Download Citrus Chem 110 Lec

Chem 100 Lec.
Practice Final Exam
Sat. Dec. 10, 2016
1. Milli is the name of which number?
A) 103
B) 10-3
C) 10-6
D) 10-9
E) 10-12
2. Nano is the name of which number?
A) 103
B) 10-3
C) 10-6
D) 10-9
E) 10-12
3. Micro is the name of which number?
A) 103
B) 10-3
C) 10-6
D) 10-9
E) 10-12
4. How many grams are in .345 kilograms?
A) 3,450 g B) 345 g C) 34.5 g D) .000345 g
E) none of these
.345 kg x 1000 g = 345 g
1 kg
5. Convert the following number to scientific notation: .004320
-2
-2
-3
-3
A) 4.32 x 10
B) 4.320 x 10
C) 4.32 x 10
D) 4.320 x 10
-4
E) 4.320 x 10
6. Perform the following calculation: 203.0 g/54.0 mL
A) 37.6 g/mL
B) 37.59 g/mL
C) 3.759 g/mL
D) 3.76 g/mL
E) 3.75 g/mL
7. Perform the following calculation: 2.235 cm + 111.2 mm =
A) 2.346 cm B) 2346 mm C) 113.4 mm D) 133.6 mm E) 3.347 cm
8. Perform the following calculation: (2.235 m + 111.2 mm)/ 1.650 sec
A) 1422 mm/sec B) 1.422 m/sec C) 1422 cm/sec D) two of these
E) all of these
9. What is the volume of a 15.36 kg sample of mercury with mass density 13.7
g/mL ?
A) 210. mL B) 210. L C) 1.12 L D) 112 mL E) 1121 mL
15.36 kg = 15360 g x 1 mL = 1121 mL = 1.12 L
13.7 g
o
o
10. Convert 175.0 F to C
o
o
o
o
A) 65.22 C B) 129.22 C C) 97.22 C D) 79.44 C E) 115.00 oC
(175.0 oF - 32.0 oF) = 79.44 oF
1.8 oF/oC
11. Which of these processes is a chemical change
A) melting B) boiling C) burning D) evaporating E) A, B, and D
12. A chemical change always involves
A) forming a new substance B) destroying an previously existing substance
C) forming new chemical bonds D) A and B only
E) all of these
13. Which quantities are conserved in a chemical reaction?
A) number of atoms B) number of chemical bonds C) charge
D) A and C only
E) all of these
14. An example of a pure substance is
A) air
B) glass
C) steel
D) rust
15. An example of a compound is
A) O2
B) S8
C) P4
E) baking soda
D) SO3
E) all of these
16. An example of a homogeneous mixture is
A) air B) marble C) NH3(l)
D) table salt E) none of these
For the following problems use these values of atomic mass:
12.01 g C/mol,
14.01 g N/mol,
16.00 g O/mol,
1.01 g H/mol
22.99 g Na/mol,
30.97 g P/mol
17. How many hydrogen atoms are in one molecule of (CH3)2NOH?
A) 6.02 x 1023
B) 6
C) 3.61 x 10
24
24
D) 4.21 x 10
7 H atoms
= 7
1 molecule(CH3)2NOH
18. What is the molar mass of Na3PO3?
A) 124.95 g/mol B) 163.94 g/mol C) 147.94 g/mol
E) 7
1 (CH3)2NOH x
D) 131.94 g/mol
E) 142.95 g/mol
3 mol Na x 22.99 g Na = 68.97 g Na
mol Na
1 mol P x 30.97 g P =
30.97 g P
mol P
3 mol O x 16.00 g O = 48.00 g O
mol O
147.94 g Na3PO3
19. The diameter of an atom is approximately
-8
-10
-13
-15
A) 10 m B) 10 m C) 10 m D) 10 m
E) none of these
20. The diameter of an atomic nucleus is approximately
-8
-10
-13
-15
A) 10 m B) 10 m C) 10 m D) 10 m E) none of these
21. An element is defined by the number of
A) electrons B) neutrons C)protons D) neutrons and protons E)all of these
22. An isotope is defined by the number of
A) electrons B) neutrons C)protons D) neutrons and protons E)all of these
23. Which of the following particles has much less than the others?
A) electrons B) protons C) neutrons D) nucleons E) none of these
234
24. An enriched sample of uranium is 10.00 % U, 25.00% 235U, and 65.00
238
% U. What is the atomic mass of this sample of uranium?
