chem 1413.001 - final exam – dec. 14, 2016 - version...
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CHEM 1413.001 - Final Exam – Dec. 14, 2016 - Version A
If you would like to have your grade posted on the course web site, using a four digit number, then please sign in the space below and put the number. If you do not wish to have your grade posted, you can still learn your grade by phone (940-382-1370) or E-mail ([email protected]). Please turn in this form with OR without posting number. ` I would like to have my final grade in CHEM 1413.001 posted on the course web site, and identified by the 4 digit number below. YES_________ NO_________ Name (Printed): ______________________________________ Signature: _______________________________________ Number (4 digits): ____________ Notes: If you use a number like 1234 or 1111, expect to try to decide which is
yours from among several different grades. You can keep the exam itself. Just turn in this form + your scantron
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CHEM 1413.001 - Final Exam – December 14, 2016 - Version A Constants:
R = 0.082 L-atm/mol-K R = 8.31 J/mol-K NA = 6.02x1023 mol-1
c = 3.00x108 m/s h = 6.63x10-34 J-s 1 amu = 1.66x10-24 g Conversion Factors: 1 atm. = 760 torr 1 L = 1.06 Qt Molar Masses: H - 1. He - 4. C - 12
N - 14. O - 16. P - 31.
Kr - 83.8 Se - 79. C5H12 - 72
H2O - 18. Cl2 - 71. PCl5 - 208.5
CH4 - 16. Fe(CO)5 - 195.8
Diatomic Molecular Orbital Energies: σ2s < σ*2s < π2p < σ2p < π*2p < σ*2p
Energy
Clausius-Clapeyron Equation: 2
1 2 1
1 1ln vapHPP R T T
∆ = − −
:
:
CHEM 1413.001 - Final Exam – Dec. 14, 2016 - Version A
(63) MULTIPLE CHOICE (Circle the ONE correct answer)
1. A 128Te2- ion has how many electrons (e) and neutrons (n)? (A) 52 e & 76 n (B) 50 e & 76 n (C) 54 e & 76 n (D) 54 e & 74 n
2. 5. g/m2 = ______ng/µm2 (A) 5x10-3 (B) 5x103 (C) 5x106 (D) 5x1021
3. The density of potassium is 0.86 g/mL. What is the volume, in Quarts (Qt.) of
0.50 kg of potassium? (A) 0.55 Qt. (B) 0.62 Qt. (C) 0.45 Qt. (D) 6.1x10-4 Qt.
4. Which one of the following formulas is incorrect?
(A) MgSO3 (B) Li2CO3 (C) (NH4)2S (D) Ga3(PO4)2
5. What is the formula of copper(II) nitrite? (A) CuNO2 (B) Cu(NO2)2 (C) Cu(NO3)2 (D) Cu2NO2
6. The name of the compound with the condensed structural formula,
CH3CBrCHCHCH2, is: (A) 4-bromo-1,3-pentadiene (B) 2-bromo-2,4-pentadiyne (C) 2-bromo-2,4-pentadiene (C) 4-bromopenta-2-ene,4-yne
7. The name of the molecule with the condensed structural formula,
CH3CH(CH3)CH2CH2CH2CH2NH2, is: (A) 5-methyl-1-hexanol (B) 2-methyl-6-hexanamine (C) 6-methyl-1-heptanamine (D) 5-methyl-1-hexanamine
8. A compound containing only selenium (Se) and oxygen (O) has the following
percent composition (by mass): 71.2% Se , 28.8% O. The empirical formula is: (A) SeO2 (B) Se2O (C) SeO (D) SeO3
9. How many atoms of hydrogen are in 20 grams of pentane, C5H12 ?
(A) 3.1x1022 (B) 2.5x1023 (C) 2.0x1024 (D) 2.5x1024
:
For #10-#14: Consider the reaction: 2 P(s) + 5 Cl2(g) → 2 PCl5(l).
10. What is the theoretical yield of PCl5 when 165 grams of Cl2 are reacted with an excess of P ? (A) 194 g (B) 1212 g (C) 485 g (D) 167 g
11. When 124 grams of P are reacted with 426 grams of Cl2, what is the theoretical
yield of PCl5 ? (A) 368 g (B) 312 g (C) 834 g (D) 500 g
12. When 124 grams of P are reacted with 426 grams of Cl2, ____ grams of
___ remain when the reaction is complete. (A) P 284 , Cl2 (B) 142.0 , Cl2 (C) 49.6 , P (D) 74.4 , P
13. When 213 grams of Cl2 reacts with an excess of P, 220 grams of PCl5 are
formed. The percent yield is: (A) 97% (B) 88% (C) 62% (D) 35%
14. How many moles of Cl2 are required to produce 4 moles of PCl5 if the percent
yield is 60% ? (A) 25.0 mol (B) 6.0 mol (C) 16.7 mol (D) 6.7 mol
15. When 20. grams of a compound containing carbon(C) and hydrogen(H) is burned completely in O2(g), 36. grams of H2O(l) is produced. What is the percent hydrogen (by mass) in this compound? (A) 13% (B) 40% (C) 32% (D) 20%
