chapter 11
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chapter 11

Course Number: CHM CHM 1045, Fall 2011

College/University: UMiami

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Chemistry: A Molecular Approach, 2e (Tro) Chapter 11 Liquids, Solids, and Intermolecular Forces Multiple Choice Questions 1) Identify the characteristics of a liquid. A) indefinite shape and volume B) indefinite shape, but definite volume C) definite shape and volume D) none of the above E) all of the above Answer: B Diff: 1 Page Ref: 11.2 2) Which one of the following has a low density? A) gas B) liquid C) solid...

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A Chemistry: Molecular Approach, 2e (Tro) Chapter 11 Liquids, Solids, and Intermolecular Forces Multiple Choice Questions 1) Identify the characteristics of a liquid. A) indefinite shape and volume B) indefinite shape, but definite volume C) definite shape and volume D) none of the above E) all of the above Register to View AnswerDiff: 1 Page Ref: 11.2 2) Which one of the following has a low density? A) gas B) liquid C) solid D) none of the above E) all of the above Register to View AnswerDiff: 1 Page Ref: 11.2 3) Which one of the following has a definite shape and volume? A) gas B) liquid C) solid D) none of the above E) all of the above Register to View AnswerDiff: 1 Page Ref: 11.2 4) Give the change in condition to go from a liquid to a gas. A) increase heat or reduce pressure B) increase heat or increase pressure C) cool or reduce pressure D) cool or increase pressure E) none of the above Register to View AnswerDiff: 1 Page Ref: 11.2 5) The forces between polar molecules is known as __________. A) hydrogen bonding B) ion-dipole forces C) dipole-dipole forces D) dispersion forces E) ionic forces Register to View AnswerDiff: 1 Page Ref: 11.2 1 Copyright (c) 2011 Pearson Education, Inc. 6) Which of the following statements is TRUE? A) Intermolecular forces are generally stronger than bonding forces. B) The potential energy of molecules decrease as they get closer to one another. C) Energy is given off when the attraction between two molecules is broken. D) Increasing the pressure on a solid usually causes it to become a liquid. E) None of the above are true. Register to View AnswerDiff: 1 Page Ref: 11.3 7) What is the strongest type of intermolecular force present in H2? A) ion-dipole B) dipole-dipole C) dispersion D) hydrogen bonding E) none of the above Register to View AnswerDiff: 1 Page Ref: 11.3 8) What is the strongest type of intermolecular force present in CHF3? A) ion-dipole B) dispersion C) hydrogen bonding D) dipole-dipole E) none of the above Register to View AnswerDiff: 1 Page Ref: 11.3 9) What is the strongest type of intermolecular force present in NH2CH3? A) dispersion B) dipole-dipole C) hydrogen bonding D) ion-dipole E) none of the above Register to View AnswerDiff: 1 Page Ref: 11.3 10) What type of intermolecular force causes the dissolution of NaCl in water? A) hydrogen bonding B) dipole-dipole forces C) ion-dipole force D) dispersion forces E) none of the above Register to View AnswerDiff: 1 Page Ref: 11.3 2 Copyright (c) 2011 Pearson Education, Inc. 11) Choose the molecule or compound that exhibits dispersion forces as its strongest intermolecular force. A) Cl2 B) CO C) HF D) NaCl E) All of these have intermolecular forces stronger than dispersion. Register to View AnswerDiff: 2 Page Ref: 11.3 12) Choose the molecule or compound that exhibits dipole-dipole forces as its strongest intermolecular force. A) H2 B) SO2 C) NH3 D) CF4 E) BCl3 Register to View AnswerDiff: 2 Page Ref: 11.3 13) Choose the compound that exhibits hydrogen bonding as its strongest intermolecular force. A) SCl2 B) C2H6 C) CH3OH D) CH2F2 E) None of