3SO4
14. If the Thomson model of the atom had been correct, Rutherford would have observed
A)
B)
C)
D)
E)
Alpha particles going through the gold foil with no deflection.
Alpha particles greatly deflected by the gold foil.
Alpha particles bouncing off the gold foil.
Positive particles formed in the gold foil.
A hole formed in the foil because of the penetration of alpha particles.
15. Which of the following are allotropes?
A)
B)
C)
D)
E)
diamond and graphite
hydrogen and deuterium
bromine and chlorine
water (H2O) and hydrogen peroxide (H2O2)
oxygen and sulfur
Page 4
16. The elements in groups 1A, 6A, and 7A are called ________, respectively.
A)
B)
C)
D)
E)
alkali metals, chalcogens, and halogens
alkaline earth metals, halogens, and chalcogens
alkali metals, halogens, and noble gases
alkaline earth metals, transition metals, and halogens
halogens, transition metals, and alkali metals
17. What is the formula mass (in amu) of calcium phosphate compound?
A)
B)
C)
D)
E)
310.
279
215
340.
170.
18. A compound of oxygen and titanium contains 59.9 % Ti by mass. The empirical
formula of this compound is
A)
B)
C)
D)
E)
TiO2
Ti2O4
Ti3O4
Ti2O3
TiO3
19. Under appropriate conditions, nitrogen and hydrogen undergo a combination reaction to
yield ammonia:
N2 (g) + 3H2 (g) → 2NH3 (g)
If the reaction yield is 87.5%, how many grams of N2 are needed to produce 300. grams
of NH3?
A)
B)
C)
D)
E)
282
343
170.
340.
232
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20. A 22.5-g sample of ammonium carbonate contains ________ mol of ammonium
ions.
A)
B)
C)
D)
E)
0.468
0.288
0.234
2.14
3.47
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Answer Key
1.
2.
3.
4.
5.
6.
7.
8.
9.
10.
11.
12.
13.
14.
15.
16.
17.
18.
19.
20.
A
A
A
A
A
A
A
A
A
A
A
A
A
A
A
A
A
A
A
A
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