16. Which of the following solutions has the lowest total concentration of ions?
(A) 0.30 M KCl (B) 0.12 M Ba3(PO4)2 (C) 0.16 M Al(NO3)3 (D) 0.18 M Na2SO4
17. What is the Molarity of a solution prepared by mixing 150 mL of a 0.40 M sucrose
solution with 75 mL of a 0.20 M sucrose solution? (A) 0.33 M (B) 0.30 M (C) 0.23 M (D) 0.27 M
18. 360 mL of 0.15 M Ca(OH)2(aq) is required to completely neutralize 150 mL of an
aqueous HNO3(aq) solution. What is the Molarity of the HNO3(aq) solution? (A) 0.18 M (B) 0.36 M (C) 0.72 M (D) 0.57 M
:
For #19-#20: Consider the reaction: __Pb(NO3)2(aq) + __KCl(aq) → __PbCl2(s) + __KNO3(aq)
19. When 400 mL of 0.50 M Pb(NO3)2(aq) are reacted with 500 mL of
0.60 M KCl(aq), how many moles of PbCl2(s) can be formed (assuming a 100% yield)? (A) 0.15 mol (B) 0.10 mol (C) 0.20 mol (D) 0.30 mol
20. When 400 mL of 0.50 M Pb(NO3)2(aq) are reacted with 500 mL of
0.60 M KCl(aq), what will be the concentration of the excess reactant which remains in solution? (A) 0.125 M KCl (B) 0.056 M Pb(NO3)2 (C) 0.056 M KCl (D) 0.125 M Pb(NO3)2
21. The pressure of a gas is 25 lb/in2 in an 800 mL container at 30 oC. What is the
pressure, in lb/in2, if the volume is decreased to 500 mL and the temperature is increased to 130 oC? (A) 12 lb/in2 (B) 21 lb/in2 (C) 173 lb/in2 (D) 53 lb/in2
22. A sample of air in a 20 L container at 200 oC contains 3x1022 molecules. What is
the pressure of the air, in torr? (A) 0.10 torr (B) 31 torr (C) 73 torr (D) 7450 torr
23. A 10 L sample of air from King Tut’s sarcophagus at a total pressure of 0.90 atm.
and 20 oC was found to contain 5x10-5 moles of CO2(g). How many ppm (parts per million) of CO2(g) does this represent? (A) 1.3x102 ppm (B) 1.3x10-4 ppm (C) 1.3x10-10 ppm (D) 2.7x102 ppm
24. A mixture contains 0.80 mol of CH4(g) and 0.40 mol of CO2(g). The partial
pressure of CO2 is 1.40 atm. Therefore, the partial pressure of CH4 is ____ atm. and the total pressure is ____ atm. (A) 4.2 , 2.8 (B) 0.7 , 2.1 (C) 2.8 , 4.2 (D) cannot be determined without the volume and temperature of the mixture
25. What is the approximate density of CH4(g) at 10 oC and 2500 torr, in g/L
(A) 3.0 g/L (B) 2.3 g/L (C) 0.60 g/L (D) 1.8 g/L
26. Iron pentacarbonyl, Fe(CO)5(s), can be made by the reaction of Fe(s) with CO(g). If you have CO(g) in a 300. L flask at 400 torr and 50 oC, approximately how many grams of Fe(CO)5 can be produced by the reaction of the CO(g) with excess Fe(s)? (A) 230 g (B) 5840 g (C) 1170 g (D) 160 g
:
27. The rate of effusion of Kr(g) through a pinhole is 0.40 mol/min. Under the same
conditions, the rate of effusion of an unknown gas through the pinhole is 0.55 mol/min. Therefore, the Molar Mass of the unknown gas is: (A) 44 g/mol (B) 160 g/mol (C) 71 g/mol (D) 61 g/mol
28. Consider the reaction, 2 N2(g) + 5 O2(g) → 2 N2O5(g). Approximately how many
moles of N2O5 can be produced by the reaction of 90 L of N2(g) at 400 K and 1. atm. with 150 L of O2(g) at 400 K and 1. atm? (A) 1.37 mol (B) 0.91 mol (C) 2.74 mol (D) 1.82 mol
29. The Enthalpy of Vaporization of pentane, C5H12, is 26.8 kJ/mol and the constant
pressure molar heat capacity of the liquid is 150 J/mol-oC. The boiling point of pentane is 36 oC. What is the heat involved (in kJ) to condense 108 g of pentane(gas) to pentane(liq) at 36 oC and cool the liquid (at constant pressure), from 36 oC down to -50 oC (A) -20.8 kJ (B) -19.4 kJ (C) -59.6 kJ (D) -86.4 kJ
30. The constant volume heat capacity of Helium, He(g), is 12.5 J/mol-oC. When
