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Test #4: Take Home
Introductory to Chemistry: CHEM 1405
Directions: Choose the best answer to the following multiple choice questions
1) BALANCE the equation first. Fecl3 + O2 → Fe2O3 + Cl2
What is the limiting reactant?
A) Fecl3
B) O2
C) Fe2O3
D) Cl2
E) none of the above
2) Use the following BALANCED equation. 2 C2H6 + 7 O2 4 CO2 + 6 H2O
Identify the limiting reactant.
A) C2H6
B) O2
C) CO2
D) H2O
E) none of the above
3) Consider the following reaction: 2 CuCl2 + 4 KI → 2 CuI + 4 KCl + I2
When 0.56 moles of CuCl2 reacts with 0.64 moles of KI, how many moles
of I2 are formed? What is the limiting reactant
A) o.75moles I2 and KI
B) 0.16moles I2 and CuCl2
C) 0.16moles I2 and KI
D) 4moles I2 and 4 KCl
E) none of the above
4) Considering the limiting reactant, what is the volume of NO gas produced from 30.0 L of
nitrogen gas and 20.0 L of oxygen gas? (Assume constant conditions.)
N2(g) + O2(g)
A) 20.0 L
B) 30.0 L
C) 40.0 L
D) 60.0 L
E) none of the above
2 NO(g)
5) Considering the limiting reactant, what is the volume of NO2 gas produced from 3.00 L of
NO gas and 2.00 L of oxygen gas? (Assume constant conditions.)
2 NO(g) + O2(g)
2 NO2(g)
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A) 1.00 L
B) 2.00 L
C) 3.00 L
D) 4.00 L
E) none of the above
6) Considering the limiting reactant, what is the volume of NO gas produced from 40.0 L of
ammonia gas and 40.0 L of oxygen gas? (Assume constant conditions.)
4 NH3(g) + 5 O2(g)
A) 32.0 L
B) 40.0 L
C) 50.0 L
D) 80.0 L
E) none of the above
4 NO(g) + 6 H2O(g)
7) Which of the following is an observed property of gases?
A) gases have a variable shape
B) gases expand uniformly
C) gases compress uniformly
D) gases mix uniformly
E) all of the above
8) Which of the following is not an observed property of gases?
A) gases have a variable shape
B) gases expand uniformly
C) gases compress and liquefy
D) gases have a high density
E) gases mix uniformly
9) Which of the following is not an observed property of gases?
A) gases have a variable volume
B) gases expand to fill the container
C) gases compress infinitely
D) gases have a low density
E) gases mix uniformly
10) A sample of neon gas at 1.20 atm compresses from 0.250 L to 0.125 L. If the temperature
remains constant, what is the final pressure in atm?
A) 0.600 atm
B) 1.00 atm
C) 1.20 atm
D) 2.40 atm
E) none of the above
11) A sample of argon gas at 520 mm Hg expands from 0.150 L to 0.300 L. If the temperature
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remains constant, what is the final pressure in mm Hg?
A) 260 mm Hg
B) 520 mm Hg
C) 760 mm Hg
D) 1040 mm Hg
E) none of the above
12) A sample of krypton gas at 75.0 psi and 100 °C expands from 0.100 L to 0.450 L. Ifthe
temperature remains constant, what is the final pressure in psi?
A) 0.167 psi
B) 3.38 psi
C) 16.7 psi
D) 75.0 psi
E) 338 psi
13) A 5.00 L volume of methane gas is cooled from 298 K to 149 K. If the pressure remains
constant, what is the final volume in liters?
A) 2.50 L
B) 4.58 L
C) 5.00 L
D) 5.46 L
E) 10.0 L
14) A 5.00 L volume of ethane gas is heated from 298 K to 596 K. If the pressure remains
constant, what is the final volume in liters?
A) 2.50 L
B) 4.58 L
C) 5.00 L
D) 5.46 L
E) 10.0 L
15) A 5.00 mL volume of methane gas is cooled from 60.0 °C to 30.0 °C. If the pressure remains
constant, what is the final volume in milliliters?
