ISC 107 Practice Exam 1
Chapter 1 Matter - Its Properties and Measurement
1) A model that explains and makes predictions about natural phenomena is referred to as a:
A) natural law
B) hypothesis
C) theory
D) generalization
E) deduction
2) Which of the following is a physical property?
A) the density of lead
B) sulfur burns in oxygen to form sulfur trioxide
C) ozone reacts with silver to give silver oxide
D) platinum metal does not react with hydrochloric acid
3) Which of the following is a physical change?
A) the freezing of water to form ice
B) the burning of paper
C) the mixing of salt and water
D) the reaction of zinc with hydrochloric acid
E) the inability of gold to react with water
4) Oxygen is:
A) a mixture
B) a compound
C) an element
D) a solution
E) always combined with hydrogen
5) Which of the following is longest?
A) 3.0 nm
B) 300 pm
C) 3.0 × 10-4 m
D) 3.0 × 10-10 cm
E) 3.00 × 10-9 km
6) Convert 21.8 in3 to liters. (1.00 in = 2.54 cm and 1 mL = 1 cm3)
A) 0.0554 L
B) 1.33 × 103 L
C) 8.58 L
D) 0.357 L
E) 8.58 × 103 L
7) What mass, in g, of a solution containing 12% by mass sodium chloride is needed for a process that
requires 8 g of sodium chloride?
A) 12 g
B) 150 g
C) 67 g
D) 0.96 g
E) 8 g
8) Calculate the length of a steel cable (density 7.91 g/cm3) with a mass of 160.0 g and cross-sectional
area of 0.500 cm2.
A) 40.5 cm
B) 20.23 cm
C) 40.46 cm
D) 20.2 cm
E) 10.1 cm
Chapter 2 Atoms and the Atomic Theory
TRUE or FALSE?
1) Atoms retain their identity during a chemical reaction.
2) All matter is composed of atoms.
3) Atoms combine in small, whole-numbered ratios.
4) All atoms of a given element are identical.
5) Different ratios of atoms produce different compounds.
6) The number of protons and neutrons in the nucleus of a given atom is called the atomic number.
7) Isotopes have different atomic number (Z) but the same mass number (A).
8) The vertical columns in the periodic table of the elements are called groups.
9) A 25 g sample of sugar is found to contain 51.4% oxygen by mass. Another 250 g sample of the same
sugar is also 51.4% oxygen by mass. This is consistent with the:
A) law of conservation of mass
B) law of constant composition
C) law of multiple proportions
D) first assumption of Dalton's atomic theory
E) second assumption of Dalton's theory
10) Which of the following would be unaffected by an electric field?
A) alpha particles
B) beta particles
C) gamma rays
D) protons
E) electrons
11) What is the mass number of the most abundant form of oxygen atom?
A) 15.9994
B) 8
C) 16
D) 24
E) 32
12) 31.0 grams of the element phosphorus contain:
A) 6.02 × 1023 P4 molecules
B) 31.0 × (6.02 × 1023) P atoms
C) 6.02 × 1023 P atoms
D) 31.0 P atoms
E) 31.0 moles of P
13) How many arsenic atoms are in 5.21 g of arsenic?
A) 0.0695 atoms
B) 9.51 × 1022 atoms
C) 3.14 × 1024 atoms
D) 2.10 × 1022 atoms
E) 4.19 × 1022 atoms
14) A cubic centimeter of lead weighs 11.35 g. How many atoms are in the block?
A) 6.8 × 1024 atoms
B) 2.4 × 1023 atoms
C) 3.3 × 1022 atoms
D) 5.3 × 1022 atoms
E) 1.1 × 1025 atoms
15) How many moles are represented by 2.5 × 1015 Na atoms?
A) 3.8 × 10-10 mol
B) 1.8 × 10-10 mol
C) 1.5 × 1039 mol
D) 4.2 × 10-9 mol
E) 1.1 × 1014 mol
16) How many atoms of rubidium-85 are in 87.2 g of rubidium? Rubidium-85 is 72.2 % abundant.
