Answers to Questions & Problems in Textbook - Chapter 6

1. 909 washers
2. in your text
3. The atomic mass unit (amu) is a unit of mass defined by scientists to more simply describe relative masses on an atomic or molecular scale. One amu is equivalent to 1.66x10^-24g
4. in your text
5.
  1. in your text
  2. 2.319x10^6 amu
  3. in your text
  4. 1.011x10^25 amu
  5. 5. 4.976x10^4
6.
in your text
10 S atoms
in your text
150.0 Xe atoms = 150 Xe atoms
133 Al atoms
7. 258 S atoms, 1.672 * 1026 amu
8. 1.204 * 1024
9. in your text
10. 20.05 g Ca, 40.08 g Ca
11. in your text
12. 2.66 * 10^-23g
13. in your text
14.
  1. in your text
  2. 1.04 mol Ca
  3. in your text
  4. 1.33x10^-5 mol Pd
  5. in your text
  6. 8.12 mol Fe
  7. 1.000 mol C
15.
  1. in your text
  2. 30.6 g Ni
  3. in your text
  4. 1.50x10^4 g Pb
  5. in your text
  6. 1.31x10^5 g Al
  7. 1468 g Li
  8. 8. 3.95x10^-5g Na
  9. 16.
  1. in your text
  2. 6.20x10^20 Co atoms
  3. in your text
  4. 0.00995 mol Co
  5. in your text
  6. 2.55x10^24 Co atoms
  7. 4.32x10^22
17. molar mass
18. in your text
19.
  1. in your text
  2. 76.15 g
  3. in your text
  4. 46.07 g
  5. in your text
  6. 98.09 g
20.
  1. in your text
  2. 120.38 g
  3. in your text
  4. 187.57 g
  5. in your text
  6. 94.11 g
21.
  1. in your text
  2. 3.11x10^5 mol PbO2
  3. in your text
  4. 2.45x10^-8 mol C2H3Cl3
  5. in your text
22.
  1. in your text
  2. 5.26 mol CuCl
  3. in your text
  4. 0.0697 mol SrF2
  5. 467 mol Al
23.
  1. in your text
  2. 0.149 g C6H6
  3. in your text
  4. 2.10 * 107 g C2H5O2
  5. 373 g Ca(NO3)2
24.
  1. in your text
  2. 4.96x105 g NCl5
  3. in your text
  4. 324 g H2O
  5. 1.00x10^4 g CuSO4
25.
  1. in your text
  2. 1.37 * 1023 molecules CO
  3. in your text
  4. 1.58 x1018 molecules H2O
  5. 4.03x1022 molecules C6H6
26.
  1. in your text
  2. 0.0159 mol S
  3. in your text
  4. 0.0254 mol S
27.
  1. in your text
  2. 36.48% Na, 25.44% S, 38.08% O
  3. in your text
  4. 29.08% Na, 40.56% S, 30.36% O
  5. in your text
  6. 44.90% K, .5787% H, 17.78% P, 36.74% O
  7. in your text
  8. 79.10% K, 20.88% P
28.
  1. in your text
  2. 44.29% Cu
  3. in your text
  4. 34.43% Fe
  5. in your text
  6. 13.41% Co
  7. in your text
8. 78.77% Sn
29.
  1. in your text
  2. 35.00% N
  3. in your text
  4. 52.56% CI
  5. in your text
  6. 39.99% C
  7. in your text
  8. 52.14% C
30.
  1. in your text
  2. 39.81% Cu2+
  3. in your text
  4. 63.51% Ag+
31. To determine the empirical formula of a new compound, the composition of the compound by mass must be known. To determine the molecular formula of the compound, the molar mass of the compound must also be known.
32. in your text
33.
  1. in your text
  2. C4H3O2
  3. in your text
  4. C2H3Cl
34.
  1. in your text
  2. no (it is not the same ratio)
  3. in your text
  4. no (they are not in the same ratio)
35. C3H2OCL
36. in your text
37. in your text
38. AlCl3
39. in your text
40. CaCl2
41. in your text
42. CuN2O6 (Cu(NO3)2)
43. in your text
44. The empirical formula of a compound represents only the smallest whole number relationship between the number and type of atoms in a compound, whereas the molecular formula represents the actual number of atoms of each type in a true molecule of the substance. Many compounds (for example, H20) may have the same empirical and molecular formulas.
45. in your text
46. C3H6O3
47. C6H12
48. in your text
49. empirical formula: C2H2ON. molecular formula: C6H6O3N3
50. in your text
51. 1,c 2,e 3,j 4,h 5,b 6,d 7,a 8, g 9, i 10, f
52. in your text
53. answers not available
54. MgO
55. in your text
56. 1,g 2,c 3,b 4,a 5,j 6, I 7, f 8, h 9, e 10, d
57. in your text
58. 2.36 g Co
59. CuSH10O9
60. in your text
61. in your text
62. in your text
63. HNO3
64. Nitrogen
65. empirical: C4H8O4S molecular: C4H8O4S (same as empirical)