1.40 kJ of heat is added to an 8 gram sample of He(g) at constant volume, the final temperature is 125 oC. What was the original temperature of the He(g) sample? (A) 56 oC (B) 69 oC (C) 181 oC (D) 84 oC
31. Consider the combustion of 3 moles of liquid benzene:
3 C6H6(l) + 22½ O2(g) → 18 CO2(g) + 9 H2O(l) ∆Ho = -9813 kJ From this value plus the Enthalpies of Formation of CO2(g) [-394 kJ/mol] and H2O(l) [-286 kJ/mol], one can determine that the Enthalpy of Formation of liquid benzene is: (A) +147 kJ/mol (B) -294 kJ/mol (C) +49 kJ/mol (D) -147 kJ/mol
32. Consider the reaction:
2 CH3OH(l) + 3 O2(g) → 2 CO2(g) + 4 H2O(l) ∆H = -1450 kJ For a given sample of CH3OH, the reaction’s enthalpy change is -725 kJ. How many grams of H2O are produced? (A) 9.0 g (B) 36.0 g (C) 2.2 g (D) 18.0 g
:
33. The energy of the H-H bond in H2 is 436 kJ/mol. What is the maximum
wavelength (in nm) of light that can break the H-H bond? (A) 2.75x10-7 nm (B) 110 nm (C) 275 nm (D) 242 nm
34. A diode laser emits light at a frequency of 7.5x1014 s-1. It emits photons at a rate
of 4.0x1018 photons/second. What is the approximate total energy of the radiation emitted in a 5 minute period? (A) 6,500 J (B) 10. J (C) 9.0x1035 J (D) 600. J
35. Consider the following Thermochemical equations:
2 SO2(g) + O2(g) → 2 SO3(g) ∆H = -196 kJ 4 S(s) + 6 O2(g) → 4 SO3(g) ∆H = -1580 kJ
Use these equations to determine ∆H for the reaction, SO2(g) → S(s) + O2(g). (A) +297 kJ (B) +692 kJ (C) +493 kJ (D) -493 kJ
36. The condensed electron configuration of Antimony (Sb , Z=51) is
(A) [Kr]5s24d105p3 (B) [Kr]5s25p3
(C) [Kr]5s25d105p3 (D) [Kr]4d104p5
37. Arrange the following atoms in order of decreasing radii: Sn , Cl , Se , Sb (A) Se > Cl > Sb > Sn (B) Cl > Se > Sb > Sn (C) Sn > Sb > Se > Cl (D) Cl > Se > Sn > Sb
38. Of the four atoms, Al, S, Ga, Se, ____ has the largest radius and ___ has the
largest First Ionization Energy. (A) Se , Al (B) S , Ga (C) Al , Se (D) Ga , S
39. Which of the following atoms is/are paramagnetic? Ge, Sr, Se
(A) Ge & Se (B) Sr (C) Ge & Sr (D) Ge, Sr & Se
40. Of the following bonds, _____ is the most polar and _____ is the least polar: Ga-Br, As-Br, Ga-Cl, Ge-Br (A) As-Br, Ga-Cl (B) Ga-Cl, As-Br (C) Ga-Br, As-Br (D) Ga-Cl, Ge-Br
41. In the NO+1 ion, the total number of lone pairs of electrons is _____ and the NO
Bond Order is ______: (A) 2 , 3 (B) 3 , 2 (C) 4 , 2 (D) 2 , 2
:
42. Of the molecules, CH2CH2, CHCH , CH3CH3, _________ has the highest
vibrational frequency, and ________ has the highest bond length (A) CH3CH3 , CH3CH3 (B) CHCH , CHCH (C) CH3CH3 , CHCH (D) CHCH , CH3CH3
43. Arrange the following in order of increasing phosphorus-oxygen Bond Lengths:
PO2-1 , PO+1 , PO-1
(A) PO2-1 < PO-1 < PO+1 (B) PO+1 < PO-1 < PO2
-1
(C) PO-1 < PO+1 < PO2-1 (D) PO+1 < PO2
-1 < PO-1
44. In the molecular ion, PCl4-1, the hybridization of the central atom is _____ and the electron pair geometry is: (A) sp3d , Trigonal Bipyramidal (B) sp3 , Tetrahedral (C) sp3d2 , Octahedral (D) sp3d2 , Square Pyramidal
45. In the molecular ion, PCl4-1, the molecular geometry is ______ and the molecule
is _______. (A) Trigonal Pyramidal , Polar (B) Trigonal Planar , non-Polar
(C) See-Sar , Polar (D) T-Shaped , Polar
46. In the molecular ion AsCl2-1, the electron pair geometry is _____ and the ion is ______. (A) tetrahedral , polar (B) trigonal bipyramidal , non-polar (C) bipyramidal , polar (D) trigonal planar , polar
47. In the molecular ion, BrF4