A) 5.16 × 1046 atoms
B) 4.44 × 1023 atoms
C) 8.51 × 1023 atoms
D) 6.14 × 1022 atoms
E) 1.02 × 1024 atoms
17) What mass of magnesium is necessary to make 10.5 g of magnesium bromide if 1.04 g of
magnesium makes 7.88 g of magnesium bromide?
A) 1.39 g
B) 79.9 g
C) 1.58 g
D) 3.66 g
E) 7.89 g
18) The total numbers of neutrons, protons, and electrons in 31P3– are:
A) 15 neutrons, 31 protons, 15 electrons
B) 16 neutrons, 15 protons, 18 electrons
C) 31 neutrons, 15 protons, 18 electrons
D) 15 neutrons, 16 protons, 12 electrons
E) 16 neutrons, 16 protons, 18 electrons
19) Iodine is a member of the family called ________.
A) metals
B) metalloids
C) noble gasses
D) halogens
E) actinides
20) What is the mass of a sample containing 1.2 moles of Ni?
A) 49 g
B) 59 g
C) 34 g
D) 61 g
E) 70 g
21) 24.9 g of Mn is equivalent to how many moles of Mn?
A) 2.21 moles
B) 0.453 moles
C) 0.461 moles
D) 0.996 moles
E) 1.00 mole
22) What is the isotopic atomic mass of an isotope if 9.7023 × 1022 atoms weighs 4.0256 g?
A) 0.64858
B) 24.305
C) 24.986
D) 13.728
E) 4.0256
23) What is the atomic weight of an element if 4.00 grams of it contain 2.98 × 1022 atoms?
A) 20.2 u
B) 80.8 u
C) 19.7 u
D) 8.08 u
E) 2.02 u
Chapter 3 Chemical Compounds
1) A 10.0 g sample of bismuth tribromide, BiBr3, contains:
A) 5.360 × 1022 total number of ions
B) 0.322 mol BiBr3
C) 3.14 × 1022 formula units BiBr3
D) 1.34 × 1022 bromide ions
E) 4.020 × 1022 total number of ions
2) How many hydrogen atoms are present in 2.84 moles of water?
A) 3.42 × 1024 H atoms
B) 1.71 × 1024 H atoms
C) 4.24 × 1023 H atoms
D) 9.44 × 1024 H atoms
E) 3.42 × 1023 H atoms
3) Combustion analysis of a 22.0 mg sample of the painkiller morphine produced 13.2 mg of water.
What is the percentage by mass of hydrogen in morphine?
A) 6.71%
B) 3.36%
C) 13.4%
D) 60.0%
4) In which compound does iodine have an oxidation state of +3?
A) HIO3
B) IF5
C) Ca(IO2)2
D) HI
E) I2
5) Choose the INCORRECT oxidation state.
A) C is 0 in H2CO
B) S is +4 in H2SO3
C) C is +2 in HCOOH
D) Fe is +2 in Fe2O3
E) Mn is +7 in KMnO4
6) The name of which compound ends in -ite?
A) HIO3
B) Na2SO3
C) H2SO3
D) Na2CO3
E) CaH2
7) Choose the INCORRECT name formula combination.
A) Fe2O3 iron(III) oxide
B) H2SO3 sulfurous acid
C) NH4ClO3 ammonium chlorate
D) CaH2 calcium hydride
E) SiO2 silicon oxide
8) Choose the INCORRECT name/formula combination.
A) NaClO
sodium hypochlorite
B) NaClO4 sodium chlorate
C) NaClO2 sodium chlorite
D) Sr(IO3)2 strontium iodate
E) SCl4
sulfur tetrachloride
9) How many grams of K are found in 1.00 × 102 g of K2Cr2O7?
