The combustion of propane 3 8 (C H ) in the presence of excess oxygen yields 2 CO and 2 H O : 3 8 2 2 2 C H (g) + 5O (g)®3CO (g) + 4H O (g) When 2.5 mol of 2 O are consumed in their reaction, __________ mol of 2 CO are produced. A) 1.5 B) 3.0 C) 5.0 D) 6.0 E) 2.5

The combustion of propane 3 8 (C H ) in the presence of excess oxygen yields 2 CO and 2 H O : 3 8 2 2 2 C H (g) + 5O (g)®3CO (g) + 4H O (g) When 2.5 mol of 2 O are consumed in their reaction, __________ mol of 2 CO are produced. A) 1.5 B) 3.0 C) 5.0 D) 6.0 E) 2.5

A) 1.5 The combustion of propane 3 8 (C H … Read More...
CHM114: Exam #3 CHM 114 Exam #3 Practice Exam (Chapters 9.1-9.4, 9.6, 10, 11.1-11.6, 13.1-13.5) Instructor: O. Graudejus Points: 100 Print Name Sign Name Student I.D. # 1. You are responsible for the information on this page. Please read it carefully. 2. If you enter your ASU ID incorrectly on the scantron, a 3 point penalty will be assessed. 3. Code your name and 10 digit affiliate identification number on the separate scantron answer sheet. Use only a #2 pencil 4. Do all calculations on the exam pages. Do not make any unnecessary marks on the answer sheet. 5. This exam consists of 25 multiple choice questions worth 4 points each and a periodic table. Make sure you have them all. 6. Choose the best answer to each of the questions and answer it on the computer-graded answer sheet. Read all responses before making a selection. 7. Read the directions carefully for each problem. 8. Avoid even casual glances at other students’ exams. 9. Stop writing and hand in your scantron answer sheet and your test promptly when instructed. LATE EXAMS MAY HAVE POINTS DEDUCTED. 10. You will have 50 minutes to complete the exam. 11. If you leave early, please do so quietly. 12. Work the easiest problems first. 13. A periodic table is attached as the last page to this exam. 14. Answers will be posted online this afternoon. Potentially useful information: K = ºC + 273.15 PV=nRT R=8.314 J·K-1·mol-1 DE = q + w 760 torr = 1 atm = 101325 Pa = 1.013 bar Avogadro’s Number = 6.022 × 1023 particles/mole q = (Sp. Heat) × m × DT (Specific Heatwater = 4.184 J/g°C) 1 2 2 3 2 ( is a constant) KE mv KE RT R = = M RT u 3 = \ -2- CHM 114: Exam #3 1) Of the following molecules, only __________ is polar. A) CCl4 B) BCl3 C) NCl3 D) BeCl2 E) Cl2 2) The molecular geometry of the CHF3 molecule is __________, and the molecule is __________. A) trigonal pyramidal, polar B) tetrahedral, nonpolar C) seesaw, nonpolar D) tetrahedral, polar E) seesaw, polar 3) The electron-domain geometry of __________ is tetrahedral. A) 4 CBr B) 3 PH C) 2 2 CCl Br D) 4 XeF E) all of the above except 4 XeF 4) Of the following substances, only __________ has London dispersion forces as its only intermolecular force. A) H2O B) CCl4 C) HF D) CH3COOH E) PH3 5) The principal reason for the extremely low solubility of NaCl in benzene (C6H6) is the __________. A) strong solvent-solvent interactions B) hydrogen bonding in C6H6 C) strength of the covalent bond in NaCl D) weak solvation (interaction) of Na+ and Cl- by C6H6 E) increased disorder due to mixing of solute and solvent -3- CHM 114: Exam #3 6) There are __________  and __________  bonds in the H −C º C−H molecule. A) 3 and 2 B) 3 and 4 C) 4 and 3 D) 2 and 3 E) 5 and 0 7) A sample of a gas (5.0 mol) at 1.0 atm is expanded at constant temperature from 10 L to 15 L. The final pressure is __________ atm. A) 1.5 B) 7.5 C) 0.67 D) 3.3 E) 15 8) A mixture of He and Ne at a total pressure of 0.95 atm is found to contain 0.32 mol of He and 0.56 mol of Ne. The partial pressure of Ne is __________ atm. A) 1.7 B) 1.5 C) 0.60 D) 0.35 E) 1.0 9) Automobile air bags use the decomposition of sodium azide as their source of gas