A) 238.03 g/ mol B) 236.85 g/mol C) 235.85 g/mol D) 236.70 g/mol
E) 238.85 g/mol
(.1000)(234g/mol) + (.2500)(235 g/mol) + (.6500)(238 g/mol) = 236.85
56
3+
25. The species Fe has
A) 26 protons B) 24 electrons C) 30 neutrons D) A & C only
E) A, B, & C
1
2
5
26. 1s 2s 2p is the electron configuration for
A) ground state oxygen B) ground state fluorine C) excited state oxygen
D) excited state nitrogen E) none of these
27. An electronic transition is viewed as an electron moving between
A) energy levels B) orbitals
C) electron clouds
D) A and B only E) all of these
28. Electrons moving from a low energy orbital to a high energy orbital
A) give off light B) absorb photons
C) release energy
D) A and B
E) A and C
29. Which of these shows elements in order of increasing atomic radii ?
A) C,O,F,N B) C,N,O,F C) Fe,O,N,C D) I,Br,Cl,F E) F,Cl,S,P
30. What is the name of PbO2?
A) lead oxide
B) lead dioxide
C) lead (II) oxide
D) tin (IV) dioxide E) lead (IV) oxide
31. What is the formula for aluminum oxide?
A) Al4O3 B) Al2O C) AlO2 D) Al2O3 E) Al3O4
32. What is the name of MnCrO4?
A) manganese chromate
B) manganese (II) chromoxide
C) manganese (II) chromoxide D) manganese (II) chromate
E) manganese (II) chromium (III) oxide
33. What is the name of SCl4?
A) sulfur (IV) chloride
B) sulfur tetrachloride
C) silicon tetrachloride
D) sulfur (IV) tetrachloride
E) silicon (IV) chloride
34. What is the formula for dinitrogen monoxide?
A) NO2
B) N2O2
C) N2O3
D) NO3 E) N2O
35. What is the name of HCl(g)?
A) hydrochloric acid
B) nitric acid
C) sulfuric acid
D) phosphoric acid
E) hydrogen chloride
36. What is the name of H2SO3(aq)?
A) sulfurous acid
B) nitric acid
D) phosphoric acid
E) none of these
C) sulfuric acid
37. What is the name of HNO3(aq)?
A) nitrous acid
B) nitric acid
D) phosphoric acid
E) none of these
C) sulfuric acid
38. What is the name of H3PO3(aq) ?
A) phosphorous acid
B) nitric acid
D) phosphoric acid
E) none of these
C) sulfuric acid
For the following problems use these values of atomic mass:
