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Chemisty Ch. 11

Quiz yourself by thinking what should be in each of the black spaces below before clicking on it to display the answer.
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Question
Answer
1) Identify the characteristics of a liquid.   show
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show A) gas  
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show C) solid  
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4) Give the change in condition to go from a liquid to a gas.   show
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show C) dipole-dipole forces  
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6) Which of the following statements is TRUE?   show
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show C) dispersion  
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show D) dipole-dipole  
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show C) hydrogen bonding  
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show C) ion-dipole force  
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show A) Cl2  
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12) Choose the molecule or compound that exhibits dipole-dipole forces as its strongest intermolecular force.   show
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13) Choose the compound that exhibits hydrogen bonding as its strongest intermolecular force.   show
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show D) F2 < CO2 < NH2CH3  
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show E) CH4 < CH3CH3 < CH3CH2CH3  
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show A) HF > CO2 > O2  
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show B) I > III > II  
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18) Which has the smallest dipole-dipole forces?   show
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19) Which is expected to have the largest dispersion forces?   show
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show E) CO2  
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show D) NH3  
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show A) (CH3)3N  
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show E) NH3 and CH3OH  
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show A) C6H14 and C10H20  
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25) Choose the pair of substances that are most likely to form a homogeneous solution.   show
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show A) Dispersion, hydrogen bonding and dipole-dipole forces are present.  
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show B) HI  
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28) The normal boiling point for H2Se is higher than the normal boiling point for H2S . This can be explained by   show
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29) In a liquid, the energy required to increase the surface of the area by a unit amount is called __________.   show
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show A) HOCH2CH2OH  
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show B) CH3CH2CH2CH3  
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32) Choose the substance with the highest viscosity.   show
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33) Choose the substance with the lowest viscosity.   show
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34) Choose the substance with the highest viscosity.   show
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show C) corn syrup  
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36) Identify the term used to describe the ability of a liquid to flow against gravity up a narrow tube.   show
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show A) Vapor pressure increases with temperature.  
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show D) Molecules with hydrogen bonding are more volatile than compounds with dipole-dipole forces.  
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show A) A2X, ΔHvap= 39.6 kJ/mol  
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show A) A liquid becomes a gas.  
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show D) critical temperature  
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42) Choose the substance with the highest vapor pressure at a given temperature.   show
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43) Choose the substance with the lowest vapor pressure at a given temperature.   show
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show E) Ne < O2 < Cl2  
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show A) Ar < CH3OCH3 < CH3CH2OH  
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46) Choose the substance with the highest boiling point.   show
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47) Choose the substance with the lowest boiling point.   show
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48) Which of the following substances would you predict to have the highest ΔHvap?   show
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show D) Br2  
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50) How much energy is required to vaporize 48.7 g of dichloromethane (CH2Cl2) at its boiling point, if its ΔHvap is 31.6 kJ/mol?   show
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51) How much energy is required to vaporize 98.6 g of ethanol (C2H5OH) at its boiling point, if its ΔHvap is 40.5 kJ/mol?   show
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52) How much energy is required to vaporize 158 g of butane (C4H10) at its boiling point, if its ΔHvap is 24.3 kJ/mol?   show
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53) Based on the figure above, the boiling point of diethyl ether under an external pressure of 1.32 atm is __________°C.   show
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54) Based on the figure above, the boiling point of ethyl alcohol under an external pressure of 0.0724 atm is __________°C.   show
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show A) 70  
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56) Place the following substances in order of increasing vapor pressure at a given temperature. SF6 SiH4 SF4   show
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57) Place the following substances in order of decreasing vapor pressure at a given temperature. PF5 BrF3 CF4   show
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show A) NH3 < NF3 < BCl3  
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59) Place the following substances in order of decreasing vapor pressure at a given temperature. BeF2 CH3OH OF2   show
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60) Place the following substances in order of decreasing boiling point. H2O N2 CO   show
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show D) O2 > N2 > H2  
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show D) Ar > He > H2  
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show A) H2O  
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show C) 24 kJ/mol  
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65) Determine the normal boiling point of a substance whose vapor pressure is 55.1 mm Hg at 35°C and has a ΔHvap of 32 .1 kJ/mol.   show
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66) Determine the vapor pressure (in mm Hg) of a substance at 29°C, whose normal boiling point is 76°C and has a ΔHvap of 38.7 kJ/mol.   show
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67) Determine the vapor pressure (in torr) of a substance at 36°C, whose normal boiling point is 84°C and has a ΔHvap of 22.1 kJ/mol.   show
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68) Define deposition.   show
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show A) the phase transition from solid to gas  
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show E) the phase transition from liquid to solid  
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show C) sublimes  