for rapid inflation: 3 2 2NaN (s)®2Na (s) + 3N (g) . What mass (g) of 3 NaN is required to provide 40.0 L of 2 N at 25.0 °C and 763 torr? A) 1.64 B) 1.09 C) 160 D) 71.1  10) The reaction of 50 mL of 2 Cl gas with 50 mL of 4 CH gas via the equation: 2 4 3 Cl (g) + CH (g)®HCl (g) + CH Cl (g) will produce a total of __________ mL of products if pressure and temperature are kept constant. A) 100 B) 50 C) 200 D) 150 E) 250 -4- CHM 114: Exam #3 11) The density of 2 N O at 1.53 atm and 45.2 °C is __________ g/L. A) 18.2 B) 1.76 C) 0.388 D) 9.99 E) 2.58 12) A gas at a pressure of 325 torr exerts a force of __________ N on an area of 2 5.5 m . A)1.8×103 B) 59 C) 5 2.4×10 D) 0.018 E) 2.4 13) According to kinetic-molecular theory, in which of the following gases will the root-mean-square speed of the molecules be the highest at 200 °C? A) HCl B) 2 Cl C) 2 H O D) 6 SF E) None. The molecules of all gases have the same root-mean-square speed at any given temperature. 14) A real gas will behave most like an ideal gas under conditions of __________. A) high temperature and high pressure B) high temperature and low pressure C) low temperature and high pressure D) low temperature and low pressure E) STP 15) Elemental iodine (I2) is a solid at room temperature. What is the major attractive force that exists among different I2 molecules in the solid? A) London dispersion forces B) dipole-dipole rejections C) ionic-dipole interactions D) covalent-ionic interactions E) dipole-dipole attractions -5- CHM 114: Exam #3 16) The heat of fusion of water is 6.01 kJ/mol. The heat capacity of liquid water is 75.3 Jmol-1K-1. The conversion of 50.0 g of ice at 0.00 °C to liquid water at 22.0 °C requires __________ kJ of heat. A) 3.8×102 B) 21.3 C) 17.2 D) 0.469 E) Insufficient data are given. 17) Of the following substances, __________ has the highest boiling point. A) 2 H O B) 2 CO C) 4 CH D) Kr E) SF4 18) Which statements about viscosity are true? (i) Viscosity increases as temperature decreases. (ii) Viscosity increases as molecular weight increases. (iii) Viscosity increases as intermolecular forces increase. A) (i) only B) (ii) and (iii) C) (i) and (iii) D) none E) all 19) Based on molecular mass and dipole moment of the five compounds in the table below, which should have the highest boiling point? A) 3 2 3 CH CH CH B) 3 3 CH OCH C) 3 CH Cl D) 3 CH CHO E) 3 CH CN -6- CHM 114: Exam #3 20) On the phase diagram shown above, the coordinates of point __________ correspond to the critical temperature and pressure. A) A B) B C) C D) D E) E 21) The vapor pressure of pure ethanol at 60 °C is 0.459 atm. Raoult’s Law predicts that a solution prepared by dissolving 10.0 mmol naphthalene (nonvolatile) in 90.0 mmol ethanol will have a vapor pressure of _______ atm. A) 0.498 B) 0.413 C) 0.790 D) 0.367 E) 0.0918 Of the following, a 0.1 M aqueous solution of __________ will have the highest freezing point. A) NaCl B) Al(NO3)3 C) K2CrO4 D) Na2SO4 E) sucrose (a sugar) 23) What is the freezing point (°C) of a solution prepared by dissolving 11.3 g of Ca(NO3)2 (formula weight = 164 g/mol) in 115 g of water? The molal freezing point depression constant for water is 1.86 °C/m. A) -3.34 B) -1.11 C) 3.34 D) 1.11 E) 0.00 -7- CHM 114: Exam #3 24) The phase changes B  C and D  E are not associated with temperature increases because the heat energy is used up to __________. A) break intermolecular bonds B) break intramolecular bonds C) rearrange atoms within molecules D) increase the velocity of molecules E) increase the density of the sample 25) Ammonium nitrate (NH4NO3) dissolves readily in water even though the dissolution is endothermic by 26.4 kJ/mol. The solution process is spontaneous because __________. A) the vapor pressure of the water decreases upon addition of the solute B) the ammonium and the nitrate ion both contain nitrogen C) of the decrease in enthalpy upon addition of the solute D) of the increase in enthalpy upon dissolution of this strong electrolyte E) of the increase in disorder (entropy) upon dissolution of this strong electrolyte    -8- CHM 114: Exam #3