the above compounds exhibit hydrogen bonding. Register to View AnswerDiff: 2 Page Ref: 11.3 14) Place the following compounds in order of increasing strength of intermolecular forces. CO2 F2 NH2CH3 A) NH2CH3 < CO2 < F2 B) F2 < NH2CH3 < CO2 C) NH2CH3 < F2 < CO2 D) F2 < CO2 < NH2CH3 E) CO2 < NH2CH3 < F2 Register to View AnswerDiff: 2 Page Ref: 11.3 3 Copyright (c) 2011 Pearson Education, Inc. 15) Place the following compounds in order of increasing strength of intermolecular forces. CH4 CH3CH2CH3 CH3CH3 A) CH3CH2CH3 < CH4 < CH3CH3 B) CH3CH2CH3 < CH3CH3 < CH4 C) CH3CH3 < CH4 < CH3CH2CH3 D) CH4 < CH3CH2CH3 < CH3CH3 E) CH4 < CH3CH3 < CH3CH2CH3 Register to View AnswerDiff: 2 Page Ref: 11.3 16) Place the following compounds in order of decreasing strength of intermolecular forces. HF O2 CO2 A) HF > CO2 > O2 B) HF > O2 > CO2 C) O2 > CO2 > HF D) CO2 > HF > O2 E) CO2 > O2 > HF Register to View AnswerDiff: 2 Page Ref: 11.3 17) Place the following compounds in order of decreasing strength of intermolecular forces. I. CH3CH2CH2CH2CH2CH3 (CH3)3CCH2CH3 II. (CH3)3CCH3 A) III > II > I B) I > III > II C) I > II > III D) II > III > I E) III > I > II Register to View AnswerDiff: 2 Page Ref: 11.3 18) Which has the smallest dipole-dipole forces? A) CH3Cl B) HBr C) O2 D) NO Register to View AnswerDiff: 2 Page Ref: 11.3 4 Copyright (c) 2011 Pearson Education, Inc. III. 19) Which is expected to have the largest dispersion forces? A) C3H8 B) C12H26 C) F2 D) Be Cl2 Register to View AnswerDiff: 2 Page Ref: 11.3 20) Identify the compound that does not have dipole-dipole forces as its strongest force. A) CH2Cl2 B) CH3OCH3 C) CH3Br D) HCCl3 E) CO2 Register to View AnswerDiff: 2 Page Ref: 11.3 21) Which of the following compounds exhibits hydrogen bonding? A) CH3Cl B) HI C) CH3OCH3 D) NH3 Register to View AnswerDiff: 2 Page Ref: 11.3 22) Identify the compound that does not have hydrogen bonding. A) (CH3)3N B) H2O C) CH3OH D) HF E) CH3NH2 Register to View AnswerDiff: 2 Page Ref: 11.3 23) Choose the pair of substances that are most likely to form a homogeneous solution. A) NaCl and Hg B) LiF and C6H14 C) C3H8 and C2H5OH D) Br2 and PF3 E) NH3 and CH3OH Register to View AnswerDiff: 2 Page Ref: 11.3 5 Copyright (c) 2011 Pearson Education, Inc. 24) Choose the pair of substances that are most likely to form a homogeneous solution. A) C6H14 and C10H20 B) LiBr and C5H12 C) N2O4 and NH4Cl D) C6H14 and H2O E) None of the pairs above will form a homogeneous solution. Register to View AnswerDiff: 2 Page Ref: 11.3 25) Choose the pair of substances that are most likely to form a homogeneous solution. A) CCl4 and SCl2 B) NF3 and SO2 C) CO and C6H6 D) NH2CH3 and CH4 E) None of the pairs above will form a homogeneous solution. Register to View AnswerDiff: 2 Page Ref: 11.3 26) In liquid propanol, CH3CH2CH2OH which intermolecular forces are present? A) Dispersion, hydrogen bonding and dipole-dipole forces are present. B) Only dipole-dipole and ion-dipole forces are present. C) Only dispersion and dipole-dipole forces are present. D) Only hydrogen bonding forces are present. Register to View AnswerDiff: 3 Page Ref: 11.3 27) Which of the following compounds exhibits only dispersion and dipole-dipole intermolecular interactions? A) H 2 B) HI C) CO2 D) CH3NH2 Register to View AnswerDiff: 3 Page Ref: 11.3 28) The normal boiling point for H2Se is higher than the normal boiling point for H2S . This can be explained by A) larger dipole-dipole forces for H2Se . B) larger dispersion forces for H2Se . C) larger hydrogen-bond forces for H2Se . D) larger dipole-dipole forces, larger dispersion forces, and larger hydrogen-bond forces for H2Se . Register to View AnswerDiff: 3 Page Ref: 11.3 6 Copyright (c) 2011 Pearson Education, Inc. 29) In a liquid, the energy