Chem 124 Exam 1 Spring 2016 Version 1 Name

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1 Chem 124 Exam 1 Spring 2016 Version 1 Name TOTAL POINTS MULTIPLE CHOICE 1.4 POINTS EACH 1) A molecule containing a central atom with sp 3 hybridization has a(n) electron geometry. A) linear B) tetrahedral C) octahedral D) bent E) trigonal bipyramidal 1) 2) What is the bond order in He 2 molecule? 2) A) 0 B) 2 C) 1 D) 1/2 3) Which will make the molecule AB 2 bent in shape? 3) A) the nonbonding electrons B) the bonding electrons C) the lone pairs on atom A D) the bond pairs 4) Identify the characteristics of a liquid. 4) A) definite shape and volume B) indefinite shape and volume C) indefinite shape, but definite volume D) none of the above E) all of the above 5) Give the change in condition to go from a liquid to a gas. 5) A) Increase heat or increase pressure. B) Increase heat or reduce pressure. C) Cool or reduce pressure. D) Cool or increase pressure. E) None of the above 6) Which of the following statements is true? 6) A) Energy is given off when the attraction between two molecules is broken. B) Intermolecular forces are generally stronger than bonding forces. C) Until a certain point, the potential energy of molecules decrease as they get closer to one another.

2 D) Increasing the pressure on a solid usually causes it to become a liquid. E) None of the above are true. 7) What is the strongest type of intermolecular force present in CHF 3? 7) A) hydrogen bonding B) ion-dipole C) dipole-dipole D) dispersion E) None of the above 8) What type of intermolecular force causes the dissolution of NaCl in water? A) ion-dipole force B) dispersion forces C) hydrogen bonding D) dipole-dipole forces E) None of the above 8) 9) Which of the following statements is true? 9) A) Intermolecular forces hold the atoms in molecules together. B) Dispersion forces are generally stronger than dipole-dipole forces. C) Vapor pressure increases with temperature. D) Hydrogen bonds are stronger than covalent bonds. E) None of the above are true. 10) Define sublimation. 10) A) The phase transition from gas to liquid. B) The phase transition from gas to solid. C) The phase transition from liquid to gas. D) The phase transition from solid to gas. E) The phase transition from liquid to solid. 11) Assign the appropriate labels to the phase diagram shown below. 11) A) A = gas, B = liquid, C = solid, D = critical point

3 B) A = solid, B = gas, C = liquid, D = supercritical fluid C) A = liquid, B = solid, C = gas, D = critical point D) A = liquid, B = gas, C = solid, D = triple point E) A = gas, B = solid, C = liquid, D = triple point 12) Why is water an extraordinary substance? 12) A) Water has strong hydrogen bonding. B) Water is the main solvent within living organisms. C) Water has a low molar mass, yet it is a liquid at room temperature. D) Water has an exceptionally high specific heat capacity. E) All of the above 13) What is the strongest type of intermolecular force present in Cl 2? 13) A) hydrogen bonding B) dipole-dipole C) dispersion D) ion-dipole E) none of the above 14) In the phase diagram, what is the triple point? 14) A) 535 C B) 184 C C) 128 C D) 114 C 15) What is the strongest type of intermolecular force present in NH 2 CH 3? A) dipole-dipole B) hydrogen bonding C) dispersion D) ion-dipole 15)

4 E) None of the above 16) Which substance below has the strongest intermolecular forces? 16) A) BY 2, H vap = 26.7 kj/mol B) EY 3, H vap = 21.5 kj/mol C) A 2 X, H vap = 39.6 kj/mol D) DX 2, H vap = 23.3 kj/mol E) C 3 X 2, H vap = 36.4 kj/mol 17) Choose the statement below that is true. 17) A) A solution will form between two substances if the solute-solute interactions are strong enough to overcome the solvent-solvent interactions. B) A solution will form between two substances only if the solvent-solvent interactions are weak enough to overcome the solute-solvent interactions. C) A solution will form between two substances if the solute-solvent interactions are of comparable strength to the solute-solute and solvent-solvent interactions. D) A solution will form between two substances if the solute-solvent interactions are small enough to be overcome by the solute-solute and solvent-solvent interactions. E) None of the above are true. 18) Which of the following compounds will be most soluble in pentane (C 5 H 12 )? A) pentanol (CH 3 CH 2 CH 2 CH 2 CH 2 OH) B) ethyl methyl ketone (CH 3 CH 2 COCH 3 ) C) benzene (C 6 H 6 ) D) acetic acid (CH 3 CO 2 H) E) None of these compounds should be soluble in pentane. 19) Which of the following compounds is most soluble in hexane (CH 3 CH 2 CH 2 CH 2 CH 2 CH 2 CH 3 )? A) 1-butanol B) ethanol C) 1-propanol D) methanol E) 1-pentanol 20) Give the intermolecular force that is responsible for the solubility of ethanol in water. A) dipole-dipole forces B) ionic forces C) ion-dipole forces D) dispersion forces E) hydrogen bonding 18) 19) 20)

