971015 Exam
Name___________________________________
MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.
1) Which of the following has the lowest % w/w oxygen composition?
A) Al2O3 B) KMnO4 C) K2CO3 D) N2O
Answer: C
2) Choose the INCORRECT statement.
A) A natural law is a generalization of natural phenomena.
B) An experiment is a test of conclusions about natural law.
C) The scientific method is the combination of observations, experimentation, and the formulation of laws, hypothesis and theories.
D) A hypothesis is a conclusion that must follow logically from observations of nature.
E) A theory is a model of nature that can be used to describe natural phenomena.
Answer: D
3) Naphthalene, commonly found in mothballs, is 93.75% carbon and 6.25% hydrogen by mass. The molar mass is 128 u. What is the formula for naphthalene?
A) C9H2O B) C10H8 C) C12H10 D) CH15 E) C5H4
Answer: B
4) When an egg is fried, what type of process is happening?
A) a physical change B) condensation C) a chemical change D) melting
E) evaporation Answer: C
5) Which is the chemical change in the following list?
A) digestion of bread
B) grinding of wheat to make flour
C) using modeling clay to make a toy horse D) drying clothes in the sunshine
E) mixing sand and water to make mud Answer: A
6) Which of the following contains the greatest number of atoms?
A) 1 mole of S8 molecules B) 2 moles of P4 molecules C) 4 moles of chlorine molecules D) 8 moles of H atoms
E) All of these contain the same number of atoms.
Answer: E
7) A species which differs in charge from the atom of the same element:
I) is called an isotope II) has more or less neutrons III) has lost or gained electrons IV) is called an ion
V) has the same number of protons of the atom
A) I and II B) I and III C) II and IV D) III and IV E) III, IV, V Answer: E
8) How many moles of H3PO4 are produced when 20.0 g of HCl are produced by the reaction PCl5 + 4 H2O H3PO4 + 5 HCl?
A) (20.0/36.5)/5 B) (20.0/36.5) C) (20.0/98.0) D) (20.0/98.0)/5 E) (20.0/35.5)/5 Answer: A
9) A nugget of gold with a mass of 521 g is added to 50.0 mL of water. The water level rises to a volume of 77.0 mL. What is the density of the gold?
A) 10.4 g/mL B) 6.77 g/mL C) 0.0518 g/mL D) 1.00 g/mL E) 19.3 g/mL Answer: E
10) Which one of the following would be classified as a heterogeneous mixture?
A) brass B) coke
C) copper nitrate solution D) salt water
E) air Answer: E
11) Which of the following compounds has its oxygen composition equal to 50.0% w/w ?
A) C10H20ONS B) CH2O2 C) (NH4)2CO3 D) C2H3NO2
Answer: C
12) Isotopes are atoms of the same element that have __________.
A) the same atomic mass but different numbers of protons B) different atomic numbers
C) the same atomic number but different numbers of neutrons D) the same atomic numbers but different numbers of electrons
E) the same atomic numbers but different numbers of protons Answer: C
13) The production of rust from iron requires what chemical?
A) chlorine B) hydrogen C) nitrogen D) oxygen E) mercury
Answer: D
14) Nitroglycerin, C3H5N3O3:
A) has less 50% w/w O by weight
B) has the same weight percent of C and N C) none of these
D) has equal amounts of C and N by weight
15) How many significant figures should the answer to the following calculation have?
(1.4312 - 1.1 x 10-2) ÷ (1.0712 x 10-4)
A) 4 B) 2 C) 5 D) 3
Answer: A
16) According to the Atomic Theory, A) all atoms are different.
B) atoms of different element combine to form compounds.
C) atoms are created and destroyed during a chemical reaction.
D) a compound can contain different numbers of atoms as long as it has the same kinds of atoms.
E) all matter is made up of tiny particles called electrons.
Answer: B
17) Choose the INCORRECT name/formula combination.
A) NaClO4 sodium chlorate B) Sr(IO3)2 strontium iodate C) NaClO sodium hypochlorite D) SCl4 sulfur tetrachloride
E) NaClO2 sodium chlorite Answer: A
18) The Rutherford gold foil experiment demonstrated that atoms
A) consist of an almost empty nucleus surrounded by a dense cloud of electrons.
B) consist of a single type of subatomic particle.
C) are visible to the naked eye.
D) consist of a dense nucleus surrounded by mostly empty space.
