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Finals Review Questions
1. An example of a chemical change is
(A) freezing of water.
(B) burning a match.
(C) boiling carbon tetrachloride.
(D) dissolving alcohol in water.
(E) stretching a rubber band
2. Which involves a chemical change?
(A) powdering sugar
(B) condensing steam
(C) magnetizing an iron bar
(D) separating cream from milk
(E) exposing photographic film to light
3. The law of multiple proportions is based upon the idea that atoms of some elements may
(A) have several isotopes.
(B) exist in several physical forms.
(C) have more than one atomic mass.
(D) have both metallic and non–metallic properties.
(E) have more than one valence number.
4. Rutherford’s alpha–particle bombardment of gold foil helped develop our current model of the atom by
(A) finding the mass of the electron.
(B) showing the existence of the neutron.
(C) showing that the electron carries a negative charge.
(D) showing that the atom has a concentrated central charge.
5. Which set consists only of compounds?
(A) Na, Ca, He
(C) NaCl, CH4, Br2
(B) H3O+, Cl–, I3–
(D) H2S, CuCl2, KI
6. Which property would be most helpful in identifying a substance?
(A) mass
(C) volume
(B) state
(D) melting point
7. An insoluble solid has a mass of 20.0 g. It is placed in a graduated cylinder containing 40.0 mL of water. The final
volume is read as 46.0 mL. What is the density of the solid?
(A) 0.300 g·cm–3
(C)
2.30 g·cm–3
–3
(B) 0.500 g·cm
(D)
3.33 g·cm–3
8. A solid, pure, orange substance was heated yielding a colorless gas and a green solid. What kind of material was
heated?
(A) an element
(C) a mixture
(B) a compound
(D) a solution
9. Which unit represents l x 10–3 mol?
(A) decimole
(C) millimole
(B) kilomole
(D) micromole
10. The volume of one milliliter most nearly equals
(A) 454 g
(B) 1000 L (C) 1 mg
(D) 1 in
(E)
1 cm3
Finals Review Questions
11. A barometer is used to measure the
(A) pressure of the air at 0 °C only.
(B) mass of a column of mercury.
(C) temperature of the air at standard pressure.
(D) density of mercury.
(E) pressure of the air.
12. Which apparatus delivers 50.00 mL of liquid most accurately?
(A) 50–mL buret
(B) 50–mL beaker
(C) 50–mL test tube
(D) 50–mL graduated cylinder
13. If atom A contains 18 protons and 22 neutrons, while atom B contains 20 protons and 20 neutrons, then atoms A
and B are
(A) isotopes.
(B) both metallic.
(C) both non–metallic.
(D) alike in number of'electrons.
(E) different in number of electrons
14
14. The number of neutrons in an atom of the radioactive carbon isotope 6 C, is
(A) 6
(B) 8
(C) 12
(D) 14
(E)
20
15. Which particle consists of 13 protons, 14 neutrons, and 10 electrons?
(A) neon atom
(D) silicon atom
(B) sodium atom
(E) phosphide ion
(C) aluminum ion
16. A hypothetical element X has three isotopes: 40X, 41X, and 42X. Their abundances are 72.0%, 9.00%, and 19.0%
respectively. What is the atomic mass of X?
(A) 40.5 u
(B) 40.8 u
(C) 41.0 u
(D) 41.5 u
17. A chlorine atom (Cl) differs from a chloride ion (Cl–) in that a chlorine atom
(A) has a positive nucleus while the ion’s nucleus is negative.
(B) has a neutral nucleus while the ion’s nucleus is positive.
(C) contains one electron less than the ion.
(D) contains one electron more than the ion.
(E) contains one proton more in the nucleus
18. All positive ions differ from their corresponding atoms by having
(A) larger diameters.
(B) fewer electrons.
(C) a charge of +1.
(D) greater atomic masses.
(E) stronger metallic properties
19. The correct formula for iron(III) sulfate is
(A) FeSO4
(D) Fe2(SO4)3
(B) Fe(SO4)2
(E)
Fe3(SO4)2
(C) Fe2SO4
Finals Review Questions
20. Which formula is incorrect?
(A) BaHCO3 (B) Ca(OH)2 (C) Al2O3
(E) ZnCO3
(D) K2SO4
21. The compound not properly named is
(A) Fe2O3, iron(III) oxide.
(B) Pb3O4, trilead tetraoxide.
(C) CuCl2, copper(II) chloride.
(D) Pb3(PO4)2, lead(III) phosphate
22. What is the total number of oxygen atoms represented by the formula KAl(SO4)2·12H2O?
(A) 9
(B) 16
(C) 20
(D) 48
(E)
96
23. Using only these formulas,
XY2
X2Z
QZ
what formula would you expect for a compound of elements Q and Y?
(A) QY
(B) QY2
(C) Q2Y
(D) QY4
24. In the reaction
4Al + 3O2  2Al2O3
how many moles of aluminum oxide, Al2O3, are produced from one mole of aluminum, Al?
(A) 0.5
(B) 2
(C) 3
(D) 4
25. Which expression is correctly balanced?
(A) Na2O2 + 2H2O  2NaOH + O2
(B) 2Na2O2 + 2H2O  4NaOH + 2O2
(C) 4Na2O2 + 3H2O  4NaOH + 2O2
(D) 2Na2O2 + 2H2O  4NaOH + O2
(E) 3Na2O2 + 2H2O  6NaOH + O2
26. Consider the unbalanced expression:
? CH3 CH2CHO(l) + ? O2(g)  ? CO2(g) + ? H2O(g)
Which set of coefficients balances the equation?