-1, the hybridization of the central atom is _____ and the electron pair geometry is: (A) sp3d , Trigonal Bipyramidal (B) sp3d2 , Octahedral (C) sp3d , SeeSaw (D) sp3d2 , Square Planar
48. In the molecular ion, BrF4
-1, the molecular geometry is _______ and the ion is: (A) SeeSaw , Polar (B) Tetrahedral , Non-Polar (C) Square Planar, Non-Polar (D) Octahedral , Non-Polar
:
49. In the molecular ion NS2-1, the hybridization of the central atom is ____ and the
electron pair geometry is ____. (A) sp3 , tetrahedral (B) sp2 , bent, (C) trigonal planar (D) sp , linear
50. In the molecular ion, AsO3
-1, the hybridization of the central atom is _____ and the molecular geometry is: (A) sp3 , Tetrahedral (B) sp2 , Trigonal Planar (C) sp3d , Trigonal Bipyramidal (D) sp2 , Trigonal Pyramidal
51. In the molecule, FSiP (Si in center) , the hybridization of the central atom is
_____ and the electron pair geometry is: (A) sp , Linear (B) sp2 , Trigonal Planar (C) sp3 , Linear (D) sp2 , Bent
52. Which of the following molecules is/are polar: SbF5 , BrF5 , XeF4 , AsF3 ?
(A) BrF5 only (B) XeF4 and AsF3 (C) BrF5 and AsF3 (D) XeF4 only
53. For the molecule with the condensed structural formula CH(O)CN, the hybridization of the carbon on the right is ____ and the O-C-C bond angle is ____. (A) sp2 , 120o (B) sp3 , 109.5o (C) sp2 , 109.5o (D) sp , 120o
54. In the molecule CH2CHNH2 the hybridization of the second carbon (closer to
right) is ____ and the C-C-N angle is: (A) sp2 , 120o (B) sp , 180o (C) sp3 , 109.5o (D) sp2 , 109.5o
55. Of the diatomic molecules or molecular ions, CF , CF+1 , CF-1, ____ has the
shortest bond length and ____ has the lowest vibrational frequency.
(A) CF-1 , CF (B) CF+1 , CF-1 (C) CF , CF+1 (D) CF-1 , CF+1
56. The OF bond order in the diatomic molecular ion, OF+1 , is ______, and this diatomic molecular ion is _______. (A) 1.5 , paramagneticc (B) 2.0 , paraagnetic (C) 2.0 , diamagnetic (D) 3.0 , diamagnetic
:
57. What type of intermolecular attractive forces are present between molecules of
trimethylamine, NH(CH3)2 ? (A) London Dispersion (B) London Dispersion, Dipole-Dipole and Hydrogen Bonding (C) London Dispersion and Dipole-Dipole (D) Dipole-Dipole and Hydrogen Bonding
58. Arrange the following molecules in order of decreasing boiling points:
GeH3Cl , CH4 , CH3Cl (A) GeH3Cl > CH4 > CH3Cl (B) CH4 > CH3Cl > GeH3Cl
(C) GeH3Cl > CH3Cl > CH4 (D) CH4 > GeH3Cl > CH3Cl
59. Arrange the following molecules in the order of increasing volatility (at room temperature): CH3CH2CH3 , CH3CH2OH , CH3OCH3 (A) CH3OCH3 < CH3CH2OH < CH3CH2CH3 (B) CH3CH2CH3 < CH3OCH3 < CH3CH2OH (C) CH3CH2OH < CH3OCH3 < CH3CH2CH3 (D) CH3CH2CH3 < CH3CH2OH < CH3OCH3
For #60 - #62, consider the phase diagram to the right.
60. The curve corresponding to solid and vapor in equilibrium is (A) A-B (B) A-D (C) A-C (D) C-D
61. At pressures below the triple point pressure the substance can exist as
(A) solid or liquid (B) solid or liquid or vapor (C) vapor only (D) solid or vapor
B
A
C
D T
P
:
62. If the applied pressure on the substance is decreased from 100 atm. to 1 atm.,
(A) the melting point will increase and the boiling point will decrease (B) the melting point will decrease and the boiling point will increase (C) the melting point will decrease and the boiling point will increase (D) the melting point will increase and the boiling point will increase
63. The normal boiling point of napthalene is 220 oC (this is the temperature at which
the vapor pressure is 1 atm. = 760 torr). The enthalpy of vaporization of napthalene is 70. kJ/mol.