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show A) 0°C  
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show A) 0°C  
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74) The boiling point of water is __________.   show
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75) The heat of vaporization of water at 100°C is 40.66 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
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76) Calculate the total quantity of heat required to convert 25.0 g of liquid CCl4(l) from 35.0°C to gaseous CCl4 at 76.8°C (the normal boiling point for CCl4). The specific heat of CCl4(l) is 0.857 J/(g · °C), its heat of fusion is 3.27 kJ/mol, and its   show
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show C) 13.16  
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show D) 7.21  
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79) The fluorocarbon C2Cl3F3 has a normal boiling point of 47.6°C. The specific heats of C2Cl3F3(l) and C2Cl3F3 (g) are 0.91 J/gK and 0.67 J/gK, respectively. The heat of vaporization of the compound is 27.49 kJ/mol. The heat required to convert 50.0 g of   show
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show C) 6.91 kJ  
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81) Ethyl chloride, C2H5Cl, is used as a local anesthetic. It works by cooling tissue as it vaporizes; its heat of vaporization is 26.4 kJ/mol. How much heat could be removed by 20.0 g of ethyl chloride?   show
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enthalpy of vaporization of water is 40.67 kJ/mol, the enthalpy of fusion for water is 6.01 kJ/mol, the molar heat capacity of liquid water is 75.4 J/(mol ∙ °C), and the molar heat capacity of ice is 36.4 J/(mol ∙ °C).   show
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show B) 87.7 kJ  
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show C) 67.7 kJ  
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85) How much energy is required to heat 87.1 g acetone (molar mass=58.08 g/mol) from a solid at -154.0°C to a liquid at -42.0°C? The following physical data may be useful.   show
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86) How much energy must be removed from a 94.4 g sample of benzene (molar mass= 78.11 g/mol) at 322.0 K to solidify the sample and lower the temperature to 205.0 K? The following physical data may be useful.   show
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87) Identify triple point.   show
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88) Assign the appropriate labels to the phase diagram shown below.   show
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89) Consider the phase diagram shown. Choose the statement below that is TRUE.   show
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show D) fusion, followed by vaporization  
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show E) All of the above.  
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show E) H2O  
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93) Give the coordination number for a body-centered cubic cell.   show
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94) Determine the radius of an Al atom (in pm) if the density of aluminum is 2.71 g/cm3. Aluminum crystallizes in a face centered cubic structure with an edge length of 2 r.   show
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show B) Pd  
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96) Vanadium crystallizes in a body centered cubic structure and has an atomic radius of 131 pm. Determine the density of vanadium, if the edge length of a bcc structure is 4r/ .   show
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show C) I2  
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show A) (NH4)2CO3  
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99) Which of the following is considered an atomic solid?   show
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100) Which of the following is considered a nonbonding atomic solid?   show
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101) Identify the type of solid for AgCl.   show
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show D) molecular solid  
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103) Identify the type of solid for gold.   show
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104) Identify the type of solid for diamond.   show
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105) Identify the type of solid for argon.   show
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106) Which of the following substances should have the highest melting point?   show
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107) Which of the following substances should have the highest melting point?   show
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show B) 362 pm  
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2) Nickel has a face-centered cubic structure and has a density of 8.90 g/cm3. What is its atomic radius?   show
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3) Gold crystallizes in a face-centered cubic structure. What is the edge length of the unit cell if the atomic radius of gold is 144 pm?   show
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show D) 628 pm  
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show C) 8  
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6) Na Cl crystallizes in a cubic unit cell with Cl- ions on each corner and each face. How many Na+ and Cl- ions are in each unit cell of Na Cl?   show
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show C) 6  
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show B) C6H4Cl2  
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show C) Rb I  
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show C) metallic  
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1) Choose the statement below that is TRUE.   show
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2) Give the major force between ethanol and water.   show
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show A) dipole-dipole  
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show B) benzene (C6H6)  
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5) Which of the following compounds will be most soluble in ethanol (CH3CH2OH)?   show
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show E) 1-pentanol  
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7) Choose the situation below that would result in a ΔHsolution near 0.   show
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show C) When |ΔHsolute| < |ΔHhydration|  
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show A) When |ΔHsolute| > |ΔHhydration|  
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10) Which of the following ions should have the most exothermic ΔHhydration?   show
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11) Determine DHsolute for KBr if the DHsolution (KBr) = +19.9 kJ/mol and the ΔHhydration(KBr)=-670. kJ/mol.   show
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show A) rate of dissolution = rate of deposition  
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show C) rate of dissolution > rate of deposition  
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14) A solution containing less than the equilibrium amount is called __________.   show
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show C) The solution is considered saturated.  
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16) Which of the following statements is generally TRUE?   show
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17) A solid can be purified through what technique?   show
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show E) NaCl  
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show A) Na2SO4  
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20) Which of the following statements is TRUE?   show
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show B) In general, the solubility of a gas in water decreases with increasing temperature.  