5 21) Which of the following ions should have the most exothermic H hydration? A) Na + B) Sr 2+ C) Mg 2+ D) Ca 2+ E) Al 3+ 21) 22) Which of the following statements is true? 22) A) The solubility of a solid is highly dependent on temperature. B) The solubility of a solid is not dependent on either temperature or pressure. C) The solubility of a solid is highly dependent on both pressure and temperature. D) The solubility of a solid is highly dependent on pressure. E) None of the above. 23) Which of the following statements is true? 23) A) The solubility of a gas in water decreases with decreasing pressure. B) The solubility of a gas in water increases with increasing pressure. C) The solubility of a gas in water decreases with increasing pressure. D) The solubility of a gas in water increases with decreasing pressure. E) None of the above statements are true. 24) Give the term for amount of solute in mole per mass of solvent in kg. 24) A) molality B) mole percent C) mass percent D) mole fraction E) molarity 25) Which of the following concentration units are temperature dependent? A) molality B) mole fraction C) molarity D) mass percent E) none of the above 25) 26) Identify the colligative property. 26) A) boiling point elevation B) vapor pressure lowering C) freezing point depression D) osmotic pressure E) all of the above

6 27) Which interaction(s) determine whether a solution will form? 27) A) solute-solute B) solvent-solute C) solvent-solvent D) all of the above 28) A solution contains 45g of KNO3 per g of water at 25 C. The solubility of KNO3 at this temperature is 37.5 g per g of water. The solution is. A) unsaturated B) saturated C) supersaturated D) none of the above 29) Choose the aqueous solution below with the lowest freezing point. These are all solutions of nonvolatile solutes and you should assume ideal van't Hoff factors where applicable. A) m LiCl B) m (NH 4 ) 3 PO 4 28) 29) C) m KNO 2 D) m NaBrO 4 E) m KCN 30) Which aqueous solution has the lowest boiling point? 30) A) 0.10 m AlCl 3 B) 0.10 m BaCl 2 C) 0.10 m NaCl D) 0.10 m C 6 H 12 O 6 31) Which is expected to have the largest dispersion forces? 31) A) C 3 H 8 B) Be Cl 2 C) C 12 H 26 D) F 2 32) Choose the pair of substances that are most likely to form a homogeneous solution. A) NaCl and Hg B) NH 3 and CH 3 OH 32) C) Br 2 and PF 3 D) C 3 H 8 and C 2 H 5 OH E) LiF and C 6 H 14

7 33) Choose the substance with the highest viscosity. 33) A) CF 4 B) (CH 3 CH 2 ) 2 CO C) C 2 H 4 Cl 2 D) C 6 H 14 E) HOCH 2 CH 2 CH 2 CH 2 OH 34) Calculate the molality of a solution formed by dissolving 27.8 g of LiI in ml of water. A) m B) m C) m D) m E) m 35) What mass (in g) of NH 3 must be dissolved in 475 g of methanol to make a m solution? A) 4.94 g B) 1.90 g C) 2.02 g D) 8.42 g E) 1.19 g 34) 35) 36) Choose the compound that exhibits hydrogen bonding as its strongest 36) intermolecular force. A) SCl 2 B) CH 3 OH C) CH 2 F 2 D) C 2 H 6 E) None of the above compounds exhibit hydrogen bonding. 37) Place the following substances in order of increasing boiling point. 37) CH 3 CH 2 OH Ar CH 3 OCH 3 A) CH 3 CH 2 OH < CH 3 OCH 3 < Ar B) CH 3 CH 2 OH < Ar < CH 3 OCH 3 C) CH 3 OCH 3 < Ar < CH 3 CH 2 OH D) Ar < CH 3 OCH 3 < CH 3 CH 2 OH E) Ar < CH 3 CH 2 OH < CH 3 OCH 3 38) Given the following rate law, how does the rate of reaction change if the concentration of Y is doubled? 38)