required to increase the surface of the area by a unit amount is called __________. A) viscosity B) surface tension C) dipole-dipole force D) hydrogen bonding E) capillary action Register to View AnswerDiff: 1 Page Ref: 11.4 30) Choose the substance with the highest surface tension. A) HOCH2CH2OH B) CH2F2 C) CH3CH2F D) CH3CH2OH E) CH3CH2CH3 Register to View AnswerDiff: 2 Page Ref: 11.4 31) Choose the substance with the lowest surface tension. A) CH3SH B) CH3CH2CH2CH3 C) C6H6 D) H2O E) (CH3)2CO Register to View AnswerDiff: 2 Page Ref: 11.4 32) Choose the substance with the highest viscosity. A) (CH3CH2)2CO B) C2H4Cl2 C) HOCH2CH2CH2CH2OH D) CF4 E) C6H14 Register to View AnswerDiff: 2 Page Ref: 11.4 33) Choose the substance with the lowest viscosity. A) Cl3CCCl3 B) Cl2CHCH2Cl C) Cl2CHCHCl2 D) ClCH2CH2Cl E) Cl3CCHCl2 Register to View AnswerDiff: 2 Page Ref: 11.4 7 Copyright (c) 2011 Pearson Education, Inc. 34) Choose the substance with the highest viscosity. A) SbCl3 B) AsCl5 C) ICl2 D) BeCl2 E) OCl2 Register to View AnswerDiff: 2 Page Ref: 11.4 35) Identify the substance with the highest viscosity. A) gasoline B) water C) corn syrup D) motor oil E) tea Register to View AnswerDiff: 2 Page Ref: 11.4 36) Identify the term used to describe the ability of a liquid to flow against gravity up a narrow tube. A) capillary action B) viscosity C) surface tension D) density E) none of the above Register to View AnswerDiff: 2 Page Ref: 11.4 37) Which of the following statements is TRUE? A) Vapor pressure increases with temperature. B) Hydrogen bonds are stronger than covalent bonds. C) Intermolecular forces hold the atoms in molecules together. D) Dispersion forces are generally stronger than dipole-dipole forces. E) None of the above are true. Register to View AnswerDiff: 1 Page Ref: 11.5 38) Which of the following statements is FALSE? A) The rate of vaporization increases with increasing surface area. B) The rate of vaporization increases with decreasing strength of intermolecular forces. C) The rate of vaporization increases with increasing temperature. D) Molecules with hydrogen bonding are more volatile than compounds with dipole-dipole forces. E) None of the above are false. Register to View AnswerDiff: 1 Page Ref: 11.5 8 Copyright (c) 2011 Pearson Education, Inc. 39) Which substance below has the strongest intermolecular forces? A) A2X, Hvap= 39.6 kJ/mol B) BY2, Hvap= 26.7 kJ/mol C) C3X2, Hvap= 36.4 kJ/mol D) DX2, Hvap= 23.3 kJ/mol E) EY3, Hvap= 21.5 kJ/mol Register to View AnswerDiff: 1 Page Ref: 11.5 40) Define boiling. A) A liquid becomes a gas. B) A gas becomes a liquid. C) A gas becomes a solid. D) A solid becomes a gas. E) A solid becomes a liquid. Register to View AnswerDiff: 1 Page Ref: 11.5 41) Give the term for the temperature at which the gas and liquid phases form a supercritical fluid. A) absolute temperature B) definite temperature C) fluid temperature D) critical temperature E) solid temperature Register to View AnswerDiff: 1 Page Ref: 11.5 42) Choose the substance with the highest vapor pressure at a given temperature. A) SiS2 B) RbCl C) CH3SCH3 D) BF3 E) SbH3 Register to View AnswerDiff: 2 Page Ref: 11.5 43) Choose the substance with the lowest vapor pressure at a given temperature. A) CO2 B) BeCl2 C) BF3 D) He E) PF5 Register to View AnswerDiff: 2 Page Ref: 11.5 9 Copyright (c) 2011 Pearson Education, Inc. 44) Place the following substances in order of increasing boiling point. Ne Cl2 O2 A) Ne < Cl2 < O2 B) Cl2 < O2 < Ne C) O2 < Cl2 < Ne D) Cl2 < Ne < O2 E) Ne < O2 < Cl2 Register to View AnswerDiff: 2 Page Ref: 11.5 45) Place the following substances in order of increasing boiling point. CH3CH2OH Ar CH3OCH3 A) Ar < CH3OCH3 < CH3CH2OH B) CH3CH2OH < Ar < CH3OCH3 C) CH3CH2OH < CH3OCH3 < Ar