E) are homogeneous.
Answer: D
19) Arrange the following in order of increasing oxidation state of chlorine:
NaClO, NaClO3, NaClO2 and NaClO4.
A) NaClO4, NaClO3, NaClO2, NaClO B) NaClO, NaClO2, NaClO3, NaClO4 C) NaClO3, NaClO2, NaClO, NaClO4 D) NaClO, NaClO3, NaClO2, NaClO4 E) NaClO4, NaClO, NaClO3, NaClO2 Answer: B
20) The trinitrotoluene, TNT, C6H3N3O6, has the same atomic proportion of:
A) N to H atoms as does NH3 B) C to O atoms as does CO2 C) H to O atoms as does H2O D) C to H atoms as does C6H6
E) N to O atoms as does NO2 Answer: E
21) Nitrogen forms at least three stable oxides: N2O, NO, and NO2. How many grams of nitrogen forms with 32 grams of oxygen in NO?
A) 14 grams B) 16 grams C) 28 grams D) 8 grams E) 32 grams
Answer: C
22) 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) 2.2 g B) 3.6 g C) 19 g D) 6.0 g E) 9.5 g
Answer: B
23) When gold is melted and formed in a mold to make a piece of jewelry, what type of change is taking place?
A) evaporation B) a change of size C) a chemical change D) boiling
E) a physical change Answer: E
24) What is the answer, with the correct number of significant figures, for this problem?
4.392 g + 102.40 g + 2.51 g =
A) 109.302 g B) 109.30 g C) 110 g D) 109.3 g E) 109 g
Answer: B
25) 3.22 g of Na2SO4 . xH2O produce 1.42 g Na2SO4, upon strong heating. The empirical formula of the compound is ________.
A) Na2SO4 . 2H2O B) Na2SO4 . 5H2O C) Na2SO4 . 10H2O D) Na2SO4 . H2O Answer: C
26) The chemical reaction during low current discharge of a simple "dry cell" involves:
(unbalanced) Zn + MnO2 + NH4Cl ZnCl2 + Mn2O3 + NH3 + H2O
What is the coefficient for zinc in the balanced equation, and what is the limiting reagent for a process in which equal masses of reactants are mixed?
A) 2/Zn B) 1/Zn C) 2/MnO2 D) 2NH4Cl E) 1/MnO2
Answer: E
27) Which of the following numbers contains the designated CORRECT number of significant figures?
A) 0.00302 2 significant figures B) 1.04 2 significant figures C) 1.56 × 103 3 significant figures D) 3.0650 4 significant figures E) 0.04300 5 significant figures Answer: C
28) Which of the following descriptions of a subatomic particle is correct?
A) A proton has a positive charge and a negligible mass.
B) A neutron has a positive charge and a mass of approximately 1 amu.
C) A proton has a positive charge and a mass of approximately 1 amu.
D) An electron has a negative charge and a mass of approximately 1 amu.
E) A neutron has no charge and its mass is negligible.
Answer: C
29) How many mL of 0.024 M solution can be produced from 14.1 mL of 3.0 M solution?
A) (14.1/0.024)/3.0 B) 14.1(0.024/3.0) C) (14.1)(0.024)(3.0) D) 14.1(3.0/0.024)
E) none of these Answer: D
30) How many atoms of sulfur are in 280 g of a 50% H2SO4 solution?
A) 8.6 × 1025 atoms B) 8.0 × 1023 atoms C) 8.6 × 1023 atoms D) 8.0 × 1025 atoms E) 2.8 × 1029 atoms Answer: C
31) Choose the INCORRECT name formula combination.
A) NH4ClO3 ammonium chlorate B) SiO2 silicon oxide
C) CaH2 calcium hydride D) H2SO3 sulfurous acid
E) Fe2O3 iron(III) oxide Answer: B
32) Which of the following examples illustrates a number that is correctly rounded to three significant figures?
A) 109 526 grams to 109 500 grams B) 20.0332 grams to 20.0 grams C) 0.03954 grams to 0.040 grams D) 4.05438 grams to 4.054 grams E) 103.692 grams to 103.7 grams Answer: B
33) Choose the INCORRECT statement.
A) The mass number is the number of protons plus neutrons.
B) The atomic number is the proton number.
C) Protons and neutrons are found in the nucleus.
D) Gamma rays are bent by magnetic fields as a ray of positive charges.