A) 18.3 g
B) 36.5 g
C) 53.2 g
D) 13.3 g
E) 26.6 g
10) Maprotiline, a tetracyclic drug prescribed for the treatment of depression, has the following mass
composition: C 86.56%, H 8.35%, and the rest is nitrogen..
The empirical formula of maprotiline is ________.
A) C7H8N3
B) C20H23N
C) C87H8N5
D) C3H3N
E) C14H14N
11) Elemental analysis of 50.0000 g of a compound showed that it contained 12.7520 g C, 3.2105 g H,
and the rest was S. The empirical formula of this compound is ________.
A) CHS
B) CH2S
C) CH3S
D) C2H2S
E) C2H3S2
12) An organic compound contains C, H, and O. The percentages of H and C are 6.73% H, and 39.99%
C by mass. The molar mass is 60.06 u. What is the molecular formula of the compound?
A) CH2O
B) C3H6O3
C) C2H3O2
D) C2H4O2
E) C4H8O4
13) What is the oxidation state of chlorine in sodium hypochlorite?
A) +1
B) -1
C) +2
D) +3
E) +5
14) The oxidation state of vanadium in VO+2 is ________.
A) -2
B) +2
C) +1
D) -4
E) +4
15) What is the formula of sodium hypochlorite?
A) NaCl
B) NaClO
C) NaClO2
D) NaClO3
E) NaClO4
16) The formula of barium nitride is ________.
A) Ba3N2
B) Ba2N2
C) BaN
D) Ba2N
Chapter 4 Chemical Reactions
1) When the equation Fe2(C2O4)3 → FeC2O4 + CO2 is balanced with the smallest integer coefficients,
the coefficient of CO2 is:
A) 1
B) 2
C) 4
D) 3
E) 5
2) When the equation CS2 + Cl2 → CCl4 + S2Cl2 is balanced with the smallest integer coefficients, the
sum of the coefficients is:
A) 5
B) 6
C) 4
D) 3
E) 7
3) For the reaction 2 Al + Fe2O3 → Al2O3 + 2 Fe, 2.5 g of Al (27.0 g/mol) and 7.2 g of
Fe2O3 (159.8 g/mol) produce how many g of Fe (55.9 g/mol)?
A) 2.5 (55.9/27.0) g
B) 2.5 (55.9)(2)/(27.0)(2) g
C) 7.2 (55.9)(2)/159.8 g
D) 7.2 (55.9/159.8) g
E) 2.5 (55.9/159.8) g
4) Which of the following represents a 1.00 M aqueous solution of glucose (C6H12O6)?
A) 90.0 g glucose per 500 mL water
B) 10.0 g glucose per 10.0 mL water
C) 0.180 g glucose per mL solution
D) 0.100 g glucose per mL solution
E) 4.5 g glucose per 4.5 g water
5) 45.8 mL of a 3.14 M sodium chloride solution were used to react completely with 50.0 mL of an
aqueous silver nitrate solution. What is the molarity of the silver nitrate solution?
A) 2.88 M
B) 1.50 M
C) 3.14 M
D) 3.42 M
E) 1.71 M
6) 52.5 mL of a solution were diluted to a volume of 6.25 L and then had a concentration of 3.16 M.
What was the molarity of the initial solution?
A) 3.16(52.5/6.25) M
B) 3.16(6.25/52.5) M
C) (3.16)(52.5)(6.25) M
D) 3.16(52.5/6250) M
E) (6.25)(3.16)/0.0525 M
7) If 5.97 mL of a solution of NaCl contains 2.54 mg of sodium ion, what is the molarity of the sodium
chloride solution?
A) 0.425 M
B) 1.85 × 10-2 M
C) 1.85 × 10-5 M
D) 7.28 × 10-3 M
E) 0.102 M
8) Given the reaction:
2 KMnO4 + 10 KI + 8 H2SO4 → 6 K2SO4 + 2 MnSO4 + 5 I2 + 8 H2O,
how many moles of K2SO4 are produced by allowing five moles each of KMnO4, KI, and H2SO4 to
react?