D) CH3OCH3 < Ar < CH3CH2OH E) Ar < CH3CH2OH < CH3OCH3 Register to View AnswerDiff: 2 Page Ref: 11.5 46) Choose the substance with the highest boiling point. A) CH4 B) KI C) CS2 D) HF E) I2 Register to View AnswerDiff: 2 Page Ref: 11.5 47) Choose the substance with the lowest boiling point. A) H2S B) NBr3 C) F2 D) CF2H2 E) H2O2 Register to View AnswerDiff: 2 Page Ref: 11.5 10 Copyright (c) 2011 Pearson Education, Inc. 48) Which of the following substances would you predict to have the highest Hvap? A) CH3Cl B) HCl C) HOCH2CH2OH D) CH3CH2OH E) CH3CH2CH2CH3 Register to View AnswerDiff: 2 Page Ref: 11.5 49) Which of the following substances would you predict to have the highest Hvap? A) Xe B) C6H6 C) SiF4 D) Br2 E) N2 Register to View AnswerDiff: 2 Page Ref: 11.5 50) How much energy is required to vaporize 48.7 g of dichloromethane (CH2Cl2) at its boiling point, if its Hvap is 31.6 kJ/mol? A) 31.2 kJ B) 6.49 kJ C) 55.1 kJ D) 15.4 kJ E) 18.1 kJ Register to View AnswerDiff: 3 Page Ref: 11.5 51) How much energy is required to vaporize 98.6 g of ethanol (C2H5OH) at its boiling point, if its Hvap is 40.5 kJ/mol? A) 86.7 kJ B) 11.5 kJ C) 18.9 kJ D) 52.8 kJ E) 39.9 kJ Register to View AnswerDiff: 3 Page Ref: 11.5 52) How much energy is required to vaporize 158 g of butane (C4H10) at its boiling point, if its Hvap is 24.3 kJ/mol? A) 15.1 kJ B) 66.1 kJ C) 89.4 kJ D) 11.2 kJ E) 38.4 kJ Register to View Answer11 Copyright (c) 2011 Pearson Education, Inc. Diff: 3 Page Ref: 11.5 53) Based on the figure above, the boiling point of diethyl ether under an external pressure of 1.32 atm is __________C. A) 10 B) 20 C) 30 D) 40 E) 0 Register to View AnswerDiff: 3 Page Ref: 11.5 54) Based on the figure above, the boiling point of ethyl alcohol under an external pressure of 0.0724 atm is __________C. A) 80 B) 60 C) 70 D) 40 E) 20 Register to View AnswerDiff: 3 Page Ref: 11.5 55) Based on the figure above, the boiling point of water under an external pressure of 0.316 atm is __________C. A) 70 B) 40 C) 60 D) 80 E) 90 Register to View Answer12 Copyright (c) 2011 Pearson Education, Inc. Diff: 3 Page Ref: 11.5 56) Place the following substances in order of increasing vapor pressure at a given temperature. SF6 SiH4 SF4 A) SF6 < SiH4 < SF4 B) SiH4 < SF4 < SF6 C) SF6 < SF4 < SiH4 D) SF4 < SF6 < SiH4 E) SiH4 < SF6 < SF4 Register to View AnswerDiff: 4 Page Ref: 11.5 57) Place the following substances in order of decreasing vapor pressure at a given temperature. PF5 BrF3 CF4 A) BrF3 > PF5 > CF4 B) BrF3 > CF4 > PF5 C) PF5 > BrF3 > CF4 D) CF4 > BrF3 > PF5 E) CF4 > PF5 > BrF3 Register to View AnswerDiff: 4 Page Ref: 11.5 58) Place the following substances in order of increasing vapor pressure at a given temperature. NF3 NH3 BCl3 A) NH3 < NF3 < BCl3 B) NF3 < NH3 < BCl3 C) BCl3 < NF3 < NH3 D) NH3 < BCl3 < NF3 E) BCl3 < NH3 < NF3 Register to View AnswerDiff: 4 Page Ref: 11.5 13 Copyright (c) 2011 Pearson Education, Inc. 59) Place the following substances in order of decreasing vapor pressure at a given temperature. BeF2 CH3OH OF2 A) CH3OH > OF2 > BeF2 B) BeF2 > OF2 > CH3OH C) OF2 > CH3OH > BeF2 D) OF2 > BeF2 > CH3OH E) BeF2 > CH3OH > OF2 Register to View AnswerDiff: 4 Page Ref: 11.5 60) Place the following substances in order of decreasing boiling point. H2O N2 CO A) CO > H2O > N2 B) N2 > CO > H2O C) H2O > CO > N2 D) CO > N2 > H2O E) N2 > H2O > CO Register to View AnswerDiff: 4 Page Ref: 11.5 61) Place the following substances in order of decreasing boiling point. N2 O2 H2 A) O2 > H2 > N2 B) N2 > H2 > O2 C) N2 > O2 > H2 D) O2 > N2 > H2 E) H2 > N2 > O2 Register to View AnswerDiff: 4 Page Ref: 11.5 14 Copyright (c) 2011 Pearson Education, Inc. 62) Place the following substances in order of decreasing boiling point. He Ar H2 A) He > H2 > Ar