8 Rate = k [X][Y] 2 A) The rate of reaction will decrease by a factor of 2. B) The rate of reaction will increase by a factor of 4. C) The rate of reaction will increase by a factor of 5. D) The rate of reaction will increase by a factor of 2. E) The rate of reaction will remain unchanged. 39) Which of the following substances would you predict to have the highest H vap? A) HOCH 2 CH 2 OH B) CH 3 CH 2 OH 39) C) CH 3 CH 2 CH 2 CH 3 D) HCl E) CH 3 Cl 40) Given the following balanced equation, determine the rate of reaction with respect to [SO 2 ]. 40) 2 SO 2 (g) + O 2 (g) 2 SO 3 (g) A) Rate = - B) Rate = + C) Rate = - D) Rate = + E) It is not possible to determine without more information. 41) What are the units of k in the following rate law? 41) Rate = k[x][y] 1/2 A) M -1/2 s -1 B) M -1 s -1/2 C) M/s D) M 1/2 s -1 E) M -1 s -1 42) What is the overall order of the following reaction, given the rate law? 42) 2 X + 3 Y 2 Z Rate = k[x] 1 [Y] 2 A) zeroth order B) 3rd order

9 C) 5th order D) 2nd order E) 1st order 43) Which is expected to have the largest dispersion forces? 43) A) C S 2 B) C 10 H 22 C) C H 4 D) O 2 44) Determine the rate law for the following reaction using the data provided. 44) NO 2 (g) + O 3 (g) NO 3 (g) + O 2 (g) [NO 2 ] i (M) [O 3 ] i (M) Initial Rate (M -1 s -1 ) A) Rate = k[no 2 ][O 3 ] 2 B) Rate = k [NO 2 ] 2.5 [O 3 ] C) Rate = k [NO 2 ][O 3 ] 2.5 D) Rate = k [NO 2 ] 2 [O 3 ] E) Rate = k [NO 2 ][O 3 ] 45) Given the following balanced equation, determine the rate of reaction with respect to [O 2 ]. If the rate of formation of O 2 is M/s, what is the rate of the loss of O 3? 45) 2 O 3 (g) 3 O 2 (g) A) 2.08 M/s B) 4.16 M/s C) 1.04 M/s D) M/s E) M/s 46) Calculate the mole fraction of total ions in an aqueous solution prepared by dissolving moles of MgCl 2 in g of water. A) B) C) D) )

10 E) ) A solution is prepared by dissolving 98.6 g of NaCl in enough water to form 875 ml of solution. Calculate the mass % of the solution if the density of the solution is 1.06 g/ml. A) 9.4% B) 10.6% C) 11.9% D) 11.3% E) 12.7% 48) How much energy is required to vaporize 158 g of butane (C 4 H 10 ) at its boiling point, if its H vap is 24.3 kj/mol? A) 38.4 kj B) 89.4 kj C) 15.1 kj D) 66.1 kj E) 11.2 kj 49) Choose the compound below that contains at least one polar covalent bond, but is nonpolar. A) ICl 3 47) 48) 49) B) SeBr 4 C) CF 4 D) HCN E) Both B and C are nonpolar and contain a polar covalent bond. 50) Which of the following statements is true? 50) A) The total number of molecular orbitals formed doesn't always equal the number of atomic orbitals in the set. B) When two atomic orbitals come together to form two molecular orbitals, one molecular orbital will be lower in energy than the two separate atomic orbitals, and one molecular orbital will be higher in energy than the separate atomic orbitals. C) A bond order of 0 represents a stable chemical bond. D) Electrons placed in antibonding orbitals stabilize the ion/molecule. E) All of the above are true. 51) What is the mole fraction of ethanol in a solution made by dissolving 29.2 g of ethanol, C 2 H 5 OH, in 53.6 g of water? A) B) C) D) ) 52) A solution is 2.25% by weight NaHCO 3. How many grams of 52)

11 NaHCO 3 are in g of solution? A) 3.38 g B) 225 g C) 1.50 g D) 66.7 g 53) At a given temperature the vapor pressures of benzene and toluene 53) are 183 mm Hg and 59.2 mm Hg, respectively. Calculate the total vapor pressure over a solution of benzene and toluene with X benzene = A) 121 mm Hg B) 106 mm Hg C) 242 mm Hg D) 131 mm Hg 54) Which of the following solutions will have the lowest freezing point? 54) A) m K Br B) m BaCl 2 C) m CH 3 CH 2 OH D) m Na 2 CO 3 55) What is the expected freezing point of a 0.50 m solution of Li 2 SO 4 in water? K f for water is 1.86 C/m. A) C B) -2.8 C C) -6.5 C D) -1.9 C 56) Consider the molecule below. Determine the hybridization at each of the 2 labeled carbons. 55) 56) A) C1 = sp, C2 = sp 2 B) C1 = sp 2, C2 = sp 3 C) C1 = sp 3, C2 = sp 3 d D) C1 = sp 2, C2 = sp 3 d E) C1 = sp 3 d, C2 = sp 3 d 2 57) Place the following substances in order of increasing vapor pressure at a given temperature. 57)