CHM114: Exam #3 CHM 114 Exam #3 Practice Exam (Chapters 9.1-9.4, 9.6, 10, 11.1-11.6, 13.1-13.5) Instructor: O. Graudejus Points: 100 Print Name Sign Name Student I.D. # 1. You are responsible for the information on this page. Please read it carefully. 2. If you enter your ASU ID incorrectly on the scantron, a 3 point penalty will be assessed. 3. Code your name and 10 digit affiliate identification number on the separate scantron answer sheet. Use only a #2 pencil 4. Do all calculations on the exam pages. Do not make any unnecessary marks on the answer sheet. 5. This exam consists of 25 multiple choice questions worth 4 points each and a periodic table. Make sure you have them all. 6. Choose the best answer to each of the questions and answer it on the computer-graded answer sheet. Read all responses before making a selection. 7. Read the directions carefully for each problem. 8. Avoid even casual glances at other students’ exams. 9. Stop writing and hand in your scantron answer sheet and your test promptly when instructed. LATE EXAMS MAY HAVE POINTS DEDUCTED. 10. You will have 50 minutes to complete the exam. 11. If you leave early, please do so quietly. 12. Work the easiest problems first. 13. A periodic table is attached as the last page to this exam. 14. Answers will be posted online this afternoon. Potentially useful information: K = ºC + 273.15 PV=nRT R=8.314 J·K-1·mol-1 DE = q + w 760 torr = 1 atm = 101325 Pa = 1.013 bar Avogadro’s Number = 6.022 × 1023 particles/mole q = (Sp. Heat) × m × DT (Specific Heatwater = 4.184 J/g°C) 1 2 2 3 2 ( is a constant) KE mv KE RT R = = M RT u 3 = \ -2- CHM 114: Exam #3 1) Of the following molecules, only __________ is polar. A) CCl4 B) BCl3 C) NCl3 D) BeCl2 E) Cl2 2) The molecular geometry of the CHF3 molecule is __________, and the molecule is __________. A) trigonal pyramidal, polar B) tetrahedral, nonpolar C) seesaw, nonpolar D) tetrahedral, polar E) seesaw, polar 3) The electron-domain geometry of __________ is tetrahedral. A) 4 CBr B) 3 PH C) 2 2 CCl Br D) 4 XeF E) all of the above except 4 XeF 4) Of the following substances, only __________ has London dispersion forces as its only intermolecular force. A) H2O B) CCl4 C) HF D) CH3COOH E) PH3 5) The principal reason for the extremely low solubility of NaCl in benzene (C6H6) is the __________. A) strong solvent-solvent interactions B) hydrogen bonding in C6H6 C) strength of the covalent bond in NaCl D) weak solvation (interaction) of Na+ and Cl- by C6H6 E) increased disorder due to mixing of solute and solvent -3- CHM 114: Exam #3 6) There are __________  and __________  bonds in the H −C º C−H molecule. A) 3 and 2 B) 3 and 4 C) 4 and 3 D) 2 and 3 E) 5 and 0 7) A sample of a gas (5.0 mol) at 1.0 atm is expanded at constant temperature from 10 L to 15 L. The final pressure is __________ atm. A) 1.5 B) 7.5 C) 0.67 D) 3.3 E) 15 8) A mixture of He and Ne at a total pressure of 0.95 atm is found to contain 0.32 mol of He and 0.56 mol of Ne. The partial pressure of Ne is __________ atm. A) 1.7 B) 1.5 C) 0.60 D) 0.35 E) 1.0 9) Automobile air bags use the decomposition of sodium azide as their source of gas for rapid inflation: 3 2 2NaN (s)®2Na (s) + 3N (g) . What mass (g) of 3 NaN is required to provide 40.0 L of 2 N at 25.0 °C and 763 torr? A) 1.64 B) 1.09 C) 160 D) 71.1  10) The reaction of 50 mL of 2 Cl gas with 50 mL of 4 CH gas