A) 2.50 mL
B) 4.55 mL
C) 5.00 mL
D) 5.50 mL
E) 10.0 mL
16) A sample of air at 7.50 atm is cooled from 448K to 224K. If the volume remains constant,
what is the final pressure?
A) 3.75 atm
B) 4.57 atm
C) 6.15 atm
D) 12.3 atm
E) 15.0 atm
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17) A sample of air at 7.50 atm is heated from 224K to 448K. If the volume remains constant,
what is the final pressure?
A) 3.75 atm
B) 4.57 atm
C) 6.15 atm
D) 12.3 atm
E) 15.0 atm
18) The pressure of an air sample at 190 K increases from 415 mm Hg to 830 mm Hg. What is
the final Kelvin temperature if the volume remains constant?
A) -42K
B) -166K
C) 95K
D) 380K
E) 653K
19) A sample of xenon gas at 786 mm Hg is cooled from 100.0 °C to 50.0 °C. If the volume
remains constant, what is the final pressure?
A) 153 mm Hg
B) 393 mm Hg
C) 681 mm Hg
D) 908 mm Hg
E) 1570 mm Hg
20) If 5.00 L of argon gas is at 0.460 atm and -123 °C, what is the volume at STP?
A) 4.19 L
B) 4.94 L
C) 5.06 L
D) 5.49 L
E) 5.97 L
21) If a 50.0 mL sample of xenon gas is at 0.921 atm and 27 °C, what is the volume of the gas at
STP?
A) 41.9 mL
B) 49.4 mL
C) 50.6 mL
D) 54.9 mL
E) 59.7 mL
22) If 7.75 L of radon gas is at 1.55 atm and -19 °C, what is the volume at STP?
A) 4.65 L
B) 5.37 L
C) 8.33 L
D) 11.2 L
E) 12.9 L
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23) How many moles of helium occupy a volume of 5.00 L at 227.0 °C and 5.00 atm? (R =
0.0821 atm•L/mol•K)
A) 0.609 mol
B) 1.64 mol
C) 5.00 mol
D) 25.0 mol
E) 6090 mol
24) If 1.06 mol of helium exert a pressure of 0.750 atm at 210.0 °C, what is the volume in liters?
(R = 0.0821 atm•L/mol•K)
A) 0.00155 L
B) 24.4 L
C) 28.1 L
D) 56.0 L
E) 4160 L
25) If 0.250 mol of hydrogen gas occupies 0.333 L at 20.0 °C, what is the pressure in
atmospheres? (R = 0.0821 atm•L/mol•K)
A) 0.00554 atm
B) 1.23 atm
C) 18.1 atm
D) 32.0 atm
E) 4750 atm
26) Which of the following statements is true regarding an ionic bond?
A) Metal atoms lose electrons and nonmetal atoms gain electrons.
B) An ionic bond is the attraction between a metal ion and a nonmetal ion.
C) The ionic radius of a metal ion is less than its atomic radius.
D) Breaking an ionic bond between two ions requires energy.
E) all of the above
27) Which of the following statements is true regarding an ionic bond in FeS?
A) Iron atoms gain electrons and sulfur atoms lose electrons.
B) Iron and sulfur ions bond by electrostatic attraction.
C) The ionic radius of an iron ion is equal to its atomic radius.
D) Breaking an ionic bond between Fe2+ and S2- releases energy.
E) none of the above
28) Which of the following statements is true regarding a covalent bond in HCl?
A) Valence electrons are shared between the hydrogen and chlorine atoms.
B) The bond length is equal to the sum of the two atomic radii.
C) Breaking the bond between H-Cl releases energy.
D) all of the above
E) none of the above
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29) Draw the electron dot formula for ammonia, NH3. How many nonbonding electron pairs are
in an ammonia molecule?
A) 1
B) 2
C) 3
D) 6
E) none of the above
30) What is the mass of insoluble lead(II) iodide (461.0 g/mol) produced from 0.830 g of
potassium iodide (166.00 g/mol) and aqueous lead(II) nitrate?
__Pb(NO3)2(aq) + __KI(s) → __PbI2(s) + __KNO3(aq)
A) 0.149 g
B) 0.598 g
C) 1.15 g
D) 2.31 g
E) 4.61 g
31) How many moles of oxygen gas react with 0.100 mol of pentane, C5H12?
