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 = πr2h).
A.
0.500 cm
B.
0.774 cm
C.
0.536 cm
D.
0.533 cm
E.
0.882 cm


2.
What is the total coefficients when the following reaction is balanced using whole-number coefficients?  
         TiO2   +    C +    Cl2 →    TiCl4 +    CO2 +    CO
A.
13
B.
12
C.
15
D.
14
E.
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.
1
B.
2
C.
3
D.
1.5
E.
4


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.
1.28 M
B.
0.153 M
C.
1.53 M
D.
0.168 M
E.
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.
1.22 g/cm3
B.
0.432 g/cm3
C.
0.864 g/cm3
D.
1.63 g/cm3
E.
2.21 g/cm3


6.
Convert 31 picometer (pm) to nanometer (nm).
A.
3.1 x 10-3
B.
3.1 x 10-2
C.
3.1 x 10-9
D.
3.1 x 10+3
E.
3.1 x 10+9


7.
Which of the following is an illustration of the law of definite propotion?
A.
Water is 11% hydrogen and 89% oxygen by mass.
B.
Water boils at 100 °C at 1 atm pressure.
C.
Water can be separated into other substances by a chemical process.
D.
Water and salt have different boiling points.
E.
Water consists hydrogen and oxygen molecules.


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.
1.0 × 101
B.
9.99224
C.
9.9922
D.
9.992
E.
1.00 × 101


9.
Which one of the following compounds can be considered non-electrolyte?
A.
Hydrofluoric acid (HF)
B.
Ethyl amine (C2H5NH2)
C.
Ethanol(CH3CH2OH)
D.
Acetic Acid (CH3COOH)
E.
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.
No reaction occurs
B.
Cu2+(aq) + S2-(aq)   → CuS(s)
C.
Li+(aq) + S2-(aq) + Cu+(aq) + NO3-(aq) → CuS(s) + Li+(aq) + NO3-(aq)
D.
Li+(aq) + S-(aq) + Cu+(aq) + NO3-(aq) → CuS(s) + LiNO3(aq)
E.
2Li+(aq) + S2-(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.
4
B.
2
C.
1
D.
3
E.
8


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.
1.60 g
B.
2.40 g
C.
0.399 g
D.
7.99 g
E.
0.160 g


13.
What is the formula for the ionic compound formed by aluminum and sulfide    
    ions?
A.
AlSO4
 
 
B.
AlS3
C.
Al2S3
D.
Al2(SO3)3
E.
Al3SO4


14.
If the Thomson model of the atom had been correct, Rutherford would have observed
A.
Alpha particles going through the gold foil with no deflection.
B.
Alpha particles greatly deflected by the gold foil.
C.
Alpha particles bouncing off the gold foil.
D.
Positive particles formed in the gold foil.
E.
A hole formed in the foil because of the penetration of alpha particles.


15.
Which of the following are allotropes?
A.
oxygen and sulfur
B.
hydrogen and deuterium
C.
bromine and chlorine
D.
water (H2O) and hydrogen peroxide (H2O2)
E.
diamond and graphite


16.
The elements in groups 1A, 6A, and 7A are called ________, respectively.
A.
alkali metals, chalcogens, and halogens
B.
alkaline earth metals, halogens, and chalcogens
C.
alkali metals, halogens, and noble gases
D.
alkaline earth metals, transition metals, and halogens
E.
halogens, transition metals, and alkali metals


17.
What is the formula mass (in amu) of calcium phosphate compound?
A.
340.
B.
279
C.
215
D.
310.
E.
170.


18.
A compound of oxygen and titanium contains 59.9 % Ti by mass. The empirical formula of this compound is
A.
TiO3
B.
Ti2O4
C.
Ti3O4
D.
Ti2O3
E.
TiO2


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.
172
B.
343
C.
282.
D.
340.
E.
232


20.
A 22.5-g sample of ammonium carbonate contains ________ mol of ammonium ions.
A.
0.288
B.
0.468
C.
0.234
D.
2.14
E.
3.47


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