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22) Identify the gas that is dissolved in carbonated sodas.   show
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show B) CO  
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24) Determine the solubility of N2 in water exposed to air at 25°C if the atmospheric pressure is 1.2 atm. Assume that the mole fraction of nitrogen is 0.78 in air and the Henry's law constant for nitrogen in water at this temperature is 6.1 × 10-4 M/atm   show
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25) Determine the solubility of CO2 in soda water at 25°C if the pressure of CO2 is 5.2 atm. The Henry's law constant for carbon dioxide in water at this temperature is 3.4 × 10-2 M/atm.   show
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show E) 0.32 atm  
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show A) 59 M/atm  
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28) Calculate the mass of oxygen (in mg) dissolved in a 5.00 L bucket of water exposed to a pressure of 1.13 atm of air. Assume the mole fraction of oxygen in air to be 0.21 and the Henry's law constant for oxygen in water at this temperature to be 1.3 ×   show
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29) Give the term for the amount of solute in moles per liter of solution.   show
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show A) molality  
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show E) 10^9  
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show D) molarity  
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33) Identify the colligative property.   show
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show E) 0.415 m  
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35) What mass (in g) of NH3 must be dissolved in 475 g of methanol to make a 0.250 m solution?   show
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36) How many moles of KF are contained in 347 g of water in a 0.175 m KF solution?   show
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37) How many moles of KF are contained in 244 mL of 0.135 m KF solution? The density of the solution is 1.22 g/mL.   show
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show D) 2.01 m  
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show E) 2.41 m  
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show A) 0.454 m  
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41) Commercial grade HCl solutions are typically 39.0% (by mass) HCl in water. Determine the molarity of the HCl, if the solution has a density of 1.20 g/mL.   show
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42) 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.   show
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show E) 9.31%  
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44) What mass of CuCl2 is contained in 75.85 g of a 22.4% by mass solution of CuCl2 in water?   show
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show C) 3.73 g  
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46) A solution is prepared by dissolving 38.6 g sucrose (C12H22O11) in 495 g of water. Determine the mole fraction of sucrose if the final volume of the solution is 508 mL.   show
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47) A solution is prepared by dissolving 76.3 g NaI in 545 g of water. Determine the mole fraction of NaI if the final volume of the solution is 576 mL.   show
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show D) 0.0252  
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show A) 0.00841  
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show C) 3.6 ppm  
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51) A 4.55 L sample of water contains 0.115 g of sodium ions. Determine the concentration of sodium ions in ppm if the density of the solution is 1.00 g/mL.   show
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52) What mass of ethane (CH3CH3) is contained in 50.0 mL of a 13.9% by mass solution of ethane in hexane? The density of the solution is 0.611 g/mL.   show
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53) Commercial grade HCl solutions are typically 39.0% (by mass) HCl in water. Determine the molality of the HCl, if the solution has a density of 1.20 g/mL.   show
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show D) 0.0476 M  
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show E) 0.318 m  
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show C) 23.1 torr  
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show A) 115 torr  
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show B) 1.65°C  
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59) Determine the freezing point of a solution that contains 78.8 g of naphthalene (C10H8, molar mass = 128.16 g/mol) dissolved in 722 mL of benzene (d = 0.877 g/mL). Pure benzene has a melting point of 5.50°C and a freezing point depression constant of   show
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show B) -30.0°C  
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show A) CCl4, Kb = 29.9°C/m  
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show A) 108°C  
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63) The boiling point elevation of an aqueous sucrose solution is found to be 0.39°C. What mass of sucrose (molar mass= 342.30 g/mol) would be needed to dissolve in 500.0 g of water? Kb (water) = 0.512°C/m.   show
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64) Determine the boiling point of a solution that contains 78.8 g of naphthalene (C10H8, molar mass = 128.16 g/mol) dissolved in 722 mL of benzene (d = 0.877 g/mL). Pure benzene has a boiling point of 80.1°C and a boiling point elevation constant of 2.5   show
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65) Give the reason that antifreeze is added to a car radiator.   show
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66) Place the following aqueous solutions of nonvolatile, nonionic compounds in order of decreasing osmotic pressure. I. 0.011 M sucrose II. 0.00095 M glucose III. 0.0060 M glycerin   show
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67) Place the following solutions in order of increasing osmotic pressure. I. 0.15 M C2H6O2 II. 0.15 M MgCl2 III. 0.15 M NaCl   show
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show B) 6.36 torr  
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69) A 150.0 mL sample of an aqueous solution at 25°C contains 15.2 mg of an unknown nonelectrolyte compound. If the solution has an osmotic pressure of 8.44 torr, what is the molar mass of the unknown compound?   show
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show E) FeCl3  
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71) Identify the solute with the lowest van't Hoff factor.   show
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show A) 0.100 m AlCl3  