A) 3 mol
B) 1 mol
C) 2 mol
D) 4 mol
E) 5 mol
9) 42.6 g Cu are combined with 84.0 g of HNO3 according to the reaction:
3 Cu + 8 HNO3 → 3 Cu(NO3)2 + 2 NO + 4 H2O.
Which reagent is limiting and how many grams of Cu(NO3)2 are produced?
A) Cu, 93.8 g
B) HNO3, 93.8 g
C) Cu, 125.6 g
D) HNO3, 125.6 g
E) Cu(NO3)2, 125.6 g
10) What is the sum of the coefficients when the following is balanced with the smallest integer
coefficients?
PCl3(l) + Cl2(g) + P4O10(s) → POCl3(l)
A) 3
B) 18
C) 45
D) 10
E) 23
11) The molarity of a solution that contains 14.7 g of H2SO4 in 200.0 mL solution is ________.
A) 1.5 M
B) 0.75 M
C) 0.77 M
D) 7.4 M
E) 3.0 M
12) What mass of MgCl2 in grams must be added to 250.0 mL of a 0.25 M MgCl2 solution to produce a
0.40 M solution, assuming no change of volume upon addition?
A) 9.5 g
B) 6.0 g
C) 2.2 g
D) 3.6 g
E) 19 g
13) What is the percent yield if 185 grams of SiO2 are made from 328 g of Cr2O3 by the following
equation?
3 Si(s) + 2 Cr2O3(s) → 3 SiO2(s) + 4 Cr(l)
A) 142%
B) 70%
C) 56%
D) 105%
E) 95%
Chapter 5 Introduction to Reactions in Aqueous Solutions
1) Choose the INCORRECT statement.
A) A non-electrolyte is not ionized and does not conduct an electric current.
B) A strong electrolyte is completely ionized in water solution.
C) A strong electrolyte in solution is a good electrical conductor.
D) A weak electrolyte in solution is a good electrical conductor.
E) A weak electrolyte is partially ionized in a water solution.
2) To precipitate Cd2+ from solution one could add:
A) H2S(aq)
B) HCl(aq)
C) HNO3(aq)
D) KI(aq)
E) NaCl(aq)
3) Which of the following pairs of aqueous solutions will give a precipitate when mixed?
A) K3PO4 and CaCl2
B) LiClO4 and Ba(OH)2
C) AgNO3 and Ca(ClO4)2
D) NaCl and K(CH3COO)
E) Sr(NO3)2 and KI
4) The substance HI is a:
A) strong acid
B) weak base
C) strong base
D) salt
E) weak acid
5) Which of the following compounds is quite insoluble in water, but would liberate a gas when treated
with aqueous acetic acid?
A) K2CO3
B) K2SO4
C) CaCO3
D) CaSO4
E) AgCl
6) Among the following reactions, find those that are redox reactions:
1) MnO4- (aq) + 5 Fe2+ (aq) + 8 H+ → 5 Fe3+ (aq) + Mn2+ (aq) + 4 H2O(l)
2) 6 HF + Al(OH)3 + 3 NaOH → Na3AlF6 + 6 H2O
3) Au(s) + 4 H+ + NO3- + 4 Cl- → [AuCl4]- + 2 H2O + NO(g)
4) FeS + 2 HCl → FeCl2 + H2S
5) SiO2 + 4HF → SiF4 + H2O
A) reaction 1)
B) reaction 2)
C) reactions 1) and 3)
D) reactions 2) and 5)
E) reaction 4)
7) Write the net ionic equation for the reaction of barium chloride and sodium sulfate.