via the equation: 2 4 3 Cl (g) + CH (g)®HCl (g) + CH Cl (g) will produce a total of __________ mL of products if pressure and temperature are kept constant. A) 100 B) 50 C) 200 D) 150 E) 250 -4- CHM 114: Exam #3 11) The density of 2 N O at 1.53 atm and 45.2 °C is __________ g/L. A) 18.2 B) 1.76 C) 0.388 D) 9.99 E) 2.58 12) A gas at a pressure of 325 torr exerts a force of __________ N on an area of 2 5.5 m . A)1.8×103 B) 59 C) 5 2.4×10 D) 0.018 E) 2.4 13) According to kinetic-molecular theory, in which of the following gases will the root-mean-square speed of the molecules be the highest at 200 °C? A) HCl B) 2 Cl C) 2 H O D) 6 SF E) None. The molecules of all gases have the same root-mean-square speed at any given temperature. 14) A real gas will behave most like an ideal gas under conditions of __________. A) high temperature and high pressure B) high temperature and low pressure C) low temperature and high pressure D) low temperature and low pressure E) STP 15) Elemental iodine (I2) is a solid at room temperature. What is the major attractive force that exists among different I2 molecules in the solid? A) London dispersion forces B) dipole-dipole rejections C) ionic-dipole interactions D) covalent-ionic interactions E) dipole-dipole attractions -5- CHM 114: Exam #3 16) The heat of fusion of water is 6.01 kJ/mol. The heat capacity of liquid water is 75.3 Jmol-1K-1. The conversion of 50.0 g of ice at 0.00 °C to liquid water at 22.0 °C requires __________ kJ of heat. A) 3.8×102 B) 21.3 C) 17.2 D) 0.469 E) Insufficient data are given. 17) Of the following substances, __________ has the highest boiling point. A) 2 H O B) 2 CO C) 4 CH D) Kr E) SF4 18) Which statements about viscosity are true? (i) Viscosity increases as temperature decreases. (ii) Viscosity increases as molecular weight increases. (iii) Viscosity increases as intermolecular forces increase. A) (i) only B) (ii) and (iii) C) (i) and (iii) D) none E) all 19) Based on molecular mass and dipole moment of the five compounds in the table below, which should have the highest boiling point? A) 3 2 3 CH CH CH B) 3 3 CH OCH C) 3 CH Cl D) 3 CH CHO E) 3 CH CN -6- CHM 114: Exam #3 20) On the phase diagram shown above, the coordinates of point __________ correspond to the critical temperature and pressure. A) A B) B C) C D) D E) E 21) The vapor pressure of pure ethanol at 60 °C is 0.459 atm. Raoult’s Law predicts that a solution prepared by dissolving 10.0 mmol naphthalene (nonvolatile) in 90.0 mmol ethanol will have a vapor pressure of _______ atm. A) 0.498 B) 0.413 C) 0.790 D) 0.367 E) 0.0918 Of the following, a 0.1 M aqueous solution of __________ will have the highest freezing point. A) NaCl B) Al(NO3)3 C) K2CrO4 D) Na2SO4 E) sucrose (a sugar) 23) What is the freezing point (°C) of a solution prepared by dissolving 11.3 g of Ca(NO3)2 (formula weight = 164 g/mol) in 115 g of water? The molal freezing point depression constant for water is 1.86 °C/m. A) -3.34 B) -1.11 C) 3.34 D) 1.11 E) 0.00 -7- CHM 114: Exam #3 24) The phase changes B  C and D  E are not associated with temperature increases because the heat energy is used up to __________. A) break intermolecular bonds B) break intramolecular bonds C) rearrange atoms within molecules D) increase the velocity of molecules E) increase the density of the sample 25) Ammonium nitrate (NH4NO3) dissolves readily in water even though the dissolution is endothermic by 26.4 kJ/mol. The solution process is spontaneous because __________. A) the vapor pressure of the water decreases upon addition of the solute B) the ammonium and the nitrate ion both contain nitrogen C) of the decrease in enthalpy upon addition of the solute D) of the increase in enthalpy upon dissolution of this strong electrolyte E) of the increase in disorder (entropy) upon dissolution of this strong electrolyte    -8- CHM 114: Exam #3