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73) Choose the aqueous solution that has the highest boiling point. These are all solutions of nonvolatile solutes and you should assume ideal van't Hoff factors where applicable.   show
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74) Choose the aqueous solution with the lowest vapor pressure. These are all solutions of nonvolatile solutes and you should assume ideal van't Hoff factors where applicable.   show
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75) Choose the aqueous solution with the highest vapor pressure. These are all solutions of nonvolatile solutes and you should assume ideal van't Hoff factors where applicable.   show
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show B) 0.075 m (NH4)3PO4  
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show C) 0.200 m HOCH2CH2OH  
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show D) 2.7  
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show A) isosmotic  
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80) Solutions having osmotic pressures less than those of body fluids are called __________.   show
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show B) a solid dispersed in a gas  
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82) Identify the classification of milk.   show
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show E) solid emulsion  
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show C) foam  
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show B) Be2+ in set I and Zn2+ in set II  
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show A) 0.0 565 mol/L  
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3) The Henry's law constant for helium gas in water at 30°C is 3.70 × 10-4 M/atm. When the partial pressure of helium above a sample of water is 0.650 atm, the concentration of helium in the water is __________ M.   show
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4) What volume of a 0.716 M KBr solution is needed to provide 30.5 g of KBr?   show
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5) What volume of 3.00 M CH3OH solution is needed to provide 0. 220 mol of CH3OH?   show
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6) To make a 0.500 M solution, one could take 0.500 moles of solute and add   show
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show C) 4.79 g  
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8) What is the molality of a glucose solution prepared by dissolving 18.0 g of glucose, C6H12O6, in 125.9 g of water?   show
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show B) 1.00 kg of solvent.  
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show C) 0.85 m  
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show C) 5.49 m LiCl  
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12) A solution is prepared by adding 1.43 mol of KCl to 889 g of water. The concentration of KCl is __________ molal.   show
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13) A solution is prepared by dissolving 16.2 g of benzene (C6H6) in 282 g of carbon tetrachloride (CCl4) The concentration of benzene in this solution is __________ molal. The molar masses of C6H6 and CCl4 are 78.1 g/mol and 154 g/mol, respectively.   show
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14) What is the weight percent of vitamin C in a solution made by dissolving 6.50 g of vitamin C, C6H8O6, in 55.0 g of water?   show
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15) What is the weight percent of a caffeine solution made by dissolving 8.35 g of caffeine, C8H10N4O2, in 75 g of benzene, C6H6?   show
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show B) 74.2 g  
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show A) 0. 0960  
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show A) 0. 176  
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19) What is the mole fraction of I2 in a solution made by dissolving 55.6 g of I2 in 245 g of hexane, C6H14?   show
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20) What is the mole fraction of oxygen in a gas mixture that is 37% oxygen and 63% nitrogen by volume?   show
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21) A solution is 2.25% by weight NaHCO3. How many grams of NaHCO3 are in 150.0 g of solution?   show
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show C) 4.79  
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23) At 20°C, a 2.32 M aqueous solution of ammonium chloride has a density of 1.0344 g/mL. What is the molality of ammonium chloride in the solution? The formula weight of NH4Cl is 53.50 g/mol.   show
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show E) 2.00  
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25) A solution is prepared by dissolving 40.0 g of sucrose, C12H22O11, in 250. g of water at 25°C. What is the vapor pressure of the solution if the vapor pressure of water at 25°C is 23.76 mm Hg?   show
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26) A KCl solution is prepared by dissolving 25.0 g KCl in 250.0 g of water at 25°C. What is the vapor pressure of the solution if the vapor pressure of water at 25°C is 23.76 mm Hg?   show
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27) At a given temperature the vapor pressures of benzene and toluene are 183 mm Hg and 59.2 mm Hg, respectively. Calculate the total vapor pressure over a solution of benzene and toluene with Xbenzene = 0. 580.   show
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28) Which of the following solutions will have the lowest freezing point?   show
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29) What is the expected freezing point of a 0.50 m solution of Li2SO4 in water? Kf for water is 1.86°C/m.   show
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30) Calculate the freezing point of a solution of 40.0 g methyl salicylate, C7H6O2, dissolved in 800. g of benzene, C6H6. Kf for benzene is 5.10 °C/m and the freezing point is 5.50°C for benzene.   show
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show D) - 4.18°C  
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32) An aqueous solution has a normal boiling point of 103.0°C. What is the freezing point of this solution? For water Kb = 0.51 °C/m and Kf = 1.86 °C/m.   show
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show D) 116.3  
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show E) -115.4  
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35) Calculate the freezing point of a solution containing 5.0 grams of KCl and 550.0 grams of water. The molal-freezing-point-depression constant (Kf) for water is 1.86 °C/m.   show
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show C) 0.0136  
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