What is the vapor pressure of anthracene at 300 oC (in torr)? (A) 1.85x104 torr (B) 8.25x103 torr (C) 2.07x107 torr (D) 70 torr
:
CHEM 1413.001 - Final Exam – Dec. 14, 2016 - Version B If you would like to have your grade posted on the course web site, using a four digit number, then please sign in the space below and put the number. If you do not wish to have your grade posted, you can still learn your grade by phone (940-382-1370) or E-mail ([email protected]). Please turn in this form with OR without posting number. ` I would like to have my final grade in CHEM 1413.001 posted on the course web site, and identified by the 4 digit number below. YES_________ NO_________ Name (Printed): ______________________________________ Signature: _______________________________________ Number (4 digits): ____________ Notes: If you use a number like 1234 or 1111, expect to try to decide which is
yours from among several different grades. You can keep the exam itself. Just turn in this form + your scantron
with your name on it
:
CHEM 1413.001 - Final Exam – December 14, 2016 - Version B Constants:
R = 0.082 L-atm/mol-K R = 8.31 J/mol-K NA = 6.02x1023 mol-1
c = 3.00x108 m/s h = 6.63x10-34 J-s 1 amu = 1.66x10-24 g Conversion Factors: 1 atm. = 760 torr 1 L = 1.06 Qt Molar Masses: H - 1. He - 4. C - 12
N - 14. O - 16. P - 31.
Kr - 83.8 Se - 79. C5H12 - 72
H2O - 18. Cl2 - 71. PCl5 - 208.5
CH4 - 16. Fe(CO)5 - 195.8
Diatomic Molecular Orbital Energies: σ2s < σ*2s < π2p < σ2p < π*2p < σ*2p
Energy
Clausius-Clapeyron Equation: 2
1 2 1
1 1ln vapHPP R T T
∆ = − −
:
:
CHEM 1413.001 - Final Exam – Dec. 14, 2016 - Version B
(63) MULTIPLE CHOICE (Circle the ONE correct answer)
1. A 128Te2- ion has how many electrons (e) and neutrons (n)? (A) 52 e & 76 n (B) 50 e & 76 n (C) 54 e & 76 n (D) 54 e & 74 n
2. 5. g/m2 = ______ng/µm2 (A) 5x10-3 (B) 5x103 (C) 5x106 (D) 5x1021
3. The density of potassium is 0.86 g/mL. What is the volume, in Quarts (Qt.) of
0.50 kg of potassium? (A) 0.55 Qt. (B) 0.62 Qt. (C) 0.45 Qt. (D) 6.1x10-4 Qt.
4. Which one of the following formulas is incorrect?
(A) MgSO3 (B) Li2CO3 (C) (NH4)2S (D) Ga3(PO4)2
5. What is the formula of copper(II) nitrite? (A) CuNO2 (B) Cu(NO2)2 (C) Cu(NO3)2 (D) Cu2NO2
6. The name of the compound with the condensed structural formula,
CH3CBrCHCHCH2, is: (A) 4-bromo-1,3-pentadiene (B) 2-bromo-2,4-pentadiyne (C) 2-bromo-2,4-pentadiene (C) 4-bromopenta-2-ene,4-yne
7. The name of the molecule with the condensed structural formula,
CH3CH(CH3)CH2CH2CH2CH2NH2, is: (A) 5-methyl-1-hexanol (B) 2-methyl-6-hexanamine (C) 6-methyl-1-heptanamine (D) 5-methyl-1-hexanamine
8. A compound containing only selenium (Se) and oxygen (O) has the following
percent composition (by mass): 71.2% Se , 28.8% O. The empirical formula is: (A) SeO2 (B) Se2O (C) SeO (D) SeO3
9. How many atoms of hydrogen are in 20 grams of pentane, C5H12 ?
(A) 3.1x1022 (B) 2.5x1023 (C) 2.0x1024 (D) 2.5x1024
:
For #10-#14: Consider the reaction: 2 P(s) + 5 Cl2(g) → 2 PCl5(l).
10. What is the theoretical yield of PCl5 when 165 grams of Cl2 are reacted with an excess of P ? (A) 194 g (B) 1212 g (C) 485 g (D) 167 g
11. When 124 grams of P are reacted with 426 grams of Cl2, what is the theoretical
yield of PCl5 ? (A) 368 g (B) 312 g (C) 834 g (D) 500 g
12. When 124 grams of P are reacted with 426 grams of Cl2, ____ grams of
___ remain when the reaction is complete. (A) P 284 , Cl2 (B) 142.0 , Cl2 (C) 49.6 , P (D) 74.4 , P
13. When 213 grams of Cl2 reacts with an excess of P, 220 grams of PCl5 are
formed. The percent yield is: (A) 97% (B) 88% (C) 62% (D) 35%
14. How many moles of Cl2 are required to produce 4 moles of PCl5 if the percent
yield is 60% ? (A) 25.0 mol (B) 6.0 mol (C) 16.7 mol (D) 6.7 mol
15. When 20. grams of a compound containing carbon(C) and hydrogen(H) is burned completely in O2(g), 36. grams of H2O(l) is produced. What is the percent hydrogen (by mass) in this compound? (A) 13% (B) 40% (C) 32% (D) 20%