CHM114: Exam #2 CHM 114, S2015 Exam #2, Version C 16 March 2015 Instructor: O. Graudejus Points: 100 Print Name Sign Name Student I.D. # 1. You are responsible for the information on this page. Please read it carefully. 2. Code your name and 10 digit affiliate identification number on the separate scantron answer sheet. Use only a #2 pencil 3. If you enter your ASU ID incorrectly on the scantron, a 3 point penalty will be assessed. 4. Do all calculations on the exam pages. Do not make any unnecessary marks on the answer sheet. 5. This exam consists of 25 multiple choice questions worth 4 points each and a periodic table. Make sure you have them all. 6. Choose the best answer to each of the questions and answer it on the computer-graded answer sheet. Read all responses before making a selection. 7. Read the directions carefully for each problem. 8. Avoid even casual glances at other students’ exams. 9. Stop writing and hand in your scantron answer sheet and your test promptly when instructed. LATE EXAMS MAY HAVE POINTS DEDUCTED. 10. You will have 50 minutes to complete the exam. 11. If you leave early, please do so quietly. 12. Work the easiest problems first. 13. A periodic table is attached as the last page to this exam. 14. Answers will be posted online this afternoon. Potentially useful information: K = ºC + 273.15 RH=2.18·10-18 J R=8.314 J·K-1·mol-1 1Å=10-10 m c=3·108 m/s Ephoton=h·n=h·c/l h=6.626·10-34 Js Avogadro’s Number = 6.022 × 1023 particles/mole DH°rxn =  n DHf° (products) –  n DHf° (reactants) ) 1 1 ( 2 2 f i H n n DE = R − \ -2- CHM114: Exam #2 1) Which one of the following is an incorrect orbital notation? A) 2s B) 2p C) 3f D) 3d E) 4s 2) The energy of a photon that has a frequency of 8.21 1015s 1 − × is __________ J. A) 8.08 10 50 − × B) 1.99 10 25 − × C) 5.44 10 18 − × D) 1.24×1049 E) 1.26 10 19 − × 3) The ground state electron configuration of Ga is __________. A) 1s22s23s23p64s23d104p1 B) 1s22s22p63s23p64s24d104p1 C) 1s22s22p63s23p64s23d104p1 D) 1s22s22p63s23p64s23d104d1 E) [Ar]4s23d11 4) Of the bonds N–N, N=N, and NN, the N-N bond is __________. A) strongest/shortest B) weakest/longest C) strongest/longest D) weakest/shortest E) intermediate in both strength and length 5) Of the atoms below, __________ is the most electronegative. A) Br B) O C) Cl D) N E) F 6) Of the following, __________ cannot accommodate more than an octet of electrons. A) P B) O C) S D) Cl E) I -3- CHM 114: Exam #2 7) Which electron configuration represents a violation of Hund’s Rule? A) B) C) D) E) 8) A tin atom has 50 electrons. Electrons in the _____ subshell experience the highest effective nuclear charge. A) 1s B) 3p C) 3d D) 5s E) 5p 9) In ionic compounds, the lattice energy_____ as the magnitude of the ion charges _____ and the radii _____. A) increases, decrease, increase B) increases, increase, increase C) decreases, increase, increase D) increases, increase, decrease E) increases, decrease, decrease 10) Which of the following ionic compounds has the highest lattice energy? A) LiF B) MgO C) CsF D) CsI E) LiI -4- CHM 114: Exam #2 11) For which one of the following reactions is the value of H°rxn equal to Hf° for the product? A) 2 C (s, graphite) + 2 H2 (g)  C2H4 (g) B) N2 (g) + O2 (g)  2 NO (g) C) 2 H2 (g) + O2 (g)  2 H2O (l) D) 2 H2 (g) + O2 (g)  2 H2O (g) E) all of the above 12) Given the data in the table below, H rxn D ° for the reaction 3 2 3 PCl (g) + 3HCl(g)®3Cl (g) + PH (g) is __________ kJ. A) -570.37 B) -385.77 C) 570.37 D) 385.77 E) The f DH° of 2 Cl (g) is needed for the calculation. 