(A) 2, 8, 3, 6
(D)
1, 8, 3, 3
(B) 3, 8, 6, 6
(E)
1, 4, 3, 3
(C) 1, 4, 3, 2
Finals Review Questions
27. Given the equation
N2 + 3H2
∅
♦
2NH3
Theoretically, the number of moles of ammonia produced from 2 mol of nitrogen is
(A) 1
(B) 2
(C) 3
(D) 4
(E)
5
28. One mole of substance X reacts with one mole of water and produces one mole of oxygen and two moles of
hydrogen fluoride.
X + H2O ∅ O2 + 2HF
What is the formula of substance X?
(A) F2
(B) OF2
(C) O2F
(D) HOF2
29. When basic copper(II) carbonate, CuCO3·Cu(OH)2, is heated, it decomposes. What is the missing product in this
equation?
CuCO3 ·Cu(OH)2 ∅ 2CuO + CO2 + ?
(A) H2CO3
(B) H2O
(C) CuH2
(D) H2
30. What is the net ionic equation for the reaction between solutions of sodium chloride, NaCl, and silver nitrate,
AgNO3?
(A) Na+(aq) + NO3–(aq)  Na(s) + 1/2N2(g) + 3/2O2(g)
(B) Ag+(aq) + Cl–(aq)  Ag(s) + 1/2 Cl2(g)
(C) Ag+(aq) + Cl–(aq) Ag+(aq) + Cl–(aq)
(D) Ag+(aq) + Cl–(aq)  AgCl(s)
31. Which two ions do not participate in the reaction between solutions of silver nitrate, AgNO3, and potassium
chloride, KCl?
(A) K+ and Ag+
(C) K+ and Cl–
(B) K+ and NO3–
(D) Ag+ and Cl
32. A compound whose empirical formula is CH2 has a molar mass of 28 g·mol–1. What is the molecular formula?
Atomic Molar Masses
C
H
(A) CH2
(B) C2H4
12.0 g·mol–1
1.0 g·mol–1
(C) C2H2
(D) CH4
Finals Review Questions
33. A substance with a molar mass of 92 g·mol–1 consists of equal numbers of S and N atoms. What is the formula
of the substance?
Atomic Molar Masses
N
S
(A) SN
(B) S2N2
g·mol–1
14.0
32.1 g·mol–1
(C) S3N3
(D) S4N4
34. What is the mass of one mole of calcium nitrate, Ca(NO3)2?
Atomic Molar Masses
Ca
N
O
(A) 82 g
(B) 102 g
40. g·mol–1
14. g·mol–1
16. g·mol–1
(C) 164 g
(D) 204 g
35. What is the percentage by mass of carbon in oxalic acid, H2C2O4?
Atomic Molar Masses
C
H
O
(A) 2.22%
(B) 3.75%
12.0 g·mol–1
1.0 g·mol–1
16.0 g·mol–1
(C) 25.0%
(D) 26.7%
36. How many molecules are in 11.0 g of carbon dioxide, CO2?
Atomic Molar Masses
C
O
g·mol–1
12.0
16.0 g·mol–1
(A) 1.50 x 1023
(C) 4.40 x 1023
(B) 2.24 x 1023
(D) 5.60 x 1023
37. Calculate the mass of 12.0 x 1023 molecules of chlorine gas, Cl2.
Atomic Molar Mass
Cl
(A) 35.5 g
(B) 71.0 g
35.5 g·mol–1
(C) 142 g
(D) 284 g
Finals Review Questions
38. At STP, 4.48 L of hydrogen was prepared using the reaction:
Zn + 2HCl ∅ ZnCl2 + H2
Approximately what mass of zinc was required?
Atomic Molar Mass
Zn
(A) 1.5 g
(B) 2.0 g
65 g·mol–1
(C) 13.0 g
(D) 36.5 g
(E)
65.0 g
Energy !
39. This potential energy diagram shows that the reaction A + B  C is
A +B
x
C
Reaction Coordinate !
(A) slow.
(D) endothermic.
(B) rapid.
(E) at equilibrium.
(C) exothermic.
40. Note the equation:
2Fe(s) + 3/2O2(g) ∅ Fe2O3(s)
If 0.100 mol of iron reacts, how much heat is liberated?
(A) 42.0 kJ
(D) 420 kJ
(B) 84.0 kJ
(E) 840 kJ
(C) 210 kJ
ΔH = –840 kJ·mol–1 Fe2O3
Finals Review Questions
41. The gaseous molecules that have the greatest average velocity at 150 °C are represented by
Atomic Molar Masses
12.0 g·mol–1
19.0 g·mol–1
1.0 g·mol–1
14.0 g·mol–1
16.0 g·mol–1
C
F
H
N
O
(A) O2
(B) F2
(C) H2
(D) N2
(E) H2O
42. The approximate number of molecules of hydrogen in
1.00 L of H2 gas at STP is
(A) 1.35 x 1022
(D) 2.69 x 1022
(B) 3.01 x 1023
(E) 5.38 x 1022
(C) 6.02 x 1023
43. A cylinder equipped with a movable piston contains
50.0 cm3 of a gas. What is the new volume when the pressure is doubled at constant temperature?
(A) 25.0 cm3
(C)
75.0 cm3
(B) 50.0 cm3
(D)
100 cm3