12.01 g C/mol, 14.01 g N/mol, 16.00 g O/mol 1.01 g H/mol
39. How many moles of oxygen atoms are in 36.5 g of NO2(g).
A) .793 mol O
B) 1.59 mol O
C) .397 mol O
D) .739 mol O
E) 1.95 mol O
36.5 g NO2 x
1 mol NO2 x
46.01 g NO2
2 mol O = 1.5866 mol O
1 mol NO2
40. What is the mass of 4.20 mol of hydrogen atoms?
A) 4.24 g H B) 8.48 g H C) 4.42 g H D) 4.61 g H E) none of these
4.20 mol H atoms x
1.01 g H atoms = 4.24 g H atoms
1 mol H atoms
41. How many atoms are in 27.0 g of carbon?
26
-26
23
A) 1.95 x 10 atoms C B) 1.95 x 10 atoms C C) 5.16 x 10 atoms C
24
D) 1.35 x 10 atoms C E) 3.73 x 10-24 atoms C
27.0 g C x
1 mol C x 6.02 x 1023 atoms C = 1.3534 x 1024 atoms C
12.01 g C
1 mol C
42. What is the molar mass of N2H5OH?
A) 49.07 g/mol
B) 36.07 g/mol
D) 52.07 g/mol
E) 50.08 g/mol
2 mol N x 14.01 g N = 28.02 g N
mol N
C) 66.08 g/mol
6 mol H x 1.01 g H = 6.06 g H
mol H
1 mol O x 16.00 g O = 16.00 g O
mol O
50.08 g Na3PO3
43. What is the mass of 1.62 mol of CH3NO2?
A) 99.8 g CH3NO2
B) 89.8 g CH3NO2
D) 88.9 g CH3NO2
E) none of these
1 mol C x 12.01 g C = 12.01 g C
mol C
1 mol N x 14.01 g N = 14.01 g N
mol N
3 mol H x 1.01 g H = 3.03 g H
mol H
2 mol O x 16.00 g O = 32.00 g O
mol O
61.05 g CH3NO2
1.62 mol CH3NO2 x 61.05 g CH3NO2 = 98.8 g
mol CH3NO2
C) 98.9 g CH3NO2
44. How many moles of CH3NO2 are in 40.0 g CH3NO2?
A) .655 mol CH3NO2
B) .565 mol CH3NO2
C) .665 mol CH3NO2
D) .556 mol CH3NO2
E) none of these
40.0 g CH3NO2 x
mol CH3NO2
= .655 mol
61.05 g CH3NO2
45. What is the mass % oxygen in CH3NO2?
A) 26.2 mass % O
B) 52.4 mass % O
D) 54.2 mass % O
E) none of these
C) 22.6 mass % O
32.00 g O
x 100 = 52.416 m/m %
61.05 g CH3NO2
Balance the following equation
Ca(HSO3)2(s)

2 SO2(g) +
Ca(OH)2(s)
46. What is the coefficient in front of Ca(OH)2(s)?
A) 1
B) 2
C) 3
D) 4
E) none of these
47. What is the coefficient in front of SO2(g)?
A) 1
B) 2
C) 3
D) 4
E) none of these
48. The reaction involving Ca(HSO3)2(s) can be described as a
A) combination
D) double replacement
B) decomposition
E) neutralization
C) single replacement
49 How many valence electrons are in ClO3-?
A) 22
B) 24
C) 26
D) 28
E) 20
Balance the following equation
3 Ca(OH)2(aq) + 2 Co(NO3)3(aq)
 2 Co(OH)3(s) + 3 Ca(NO3)2(aq)
50. What is the coefficient in front of Co(NO3)3(aq)?
A) 1
B) 2
C) 3
D) 4
E) none of these
51. What is the coefficient in front of Ca(NO3)2(aq)?
A) 1
B) 2
C) 3
D) 4
E) none of these
52. This reaction can be described as a
A) combination
D) double replacement
B) decomposition
E) neutralization
Balance the following equation: 2 Al(s) + 3 Cl2(g)
53. What is the coefficient in front of Cl2(g)?
A) 1
B) 2
C) 3
D) 4
C) single replacement

2 AlCl3(s)
E) none of these
54. This reaction can be described as a
A) combination
D) double replacement
B) decomposition
E) neutralization
C) single replacement
Balance the following equation
2 Al(s) + 3 Mn(NO3)2(aq) 
2 Al(NO3)3(aq) + 3 Mn(s)
55. What is the coefficient in front of Mn(s)?
A) 1
B) 2
C) 3
D) 4
E) none of these
56. What is the coefficient in front of Al(NO3)3(aq)?
A) 1
B) 2
C) 3
D) 4
E) none of these
57. This reaction can be described as a
A) combination
B) decomposition
C) single replacement
D) double replacement E) neutralization
Consider the following equation
4 Mg(s) +
Fe3O4(s)

4 MgO(s)
+
3 Fe(l)
24.3 g/mol
231.6 g/mol
40.3 g/mol
55.8 g/mol
58. How many moles of magnesium are needed to make 1.34 moles of iron?
A) 1.34 mols Mg(s)
B) 1.79 mols Mg(s)
C) 1.01 mols Mg(s)
D) 2.38 mols Mg(s)
E) 3.58 mols Mg(s)
1.34 mol Fe x 4 mol Mg = 1.786666 mol Mg
3 mol Fe
59. How many grams of Mg are needed react with 4.65 grams of Fe3O4(s)?
A) .122 g Mg(s) B) 11.1 g Mg(s) C) .488 g Mg(s) D) 1.95 g Mg(s)
E) none of these answers
4.65 g Fe3O4 x
mol Fe3O4 x 4 mol Mg x 24.3 g Mg = 1.95 g Mg
231.6 g Fe3O4
1 mol Fe3O4
mol Mg
60. If 6.80 g Mg are reacted with 16.50 g of Fe3O4, then what is the limiting
reagent?
A) Mg(s)
B) Fe3O4(s)
C) MgO(s)
D) Fe(l)
16.50 g Fe3O4 x
mol Fe3O4 x
231.6 g Fe3O4
3 mol Fe x 55.8 g Fe = 11.926 g Fe
1 mol Fe3O4
mol Fe
6.80 g Mg x mol Mg x
24.3 g Mg
3 mol Fe x 55.8 g Fe = 11.7 g Fe
4 mol Mg
mol Fe
61. If 6.80 g Mg are reacted with 16.50 g of Fe3O4, then how many grams of
Fe(l) are produced?
A) 11.7 g Fe
B) 11.9 g Fe
C) 15.6 g Fe
D) 3.91 g Fe
E) 20.8 g Fe
62. If 6.80 g Mg are reacted with 16.50 g of Fe3O4, then how many grams of
MgO(s) are produced?
A) 2.87 g MgO
B) 11.3 g MgO
C) 11.5 g MgO
D) 4.10 g MgO
E) 9.95 g MgO
6.80 g Mg x mol Mg x
24.3 g Mg
4 mol MgO
4 mol Mg
x 40.3 g MgO = 11.277 g Fe
mol MgO
63. If 6.80 g Mg are reacted with 16.50 g of Fe3O4, then how many grams of
starting material are left unreacted?