13) Given the following reactions (1) 2 2 2NO® N +O H = -180 kJ (2) 2 2 2NO+O ®2NO H = -112 kJ the enthalpy of the reaction of nitrogen with oxygen to produce nitrogen dioxide 2 2 2 N + 2O ®2NO is __________ kJ. A) 68 B) -68 C) -292 D) 292 E) -146 14) Of the following transitions in the Bohr hydrogen atom, the __________ transition results in the absorption of the lowest-energy photon. A) n = 1  n = 6 B) n = 6  n = 1 C) n = 6  n = 5 D) n = 3  n = 6 E) n = 1  n = 4 -5- CHM 114: Exam #2 15) Which equation correctly represents the electron affinity of calcium? A) Ca (g)  Ca+ (g) + e- B) Ca (g)  Ca- (g) + e- C) Ca (g) + e-  Ca- (g) D) Ca- (g)  Ca (g) + e- E) Ca+ (g) + e-  Ca (g) 16) Which of the following does not have eight valence electrons? A) Ca+ B) Rb+ C) Xe D) Br− E) All of the above have eight valence electrons. 17) The specific heat of liquid bromine is 0.226 J/g · K. The molar heat capacity (in J/mol-K) of liquid bromine is __________. A) 707 B) 36.1 C) 18.1 D) 9.05 E) 0.226 18) Given the electronegativities below, which covalent single bond is least polar? Element: H C N O F Electronegativity: 2.1 2.5 3.0 3.5 4.0 A) C-H B) C-F C) O-H D) O-C E) F-H 19) The bond length in an HCl molecule is 1.27 Å and the measured dipole moment is 1.08 D. What is the magnitude (in units of e) of the negative charge on Cl in HCl? (1 debye = 3.34 10 30 coulomb-meters − × ; e=1.6 10 19 coulombs − × ) A) 1.6 10 19 − × B) 0.057 C) 0.18 D) 1 E) 0.22 -6- CHM 114: Exam #2 20) The F-B-F bond angle in the BF3 molecule is approximately __________. A) 90° B) 109.5° C) 120° D) 180° E) 60° 21) Which isoelectronic series is correctly arranged in order of increasing radius? A) K+ < Ca2+ < Ar < Cl- B) Cl- < Ar < K+ < Ca2+ C) Ca2+ < Ar < K+ < Cl- D) Ca2+ < K+ < Ar < Cl- E) Ca2+ < K+ < Cl- < Ar 22) What is the electron configuration for the Fe2+ ion? A) [Ar]4s03d6 B) [Ar]4s23d4 C) [Ar]4s03d8 D) [Ar]4s23d8 E) [Ar]4s63d2 23) The formal charge on carbon in the Lewis structure of the NCS - ion is __________: A) -1 B) +1 C) +2 D) 0 E) +3 -7- CHM 114: Exam #2 24) Using the table of bond dissociation energies, the H for the following gas-phase reaction is __________ kJ. A) 291 B) 2017 C) -57 D) -356 E) -291 25) According to VSEPR theory, if there are six electron domains in the valence shell of an atom, they will be arranged in a(n) __________ geometry. A) octahedral B) linear C) tetrahedral D) trigonal planar E) trigonal bipyramidal -8- CHM 114: Exam #2

CHM114: Exam #2 CHM 114, S2015 Exam #2, Version C 16 March 2015 Instructor: O. Graudejus Points: 100 Print Name Sign Name Student I.D. # 1. You are responsible for the information on this page. Please read it carefully. 2. Code your name and 10 digit affiliate identification number on the separate scantron answer sheet. Use only a #2 pencil 3. If you enter your ASU ID incorrectly on the scantron, a 3 point penalty will be assessed. 4. Do all calculations on the exam pages. Do not make any unnecessary marks on the answer sheet. 5. This exam consists of 25 multiple choice questions worth 4 points each and a periodic table. Make sure you have them all. 6. Choose the best answer to each of the questions and answer it on the computer-graded answer sheet. Read all responses before making a selection. 7. Read the directions carefully for each problem. 8. Avoid even casual glances at other students’ exams. 9. Stop writing and hand in your scantron answer sheet and your test promptly when instructed. LATE EXAMS MAY HAVE POINTS DEDUCTED. 10. You will have 50 minutes to complete the exam. 11. If you leave early, please do so quietly. 12. Work the easiest problems first. 