A) BaCl(aq) + NaSO4(aq) → BaSO4(s) + NaCl(aq)
B) BaCl(aq) + SO42- → BaSO4(s) + Ba2+
C) Ba2+ + SO42- → BaSO4(aq)
D) Ba2+ + SO42- → BaSO4(s)
E) no reaction
8) Balance the following equation for an oxidation-reduction reaction occurring in an acidic solution:
HCl + H2C2O4 + MnO2(s) → MnCl2 + CO2(g) + H2O
The sum of the coefficients is ________.
A) 7
B) 15
C) 45
D) 12
E) 9
9) Balance the following equation for an oxidation-reduction reaction occurring in an acidic solution:
HNO3 + I2 → HIO3 + NO2 + H2O
The sum of the coefficients is ________.
A) 26
B) 27
C) 28
D) 33
E) 45
10) What volume of 0.110 M H2SO4 is required to exactly neutralize 10.0 mL of 0.085 M NaOH?
A) 7.7 mL
B) 1.9 mL
C) 0.39 mL
D) 3.9 mL
E) 0.19 mL
Chapter 6 Gases
1) Convert 4.32 × 105 N/m2 to the equivalent pressure in atmospheres.
A) 4.26 atm
B) 4.38 × 1010 atm
C) 4.26 × 103 atm
D) 3.31 × 105 atm
E) 0.235 atm
2) The relationship between the "absolute temperature" on the Kelvin scale and the Celsius temperature
is given by:
A) T(K) = t(°C) + 273.15
B) t(°C) = T(K) + 273.15
C) T(K) = 5/9[t(°C)] - 32
D) T(K) = 9/5[t(°C)] + 32
E) t(°C) = 98.6 + T(K)
3) 53.5 g of an ideal gas of molecular weight = 30.5 g/mol is confined at a pressure of 133 mmHg. The
density of the gas is 0.228 g/L. Compute the temperature of the gas in degrees Celsius.
A) 261°C
B) 12.°C
C) -57°C
D) 285°C
E) -12.°C
4) What volume of acetylene gas, C2H2, would be required at 0°C and 1 atm to obtain a 200.0 g C2H2
sample?
A) 4480 L
B) 1.309 × 105 L
C) 320.0 L
D) 0.6304 L
E) 172.1 L
5) Of the following gases, the one with the greatest density at STP is:
A) CH4
B) NH3
C) Ne
D) H2
E) He
6) When one volume of CO reacts with one volume of Cl2 phosgene is obtained as the only product.
What is empirical formula of phosgene?
A) COCl2
B) C2O2Cl2
C) C2O2Cl
D) C3O3Cl2
E) COCl4
7) A gaseous mixture consists of 50.0% O2, 25.0% N2, and 25.0% Cl2, by mass. At standard
temperature and pressure, the partial pressure of:
A) Cl2(g) is greater than 0.25 atm
B) O2(g) is equal to 380 torr
C) Cl2(g) is less than 0.25 atm
D) N2(g) is equal to 0.20 atm
E) O2(g) is equal to 1.6 atm
8) A balloon with volume 750 cm3 is filled with O2 at 27°C has a mass of 83.3 g. The mass of empty
balloon is 82.1 g. Calculate the pressure of O2.
A) 125 kPa
B) 150 kPa
C) 250 kPa
D) 75 kPa
E) 400 kPa
9) Which of the following is a characteristic of an ideal gas?
A) Gas cannot be compressed infinitely.
B) Inter-particle forces are prominent.
C) Collisions between gas particles are perfectly elastic
D) Collisions between gas particles and container walls are not elastic
E) Individual gas particles occupy fixed volume.
10) If someone were to light a cigar at one end of a closed room, persons at the other end of the room
might soon perceive an odor due to gaseous emissions from the cigar. Such a phenomenon is an example
of:
A) monometry
B) ideality
C) effusion
D) diffusion
E) barometry
11) Gases tend to behave ideally at:
A) low temperature and low pressure
B) low temperature and high pressure
C) high temperature and low pressure
D) high temperature and high pressure
E) gases always behave ideally
12) Convert to the equivalent pressure in atmospheres, 1250 mmHg.