12 NF 3 NH 3 BCl 3 A) NH 3 < BCl 3 < NF 3 B) NH 3 < NF 3 < BCl 3 C) BCl 3 < NF 3 < NH 3 D) NF 3 < NH 3 < BCl 3 E) BCl 3 < NH 3 < NF 3 58) The osmotic pressure of a solution formed by dissolving 25.0 mg of aspirin in L of water at 25 C is atm. A) 2.45 B) 13.6 C) D) 1.38 E) ) 59) Which of the following compounds has the highest boiling point? 59) A) N H 3 B) H 2 S C) H 2 O D) H Cl 60) List the number of sigma bonds and pi bonds in a triple bond. 60) A) 2 sigma, 1 pi B) 2 sigma, 2 pi C) 1 sigma, 1 pi D) 1 sigma, 2 pi NAME SHORT ANSWER QUESTIONS - 4 POINTS EACH - TOTAL 32 POINTS 61) Is it possible for a molecule to be nonpolar even though it contains polar bonds? Explain your answer and give an example. 61) Yes - The polarity of a molecule depends on its molecular geometry. In class we used CCl4 as an example of a solvent with 4 polar bonds but because it was completely symmetrical (tetrahedral) the molecule was not polar - there was no net dipole 62) Rank the following forces in order of INCREASING strength: ion-dipole, dispersion, hydrogen bonding, dipole-dipole, ion-ion 62) dispersion, dipole-dipole, hydrogen bonding, ion dipole, ion-ion (its ok if dipole dipole and hydrogen bonding are switched - although hydrogen bonding is generally greater than dipole-dipole there are

13 some weaker H bonds and some very strong dipole-dipole bonds) 63) Explain why the bolling point of water is so much higher than other compounds of similar molecular weight. 63) This is due to the intermolecular hydrogen bonds 64) Of the following molecules which would have the highest surface tension? Explain your answer BRIEFLY by discussing the appropriate forces. CH 3 CH 2 CH 3, CH 3 CH 2 F, CH 2 F 2, CH 3 CH 2 OH, HOCH 2 CH 2 OH 64) HOCH 2 CH 2 OH - this molecule would have the greatest number and strength of intermolecular forces due to the hydrogen bonding of the OH groups. The higher the intermolecular forces of the liquid the higher the surface tension. 65) Why does the temperature of a substance stay constant during a phase change such as vaporization? 65) The energy added to the substance is not used to raise the kinetic energy of the substance. Instead it is "used up" in breaking the intermolecular attractions between particles to take them from a liquid (with intermolecular attractions) to a gas (with no intermolecular attractions). 66) What is the weight percent of vitamin C in a solution made by dissolving 6.50 g of vitamin C, C 6 H 8 O 6, in 55.0 g of water? (SHOW YOUR WORK WITH UNITS FOR CREDIT) 66) 6.50 g g = 61.5 g 6.50g/61.5g * 100 = 10.5% 67) The heat of vaporization of water at 100 C is kj/mol. Calculate the quantity of heat that is absorbed/released when 9.00 g of steam condenses to liquid water at 100 C. (SHOW YOUR WORK WITH UNITS FOR CREDIT) 67) 9.00g * 1mol/18 g = 0.5 mol kj/mol * 0.5 mol = kj The heat is absorbed so the sign is positive 68) Calculate the rate constant for the reaction between phenolphthalein and the OH - ion if the instantaneous rate of reaction is 2.5 x 10-5 mole per liter per 68)

14 second when the concentration of phenolphthalein is M. The reactionis first order in phenolpthalein. (SHOW YOUR WORK WITH UNITS FOR CREDIT) rate = k[pt] this expression can be written because the problem says the reaction is first order in phenolpthalein (pt) rate = 2.5 x 10-5 mole/l second = k* mol/l k = s -1 Multiple(Choice(Key(/(Version(1 1)B 2)A 3)C 4)C 5)B 6)C 7)C 8)A 9)C 10)D 11)E 12)E 13)C 14)D 15)B 16)C 17)C 18)C 19)E 20)E 21)E 22)A 23)B 24)A 25)C 26)E 27)D 28)C 29)B 30)D 31)C 32)B 33)E 34)D 35)C

15 36)B 37)D 38)B 39)A 40)C 41)A 42)B 43)B 44)E 45)D 46)D 47)B 48)D 49)C 50)B 51)D 52)A 53)D 54)B 55)B 56)B 57)B 58)C 59)C 60)D (

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