16. Which of the following solutions has the lowest total concentration of ions?
(A) 0.30 M KCl (B) 0.12 M Ba3(PO4)2 (C) 0.16 M Al(NO3)3 (D) 0.18 M Na2SO4
17. What is the Molarity of a solution prepared by mixing 150 mL of a 0.40 M sucrose
solution with 75 mL of a 0.20 M sucrose solution? (A) 0.33 M (B) 0.30 M (C) 0.23 M (D) 0.27 M
18. 360 mL of 0.15 M Ca(OH)2(aq) is required to completely neutralize 150 mL of an
aqueous HNO3(aq) solution. What is the Molarity of the HNO3(aq) solution? (A) 0.18 M (B) 0.36 M (C) 0.72 M (D) 0.57 M
:
For #19-#20: Consider the reaction: __Pb(NO3)2(aq) + __KCl(aq) → __PbCl2(s) + __KNO3(aq)
19. When 400 mL of 0.50 M Pb(NO3)2(aq) are reacted with 500 mL of
0.60 M KCl(aq), how many moles of PbCl2(s) can be formed (assuming a 100% yield)? (A) 0.15 mol (B) 0.10 mol (C) 0.20 mol (D) 0.30 mol
20. When 400 mL of 0.50 M Pb(NO3)2(aq) are reacted with 500 mL of
0.60 M KCl(aq), what will be the concentration of the excess reactant which remains in solution? (A) 0.125 M KCl (B) 0.056 M Pb(NO3)2 (C) 0.056 M KCl (D) 0.125 M Pb(NO3)2
21. The pressure of a gas is 25 lb/in2 in an 800 mL container at 30 oC. What is the
pressure, in lb/in2, if the volume is decreased to 500 mL and the temperature is increased to 130 oC? (A) 12 lb/in2 (B) 21 lb/in2 (C) 173 lb/in2 (D) 53 lb/in2
22. A sample of air in a 20 L container at 200 oC contains 3x1022 molecules. What is
the pressure of the air, in torr? (A) 0.10 torr (B) 31 torr (C) 73 torr (D) 7450 torr
23. A 10 L sample of air from King Tut’s sarcophagus at a total pressure of 0.90 atm.
and 20 oC was found to contain 5x10-5 moles of CO2(g). How many ppm (parts per million) of CO2(g) does this represent? (A) 1.3x102 ppm (B) 1.3x10-4 ppm (C) 1.3x10-10 ppm (D) 2.7x102 ppm
24. A mixture contains 0.80 mol of CH4(g) and 0.40 mol of CO2(g). The partial
pressure of CO2 is 1.40 atm. Therefore, the partial pressure of CH4 is ____ atm. and the total pressure is ____ atm. (A) 4.2 , 2.8 (B) 0.7 , 2.1 (C) 2.8 , 4.2 (D) cannot be determined without the volume and temperature of the mixture
25. What is the approximate density of CH4(g) at 10 oC and 2500 torr, in g/L
(A) 3.0 g/L (B) 2.3 g/L (C) 0.60 g/L (D) 1.8 g/L
26. Iron pentacarbonyl, Fe(CO)5(s), can be made by the reaction of Fe(s) with CO(g). If you have CO(g) in a 300. L flask at 400 torr and 50 oC, approximately how many grams of Fe(CO)5 can be produced by the reaction of the CO(g) with excess Fe(s)? (A) 230 g (B) 5840 g (C) 1170 g (D) 160 g
:
27. The rate of effusion of Kr(g) through a pinhole is 0.40 mol/min. Under the same
conditions, the rate of effusion of an unknown gas through the pinhole is 0.55 mol/min. Therefore, the Molar Mass of the unknown gas is: (A) 44 g/mol (B) 160 g/mol (C) 71 g/mol (D) 61 g/mol
28. Consider the reaction, 2 N2(g) + 5 O2(g) → 2 N2O5(g). Approximately how many
moles of N2O5 can be produced by the reaction of 90 L of N2(g) at 400 K and 1. atm. with 150 L of O2(g) at 400 K and 1. atm? (A) 1.37 mol (B) 0.91 mol (C) 2.74 mol (D) 1.82 mol
29. The Enthalpy of Vaporization of pentane, C5H12, is 26.8 kJ/mol and the constant
pressure molar heat capacity of the liquid is 150 J/mol-oC. The boiling point of pentane is 36 oC. What is the heat involved (in kJ) to condense 108 g of pentane(gas) to pentane(liq) at 36 oC and cool the liquid (at constant pressure), from 36 oC down to -50 oC (A) -20.8 kJ (B) -19.4 kJ (C) -59.6 kJ (D) -86.4 kJ
30. The constant volume heat capacity of Helium, He(g), is 12.5 J/mol-oC. When
1.40 kJ of heat is added to an 8 gram sample of He(g) at constant volume, the final temperature is 125 oC. What was the original temperature of the He(g) sample? (A) 56 oC (B) 69 oC (C) 181 oC (D) 84 oC