A) 9.50 × 105 atm
B) 490 atm
C) 1.64 atm
D) 0.608 atm
E) 1.22 atm
13) Liquid mercury freezes at a temperature of -39 °C. The freezing point of mercury on the Kelvin
scale is ________.
A) 234 K
B) 39 K
C) 312 K
D) 273 K
E) -39 K
14) A 4.0 L sample of N2(g) at 760 mmHg is compressed, at constant temperature, to 3.2 atm. What is
the final gas volume?
A) 950 L
B) 13 L
C) 59 L
D) 1.3 L
E) 0.77 L
15) A 5.00 L container of unknown gas at 25.0°C has a pressure of 2.45 atm. The mass of the gas is
32.1 g. What gas is in the container?
A) Cl2
B) F2
C) NO2
D) SO3
E) SO2
16) How many liters of H2 are needed to make 327 L of NH3 by the reaction:
N2 (g) + 3 H2 (g) → 2 NH3 (g),
if the gases are at the same temperature and pressure?
A) 654 L
B) 491 L
C) 218 L
D) 38.5 L
E) 327 L
17) A sample of oxygen gas is collected over water at 23°C at a barometric pressure of 751 mmHg (the
vapor pressure of water at 23°C = 21 mmHg). The partial pressure of oxygen gas in the sample collected
is ________.
A) 0.96 atm
B) 21 mmHg
C) 751 mmHg
D) 1.02 atm
E) 44 mmHg
18) What volume would be occupied by a mixture of 0.33 g of hydrogen gas and 0.67 g of nitrogen gas
at 157°C and 4.4 atm?
A) 12 L
B) 4.2 L
C) 3.1 L
D) 1.5 L
E) 0.55 L
19) A gas of twice the molecular weight as CO2 will pass through a small hole how much faster than
CO2?
A) 1/2 as fast
B) 2 times as fast
C) Error! Objects cannot be created from editing field codes. as fast
D) (1/ 2 ) as fast
E) 4 times as fast
Solubility rules:
Compounds that are soluble or mostly soluble––
• Salts of Group 1 cations and NH4+
• Nitrates, acetates, perchlorates
• Halides (except Ag+, Pb2+. and Hg22+)
• Sulfates (except Ba2+, Sr2+ , Pb2+. and Hg22+)
Compounds that are insoluble––
• Hydroxides, sulfides (except Group 1 and NH4+, and sulfides of Group 2)
• Carbonates, phosphates, chromates (except Group 1 and NH4+)
Possibly useful information (values, conversions, formulas):
Avogadro’s number = NA = 6.02 x 1023 mol–1
e = – 1.602 x 10–19 Coulombs
me = 9.109 x 10–31 kg
mp = 1.673 x 10–27 kg
mn = 1.675 x 10–27 kg
–27
1 amu = 1.661 x 10 kg
ρ (H2O) = 1.0 g cm–3 = 1.0 g mL–1
1 L = 1000 cm3
1 inch = 2.54 cm
Concentration1 x Volume1 = Concentration2 x Volume2; i.e. M1V1 = M2V2
Force:
1 newton (N) = 1 kg m s–2
Energy units:
1 joule (J) = 1 N m = 1 kg m2 s–2
1 kPa L = 1 J
1 bar L = 100 J
1 atm L = 101.325 J
Gases:
1 atm = 760 mmHg = 760 Torr
1 atm = 1.01325 bar = 101325 pascal (Pa) = 101.325 J L–1
1 Pa = 1 N m–2
R = 0.082 L atm mol–1 K–1 = 8.31 J mol–1 K–1 = 8.31 kPa L mol–1 K–1 = 8.31 Pa m3 mol–1 K–1
PV = nRT
Ptotal = P1 + P2 + …
Mole fraction of component A = XA = nA / ntotal = PA / Ptotal = VA / Vtotal
rate of effusion of A / rate of effusion of B