__C5H12 (g) + __O2(g)
A) 0.100 mol
B) 0.500 mol
C) 0.600 mol
D) 0.800 mol
E) none of the above
__CO2(g) + __H2O(g)
32) How many moles of water are produced from 0.100 mol pentane, C5H12?
__C5H12 (g) + __O2(g)
A) 0.100 mol
B) 0.500 mol
C) 0.600 mol
D) 0.800 mol
E) none of the above
__CO2(g) + __H2O(g)
33) How many moles of oxygen gas react to yield 0.100 mol water?
__C5H12 (g) + __O2(g)
A) 0.100 mol
B) 0.500 mol
C) 0.600 mol
D) 0.800 mol
E) none of the above
__CO2(g) + __H2O(g)
34) In an experiment, 0.520 g of chromium metal reacts with 3.807 g of iodine. Using the
conservation of mass law, predict the mass of product.
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2 Cr(s) + 3 I2(s)
A) 1.529 g
B) 3.287 g
C) 4.327 g
D) 8.654 g
E) 12.461 g
2 CrI3(s)
35) In an experiment, 0.243 g of magnesium reacts to give 0.403 g magnesium oxide. Using the
conservation of mass law, predict the mass of reacting oxygen gas.
2 Mg(s) + O2(g)
A) 0.080 g
B) 0.160 g
C) 0.320 g
D) 0.646 g
E) 1.292 g
2 MgO(s)
36) In an experiment, 0.327 g of zinc metal reacts to produce 0.407 g of zinc oxide. Using the
conservation of mass law, predict the mass of reacting oxygen gas.
2 Zn(s) + O2(g)
A) 0.040 g
B) 0.080 g
C) 0.160 g
D) 0.734 g
E) 1.468 g
2 ZnO(s)
37) What is the volume of oxygen gas at STP from the decomposition of 10.8 g of mercuric
oxide (216.59 g/mol)?
__HgO(s)
A) 0.558 L
B) 1.12 L
C) 2.23 L
D) 52.2 L
E) 209 L
__Hg(l) + __O2(g)
38) What is the mass of mercuric oxide (216.59 g/mol) that decomposes to release 0.750L of
oxygen gas at STP?
__HgO(s)
A) 0.0388 g
B) 0.155 g
C) 3.63 g
D) 7.25 g
E) 14.5 g
__Hg(l) + __O2(g)
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39) What volume of oxygen gas reacts to produce 30.0 L of sulfur trioxide gas?
(Assume temperature and pressure remain constant.)
__SO2(g) + __O2(g)
A) 10.0 L
B) 15.0 L
C) 30.0 L
D) 60.0 L
E) none of the above
__SO3(g)
40) What volume of hydrogen gas reacts with 12.0 mL of nitrogen gas?
(Assume temperature and pressure remain constant.)
__N2(g) + __H2(g)
A) 4.00 mL
B) 6.00 mL
C) 24.0 mL
D) 36.0 mL
E) none of the above
41.
__NH3(g)
Which variable is not used to describe the amounts and properties of gases?
a) temperature b) pressure c) compressibility d) volume d) number of molecules present
42.
The statement "At constant temperature, the volume occupied by a definite mass of a gas
is inversely proportional to the applied pressure." is a statement of _______ Law.
a) Charles's
b) Boyle's c) Graham's d) Avogadro's
e) Gay-Lussac's
43.
The statement "At constant pressure, the volume occupied by a definite mass of a gas is
directly proportional to the absolute temperature." is a statement of _______ Law.
(a) Charles's b) Boyle's c) Graham's d) Avogadro's
e) Gay-Lussac's
2.00 g of fluorine occupies 1.18 L at STP. What volume will it occupy at –14oC and
1 atm?
(a) 1.20 L
(b) 2.73 L
(c) 5.89 L
(d) 1.12 L
(e) 6.20 L
44.
45.
A gas sample occupies 1.00 L at 120.°C and 1.00 atm. What volume will it occupy at
STP?
a) 1.14 L
(b) 1.44 L
(c) 0.846 L
(d) 0.782 L
(e) 0.695 L
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