13. A periodic table is attached as the last page to this exam. 14. Answers will be posted online this afternoon. Potentially useful information: K = ºC + 273.15 RH=2.18·10-18 J R=8.314 J·K-1·mol-1 1Å=10-10 m c=3·108 m/s Ephoton=h·n=h·c/l h=6.626·10-34 Js Avogadro’s Number = 6.022 × 1023 particles/mole DH°rxn =  n DHf° (products) –  n DHf° (reactants) ) 1 1 ( 2 2 f i H n n DE = R − \ -2- CHM114: Exam #2 1) Which one of the following is an incorrect orbital notation? A) 2s B) 2p C) 3f D) 3d E) 4s 2) The energy of a photon that has a frequency of 8.21 1015s 1 − × is __________ J. A) 8.08 10 50 − × B) 1.99 10 25 − × C) 5.44 10 18 − × D) 1.24×1049 E) 1.26 10 19 − × 3) The ground state electron configuration of Ga is __________. A) 1s22s23s23p64s23d104p1 B) 1s22s22p63s23p64s24d104p1 C) 1s22s22p63s23p64s23d104p1 D) 1s22s22p63s23p64s23d104d1 E) [Ar]4s23d11 4) Of the bonds N–N, N=N, and NN, the N-N bond is __________. A) strongest/shortest B) weakest/longest C) strongest/longest D) weakest/shortest E) intermediate in both strength and length 5) Of the atoms below, __________ is the most electronegative. A) Br B) O C) Cl D) N E) F 6) Of the following, __________ cannot accommodate more than an octet of electrons. A) P B) O C) S D) Cl E) I -3- CHM 114: Exam #2 7) Which electron configuration represents a violation of Hund’s Rule? A) B) C) D) E) 8) A tin atom has 50 electrons. Electrons in the _____ subshell experience the highest effective nuclear charge. A) 1s B) 3p C) 3d D) 5s E) 5p 9) In ionic compounds, the lattice energy_____ as the magnitude of the ion charges _____ and the radii _____. A) increases, decrease, increase B) increases, increase, increase C) decreases, increase, increase D) increases, increase, decrease E) increases, decrease, decrease 10) Which of the following ionic compounds has the highest lattice energy? A) LiF B) MgO C) CsF D) CsI E) LiI -4- CHM 114: Exam #2 11) For which one of the following reactions is the value of H°rxn equal to Hf° for the product? A) 2 C (s, graphite) + 2 H2 (g)  C2H4 (g) B) N2 (g) + O2 (g)  2 NO (g) C) 2 H2 (g) + O2 (g)  2 H2O (l) D) 2 H2 (g) + O2 (g)  2 H2O (g) E) all of the above 12) Given the data in the table below, H rxn D ° for the reaction 3 2 3 PCl (g) + 3HCl(g)®3Cl (g) + PH (g) is __________ kJ. A) -570.37 B) -385.77 C) 570.37 D) 385.77 E) The f DH° of 2 Cl (g) is needed for the calculation. 13) Given the following reactions (1) 2 2 2NO® N +O H = -180 kJ (2) 2 2 2NO+O ®2NO H = -112 kJ the enthalpy of the reaction of nitrogen with oxygen to produce nitrogen dioxide 2 2 2 N + 2O ®2NO is __________ kJ. A) 68 B) -68 C) -292 D) 292 E) -146 14) Of the following transitions in the Bohr hydrogen atom, the __________ transition results in the absorption of the lowest-energy photon. A) n = 1  n = 6 B) n = 6  n = 1 C) n = 6  n = 5 D) n = 3  n = 6 E) n = 1  n = 4 -5- CHM 114: Exam #2 15) Which equation correctly represents the electron affinity of calcium? A) Ca (g)  Ca+ (g) + e- B) Ca (g)  Ca- (g) + e- C) Ca (g) + e-  Ca- (g) D) Ca- (g)  Ca (g) + e- E) Ca+ (g) + e-  Ca (g) 16) Which of the following does not have eight valence electrons? A) Ca+ B) Rb+ C) Xe D) Br− E) All of the above have eight valence electrons. 17) The specific heat of liquid bromine is 0.226 J/g · K. The molar heat capacity (in J/mol-K) of liquid bromine is __________. A) 707 B) 36.1 C) 18.1 D) 9.05 E) 0.226 18) Given the electronegativities below, which covalent single bond is least polar? Element: H C N O F Electronegativity: 2.1 2.5 3.0 3.5 4.0 A) C-H B) C-F C) O-H D) O-C E) F-H 19) The bond length in an HCl molecule is 1.27 Å and the measured dipole moment is 1.08 D. What is the magnitude (in units of e) of the negative charge on Cl in HCl? (1 debye = 3.34 10 30 coulomb-meters − × ; e=1.6 10 19 coulombs − × ) A) 1.6 10 19 − × B) 0.057 C) 0.18 D) 1 E) 0.22 -6- CHM 114: Exam #2 20) The F-B-F bond angle in the