31. Consider the combustion of 3 moles of liquid benzene:
3 C6H6(l) + 22½ O2(g) → 18 CO2(g) + 9 H2O(l) ∆Ho = -9813 kJ From this value plus the Enthalpies of Formation of CO2(g) [-394 kJ/mol] and H2O(l) [-286 kJ/mol], one can determine that the Enthalpy of Formation of liquid benzene is: (A) +147 kJ/mol (B) -294 kJ/mol (C) +49 kJ/mol (D) -147 kJ/mol
32. Consider the reaction:
2 CH3OH(l) + 3 O2(g) → 2 CO2(g) + 4 H2O(l) ∆H = -1450 kJ For a given sample of CH3OH, the reaction’s enthalpy change is -725 kJ. How many grams of H2O are produced? (A) 9.0 g (B) 36.0 g (C) 2.2 g (D) 18.0 g
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33. The energy of the H-H bond in H2 is 436 kJ/mol. What is the maximum
wavelength (in nm) of light that can break the H-H bond? (A) 2.75x10-7 nm (B) 110 nm (C) 275 nm (D) 242 nm
34. A diode laser emits light at a frequency of 7.5x1014 s-1. It emits photons at a rate
of 4.0x1018 photons/second. What is the approximate total energy of the radiation emitted in a 5 minute period? (A) 6,500 J (B) 10. J (C) 9.0x1035 J (D) 600. J
35. Consider the following Thermochemical equations:
2 SO2(g) + O2(g) → 2 SO3(g) ∆H = -196 kJ 4 S(s) + 6 O2(g) → 4 SO3(g) ∆H = -1580 kJ
Use these equations to determine ∆H for the reaction, SO2(g) → S(s) + O2(g). (A) +297 kJ (B) +692 kJ (C) +493 kJ (D) -493 kJ
36. The condensed electron configuration of Antimony (Sb , Z=51) is
(A) [Kr]5s24d105p3 (B) [Kr]5s25p3
(C) [Kr]5s25d105p3 (D) [Kr]4d104p5
37. Arrange the following atoms in order of decreasing radii: Sn , Cl , Se , Sb (A) Se > Cl > Sb > Sn (B) Cl > Se > Sb > Sn (C) Sn > Sb > Se > Cl (D) Cl > Se > Sn > Sb
38. Of the four atoms, Al, S, Ga, Se, ____ has the largest radius and ___ has the
largest First Ionization Energy. (A) Se , Al (B) S , Ga (C) Al , Se (D) Ga , S
39. Which of the following atoms is/are paramagnetic? Ge, Sr, Se
(A) Ge & Se (B) Sr (C) Ge & Sr (D) Ge, Sr & Se
40. Of the following bonds, _____ is the most polar and _____ is the least polar: Ga-Br, As-Br, Ga-Cl, Ge-Br (A) As-Br, Ga-Cl (B) Ga-Cl, As-Br (C) Ga-Br, As-Br (D) Ga-Cl, Ge-Br
41. In the NO+1 ion, the total number of lone pairs of electrons is _____ and the NO
Bond Order is ______: (A) 2 , 3 (B) 3 , 2 (C) 4 , 2 (D) 2 , 2
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42. Of the molecules, CH2CH2, CHCH , CH3CH3, _________ has the highest
vibrational frequency, and ________ has the highest bond length (A) CH3CH3 , CH3CH3 (B) CHCH , CHCH (C) CH3CH3 , CHCH (D) CHCH , CH3CH3
43. Arrange the following in order of increasing phosphorus-oxygen Bond Lengths:
PO2-1 , PO+1 , PO-1
(A) PO2-1 < PO-1 < PO+1 (B) PO+1 < PO-1 < PO2
-1
(C) PO-1 < PO+1 < PO2-1 (D) PO+1 < PO2
-1 < PO-1
44. In the molecular ion, PCl4-1, the hybridization of the central atom is _____ and the electron pair geometry is: (A) sp3d , Trigonal Bipyramidal (B) sp3 , Tetrahedral (C) sp3d2 , Octahedral (D) sp3d2 , Square Pyramidal
45. In the molecular ion, PCl4-1, the molecular geometry is ______ and the molecule
is _______. (A) Trigonal Pyramidal , Polar (B) Trigonal Planar , non-Polar
(C) See-Sar , Polar (D) T-Shaped , Polar
46. In the molecular ion AsCl2-1, the electron pair geometry is _____ and the ion is ______. (A) tetrahedral , polar (B) trigonal bipyramidal , non-polar (C) bipyramidal , polar (D) trigonal planar , polar
47. In the molecular ion, BrF4
-1, the hybridization of the central atom is _____ and the electron pair geometry is: (A) sp3d , Trigonal Bipyramidal (B) sp3d2 , Octahedral (C) sp3d , SeeSaw (D) sp3d2 , Square Planar
48. In the molecular ion, BrF4