A) .3 g Mg
B) .3 g Fe3O4
C) .3 g Mg
D) .13 g Fe3O4
E) .2 g Fe3O4
6.80 g Mg x mol Mg x 1 mol Fe3O4 x 231.6 g Fe3O4 = 16.202 g Fe3O4
24.3 g Mg
4 mol Mg
mol Fe3O4
16.50 g Fe3O4 - 16.202 g Fe3O4 = .3 g Fe3O4
64. A material that accepts a proton is
A) an acid B) a base C) a salt D) a non-electrolyte E) none of these
65. A material the donates a proton is
A) an acid B) a base C) a salt D) a non-electrolyte E) none of these
66. When an acid is mixed with a base, the product is
A) an acid
B) a base
C) a salt
D) water
E) C and D
67. Which of the colors of visible light has the least energy per photon?
A) blue
B) yellow C) orange
D) violet
E) green
68. How many grams of NaCl are contained in 150.0 g of 12.5 m/m% solution?
A) 12.0 g NaCl
D) 8.333 g NaCl
B) 8.33 g NaCl
E) 18.8 g NaCl
150.0 g soln x 12.5 g NaCl
100 g soln
C) 12.5 g NaCl
= 18.75 g NaCl
69. 10.0 g of NaCl are dissolved in water and diluted 1.50 L total volume.
What is the molarity of this solution?
A) 6.66 M B) .150 M C) .114 M D) .257 M E) none of these
10.0 g NaCl x
mol NaCl
1.50 L soln
58.44 g NaCl
= .114 M
70. What volume of 3.00 M HCl is needed to make .500 L of .556 M HCl?
A) 3.34 mL B) .371 L C) 2.70 mL D) 92.7 mL
E) none of these
.500 L x .556 M = .0926666 L
3.00 M
71. If you start with 20.0 grams of each of the reactants below, which is the
limiting reagent?
LiF + NH3 + H2O + CO2  NH4F + LiHCO3
A) LiF
B) NH3
C) H2O
D) CO2
25.94 g/mol
17.04 g/mol
18.02 g/mol
44.01 g/mol
For a stoichiometric reaction, one mole of each reactant is needed. CO2 is the
most massive molecule, so 20 g of it has the fewest number of moles.
72. For the reaction N2H4(g) + 3 O2(g)  2 NO2(g) + 2 H2O(l), how many
molecules of NO2 are produced when 5 mol of oxygen completely reacts?
A) 4.51 x 1024 B) 2.01 x 1024 C) 4.51 x 1023 D) 2.01 x 1023 E) 7.5
5 mol O2 x 2 mol NO2 x 6.02 x 1023 molecules NO2 = 2.0067 x 1024 NO2
3 mol O2
mol NO2
73. Which represents the largest number of atoms?
A) 50.0 g I
B) 50.0 g Br
C) 50.0 g Co
D) 50.0 g S
E) all are the same
Sulfur is the lightest atom so it has more atoms per 50 g
74. Which of the following elements has the smallest number of electrons in its
valence shell?
A) S
B) As
C) K
D) F
E) Ar
75. As an electron’s principle energy level increases, the average distance of
the electron from the nucleus does what?
A) increases
B) decreases
C) stays the same
D) varies
+
+
-
-
B
C
+
A
+
-
+
-
+
- -
D
+
E
76. Which of the above shapes best describes the d orbital of an atom? D
77. Which of the following atoms has d electrons in orbitals?
A) iron B) beryllium C) oxygen
D) sodium E) all of these
78. What happens when an electron moves from the 3d orbital to the 4p
orbital?
A) the atom is ionized
B) light is absorbed C) light is emitted
D) the atom gets heavier
E) both D and C
79. What is the correct electron configuration for ground state S?
2 2
5 2
5
1 2
6 2
4
2 2
6 2
5
A) 1s 2s 2p 3s 3p B) 1s 2s 2p 3s 3p
C) 1s 2s 2p 3s 3p
2 2
6 2
4
1s 2s 2p 3s 3p
1 2
5 2
5
E) 1s 2s 2p 3s 3p
1
2
6
D)
1
80. 1s 2s 2p 3s is the electron configuration for
A) ground state neon
B) ground state magnesium
sodium
D) excited state neon
E) none of these
C) excited state
81. Which of these shows elements in order of increasing atomic size?
A) C,O,F,N
B) C,N,O,B
C) O,N,P,S
D) I,Br,Cl,F E) none of
these
82. How many valence electrons does the boron atom have?
A) 8
B) 3
C) 4
D) 9
E) none, it isn’t bonded to another
atom