E) Protons and neutrons are close to the same mass.
Answer: D
34) Complete combustion of a 0.500 g sample of a pure hydrocarbon yielded 0.973 g CO2 and 0.323 g H2O. The empirical formula of this hydrocarbon is:
A) C3H5 B) C6H9 C) C5H8 D) C2H3 E) C4H6
Answer: C
35) Silver possesses two stable forms: 107Ag (106.90 u) and 109Ag (108.90 u). If the average atomic mass of Ag is 107.87 u, what is the % w/w abundance of 107Ag?
A) 53.8% B) 48.5% C) 50.0% D) 46.3% E) 51.5%
Answer: E
36) 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) second assumption of Dalton's theory.
C) first assumption of Dalton's atomic theory.
D) law of multiple proportions.
E) law of constant composition.
Answer: E
37) Which of the following represents a 1.00 M aqueous solution of glucose (C6H12O6)?
A) 0.100 g glucose per mL solution B) 10.0 g glucose per 10.0 mL water C) 0.180 g glucose per mL solution D) 90.0 g glucose per 500 mL water
E) 4.5 g glucose per 4.5 g water Answer: C
38) Significant figures are important because they indicate __________.
A) the accuracy of the conversion factor B) the number of digits in a measurement C) the number of digits on a calculator D) a counted number
E) the number of measurements Answer: B
39) When you observe the formation of fog on a cool, humid day, what type of event are you observing?
A) a chemical change in oxygen B) a chemical change in water
C) a combination of nitrogen and oxygen D) a physical change in water
E) a physical change in air Answer: D
40) Consider the gaseous reaction:
N2H4(g) + 3 O2(g) 2 NO2(g) + 2 H2O(g)
If the above reaction has a percent yield of 98.5%, what mass in grams of oxygen is needed to produce 49.0 g of NO2(g)?
A) 50.4 g B) 25.9 g C) 23.1 g D) 51.9 g E) 11.5 g
41) A student measuring the density of a solution (d = 1.233 g/mol) reported the following results:
1.285, 1.287, 1.284, 1.279. Which of the following is the best description of the student's data?
A) precise, inaccurate B) not precise, inaccurate C) precise, accurate
D) precise, but with a systematic error E) not precise, accurate
Answer: D
42) Which of the following is NOT true for the atoms 13N, 14N, and 15N?
A) They all have 7 electrons.
B) They are isotopes.
C) They all have 7 protons.
D) They all have the same mass number.
E) They all have the same atomic number.
Answer: D
43) When decomposed chemically, 73.0 grams of a sample of HCl produce 71.0 g of Cl2 and 2.0 g of H2, while 34.0 g of a sample of H2S produce 32.0 g of S and 2.0 g of H2. This is an example of the Law:
A) of Conservation of Mass B) E = mc2
C) of Multiple Proportions D) of Definite Proportions
E) none of these Answer: A
44) Dalton's atomic theory is based on several assumptions which are listed below. Which of these assumptions is strictly correct?
I) All atoms of the same element are identical.
II) Atoms are indivisible and unchangeable.
III) Chemical changes are the result of the combination, separation, and rearrangement of atoms.
A) III is correct.
B) I, II, and III are correct.
C) I and II are correct.
D) I and III are correct.
E) II and III are correct.
Answer: A
45) The number of significant figures in the measurement of 45.030 mm is __________.
A) none B) five C) four D) three E) six
Answer: B
Use the equation C2H6O + O2 CO2 + H2O to answer the following question(s).
46) The balanced equation involves the corresponding coefficients ________.
A) 1: 2: 2: 3 B) 2: 7: 4: 6 C) 1: 3: 2: 3 D) 2: 9: 4: 6
Answer: C
47) The theoretical number of carbon dioxide moles produced from 3 moles C2H6O is ________.
A) 3 B) 6 C) 9 D) 4
Answer: B
48) The theoretical number of moles of water produced from 2 moles C2H6O is ________.
A) 2 B) 9 C) 6 D) 3
Answer: C
49) What is the theoretical mass of carbon dioxide produced from one mole of C2H6O?
A) 44 g B) 176 g C) 88 g D) 6 g
Answer: C
50) The % yield of an experiment in which 1 mole C2H6O was used and 22g carbon dioxide was isolated is ________.
A) 50% B) 25% C) 37.5% D) 100%
Answer: B