-1, the molecular geometry is _______ and the ion is: (A) SeeSaw , Polar (B) Tetrahedral , Non-Polar (C) Square Planar, Non-Polar (D) Octahedral , Non-Polar
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49. In the molecular ion NS2-1, the hybridization of the central atom is ____ and the
electron pair geometry is ____. (A) sp3 , tetrahedral (B) sp2 , bent, (C) trigonal planar (D) sp , linear
50. In the molecular ion, AsO3
-1, the hybridization of the central atom is _____ and the molecular geometry is: (A) sp3 , Tetrahedral (B) sp2 , Trigonal Planar (C) sp3d , Trigonal Bipyramidal (D) sp2 , Trigonal Pyramidal
51. In the molecule, FSiP (Si in center) , the hybridization of the central atom is
_____ and the electron pair geometry is: (A) sp , Linear (B) sp2 , Trigonal Planar (C) sp3 , Linear (D) sp2 , Bent
52. Which of the following molecules is/are polar: SbF5 , BrF5 , XeF4 , AsF3 ?
(A) BrF5 only (B) XeF4 and AsF3 (C) BrF5 and AsF3 (D) XeF4 only
53. For the molecule with the condensed structural formula CH(O)CN, the hybridization of the carbon on the right is ____ and the O-C-C bond angle is ____. (A) sp2 , 120o (B) sp3 , 109.5o (C) sp2 , 109.5o (D) sp , 120o
54. In the molecule CH2CHNH2 the hybridization of the second carbon (closer to
right) is ____ and the C-C-N angle is: (A) sp2 , 120o (B) sp , 180o (C) sp3 , 109.5o (D) sp2 , 109.5o
55. Of the diatomic molecules or molecular ions, CF , CF+1 , CF-1, ____ has the
shortest bond length and ____ has the lowest vibrational frequency.
(A) CF-1 , CF (B) CF+1 , CF-1 (C) CF , CF+1 (D) CF-1 , CF+1
56. The OF bond order in the diatomic molecular ion, OF+1 , is ______, and this diatomic molecular ion is _______. (A) 1.5 , paramagneticc (B) 2.0 , paraagnetic (C) 2.0 , diamagnetic (D) 3.0 , diamagnetic
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57. What type of intermolecular attractive forces are present between molecules of
trimethylamine, NH(CH3)2 ? (A) London Dispersion (B) London Dispersion, Dipole-Dipole and Hydrogen Bonding (C) London Dispersion and Dipole-Dipole (D) Dipole-Dipole and Hydrogen Bonding
58. Arrange the following molecules in order of decreasing boiling points:
GeH3Cl , CH4 , CH3Cl (A) GeH3Cl > CH4 > CH3Cl (B) CH4 > CH3Cl > GeH3Cl
(C) GeH3Cl > CH3Cl > CH4 (D) CH4 > GeH3Cl > CH3Cl
59. Arrange the following molecules in the order of increasing volatility (at room temperature): CH3CH2CH3 , CH3CH2OH , CH3OCH3 (A) CH3OCH3 < CH3CH2OH < CH3CH2CH3 (B) CH3CH2CH3 < CH3OCH3 < CH3CH2OH (C) CH3CH2OH < CH3OCH3 < CH3CH2CH3 (D) CH3CH2CH3 < CH3CH2OH < CH3OCH3
For #60 - #62, consider the phase diagram to the right.
60. The curve corresponding to solid and vapor in equilibrium is (A) A-B (B) A-D (C) A-C (D) C-D
61. At pressures below the triple point pressure the substance can exist as
(A) solid or liquid (B) solid or liquid or vapor (C) vapor only (D) solid or vapor
B
A
C
D T
P
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62. If the applied pressure on the substance is decreased from 100 atm. to 1 atm.,
(A) the melting point will increase and the boiling point will decrease (B) the melting point will decrease and the boiling point will increase (C) the melting point will decrease and the boiling point will increase (D) the melting point will increase and the boiling point will increase
63. The normal boiling point of napthalene is 220 oC (this is the temperature at which
the vapor pressure is 1 atm. = 760 torr). The enthalpy of vaporization of napthalene is 70. kJ/mol.
What is the vapor pressure of anthracene at 300 oC (in torr)? (A) 1.85x104 torr (B) 8.25x103 torr (C) 2.07x107 torr (D) 70 torr
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