BF3 molecule is approximately __________. A) 90° B) 109.5° C) 120° D) 180° E) 60° 21) Which isoelectronic series is correctly arranged in order of increasing radius? A) K+ < Ca2+ < Ar < Cl- B) Cl- < Ar < K+ < Ca2+ C) Ca2+ < Ar < K+ < Cl- D) Ca2+ < K+ < Ar < Cl- E) Ca2+ < K+ < Cl- < Ar 22) What is the electron configuration for the Fe2+ ion? A) [Ar]4s03d6 B) [Ar]4s23d4 C) [Ar]4s03d8 D) [Ar]4s23d8 E) [Ar]4s63d2 23) The formal charge on carbon in the Lewis structure of the NCS - ion is __________: A) -1 B) +1 C) +2 D) 0 E) +3 -7- CHM 114: Exam #2 24) Using the table of bond dissociation energies, the H for the following gas-phase reaction is __________ kJ. A) 291 B) 2017 C) -57 D) -356 E) -291 25) According to VSEPR theory, if there are six electron domains in the valence shell of an atom, they will be arranged in a(n) __________ geometry. A) octahedral B) linear C) tetrahedral D) trigonal planar E) trigonal bipyramidal -8- CHM 114: Exam #2

What is a correct method for determining how many moles of calcium oxide are produced in the reaction of 10.0 g calcium with excess oxygen? Question 4. 4. What is a correct method for determining how many moles of calcium oxide are produced in the reaction of 10.0 g calcium with excess oxygen? 2 Ca(s) + O2(g)  2 CaO(s) (Points : 5) 10 g Ca x [1 mol/40.07 g] x 56.07 g/mol 10 g Ca x [2 mole Ca / 2 mole CaO] x 40.07 g/mol 10 g Ca x [2 mole CaO/ 2mole Ca] x [56.07 g/mol] 40.07 g/mol x 10 g/mol x [2 mole CaO/2 mole Ca] 10 g Ca x 40.07 g/mol x [56.07 g/mol]

What is a correct method for determining how many moles of calcium oxide are produced in the reaction of 10.0 g calcium with excess oxygen? Question 4. 4. What is a correct method for determining how many moles of calcium oxide are produced in the reaction of 10.0 g calcium with excess oxygen? 2 Ca(s) + O2(g)  2 CaO(s) (Points : 5) 10 g Ca x [1 mol/40.07 g] x 56.07 g/mol 10 g Ca x [2 mole Ca / 2 mole CaO] x 40.07 g/mol 10 g Ca x [2 mole CaO/ 2mole Ca] x [56.07 g/mol] 40.07 g/mol x 10 g/mol x [2 mole CaO/2 mole Ca] 10 g Ca x 40.07 g/mol x [56.07 g/mol]

The reaction of 50 mL of 2 Cl gas with 50 mL of 4 CH gas via the equation: 2 4 3 Cl (g) + CH (g)®HCl (g) + CH Cl (g) will produce a total of __________ mL of products if pressure and temperature are kept constant. A) 100 B) 50 C) 200 D) 150 E) 250

The reaction of 50 mL of 2 Cl gas with 50 mL of 4 CH gas via the equation: 2 4 3 Cl (g) + CH (g)®HCl (g) + CH Cl (g) will produce a total of __________ mL of products if pressure and temperature are kept constant. A) 100 B) 50 C) 200 D) 150 E) 250

A) 100 The reaction of 50 mL of 2 Cl … Read More...
The combustion of propane 3 8 (C H ) in the presence of excess oxygen yields 2 CO and 2 H O : 3 8 2 2 2 C H (g) + 5O (g)®3CO (g) + 4H O (g) When 2.5 mol of 2 O are consumed in their reaction, __________ mol of 2 CO are produced. A) 1.5 B) 3.0 C) 5.0 D) 6.0 E) 2.5

The combustion of propane 3 8 (C H ) in the presence of excess oxygen yields 2 CO and 2 H O : 3 8 2 2 2 C H (g) + 5O (g)®3CO (g) + 4H O (g) When 2.5 mol of 2 O are consumed in their reaction, __________ mol of 2 CO are produced. A) 1.5 B) 3.0 C) 5.0 D) 6.0 E) 2.5

A) 1.5
Thermite is a mixture of iron(iii) oxide and aluminum pwders that as once used to weld railroad tracks. It undergoes a spectacular reaction to yield solid aluminum oxide and molten iron. How many moles of iron(iii) oxide are needed to form 3.60*10^3 mol of iron?

Thermite is a mixture of iron(iii) oxide and aluminum pwders that as once used to weld railroad tracks. It undergoes a spectacular reaction to yield solid aluminum oxide and molten iron. How many moles of iron(iii) oxide are needed to form 3.60*10^3 mol of iron?

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