B) H2 > He > Ar C) He > Ar > H2 D) Ar > He > H2 E) H2 > Ar > He Register to View AnswerDiff: 4 Page Ref: 11.5 63) Which of the following compounds has the highest boiling point? A) H2O B) H Cl C) H2S D) N H3 Register to View AnswerDiff: 4 Page Ref: 11.5 64) Determine Hvap for a compound that has a measured vapor pressure of 24.3 torr at 273 K and 135 torr at 325 K. A) 41 kJ/mol B) 79 kJ/mol C) 24 kJ/mol D) 13 kJ/mol E) 34 kJ/mol Register to View AnswerDiff: 5 Page Ref: 11.5 65) Determine the normal boiling point of a substance whose vapor pressure is 55.1 mm Hg at 35C and has a Hvap of 32 .1 kJ/mol. A) 255 K B) 368 K C) 412 K D) 390. K E) 466 K Register to View AnswerDiff: 5 Page Ref: 11.5 15 Copyright (c) 2011 Pearson Education, Inc. 66) Determine the vapor pressure (in mm Hg) of a substance at 29C, whose normal boiling point is 76C and has a Hvap of 38.7 kJ/mol. A) 80 mm Hg B) 13 mm Hg C) 21 mm Hg D) 48 mm Hg E) 96 mm Hg Register to View AnswerDiff: 5 Page Ref: 11.5 67) Determine the vapor pressure (in torr) of a substance at 36C, whose normal boiling point is 84C and has a Hvap of 22.1 kJ/mol. A) 239 torr B) 31.8 torr C) 41.8 torr D) 147 torr E) 98 torr Register to View AnswerDiff: 5 Page Ref: 11.5 68) Define deposition. A) A liquid becomes a gas. B) A gas becomes a liquid. C) A gas becomes a solid. D) A solid becomes a gas. E) A solid becomes a liquid. Register to View AnswerDiff: 1 Page Ref: 11.6 69) Define sublimation. A) the phase transition from solid to gas B) the phase transition from gas to solid C) the phase transition from gas to liquid D) the phase transition from liquid to gas E) the phase transition from to liquid solid Register to View AnswerDiff: 1 Page Ref: 11.6 70) Define freezing. A) the phase transition from solid to gas B) the phase transition from gas to solid C) the phase transition from gas to liquid D) the phase transition from liquid to gas E) the phase transition from liquid to solid Register to View AnswerDiff: 1 Page Ref: 11.6 16 Copyright (c) 2011 Pearson Education, Inc. 71) At atmospheric pressure, dry ice __________. A) freezes B) deposits C) sublimes D) melts E) boils Register to View AnswerDiff: 1 Page Ref: 11.6 72) The melting point of water is __________. A) 0C B) 32C C) 212C D) 100C E) 273C Register to View AnswerDiff: 1 Page Ref: 11.6 73) The freezing point of water is __________. A) 0C B) 32C C) 212C D) 100C E) 273C Register to View AnswerDiff: 1 Page Ref: 11.6 74) The boiling point of water is __________. A) 0C B) 32C C) 212C D) 100C E) 273C Register to View AnswerDiff: 1 Page Ref: 11.6 75) The heat of vaporization of water at 100C 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 100C. A) 20.3 kJ of heat are absorbed. B) 20.3 kJ of heat are released. C) 81.3 kJ of heat are absorbed. D) 81.3 kJ of heat are released. Register to View AnswerDiff: 4 Page Ref: 11.7 17 Copyright (c) 2011 Pearson Education, Inc. 76) Calculate the total quantity of heat required to convert 25.0 g of liquid CCl4(l) from 35.0C to gaseous CCl4 at 76.8C (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 heat of vaporization is 29.82 kJ/mol. A) 0.896 kJ B) 1.43 kJ C) 5.74 kJ D) 6.28 kJ Register to View AnswerDiff: 4 Page Ref: 11.7 77) The enthalpy change for converting 1.00 mol of ice at -50.0C to water at 70.0C is __________ kJ. The specific heats of ice, water, and steam are 2.09 J/gK, 4.18 J/gK, and 1.84 J/gK, respectively. For H2O, Hfus = 6.01 kJ/mol, and Hvap = 40.67 kJ/mol. A) 12.28 B) 6.41 C) 13.16 D) 7154 E) 9.40 Register to View AnswerDiff: 4 Page Ref: 11.7 78) The enthalpy change for converting 10.0 g of ice at -25.0C to water at 80.0C is __________ kJ. The specific heats of ice, water, and steam are 2.09 J/gK, 4.18 J/gK, and 1.84 J/gK, respectively. For H2O, Hfus = 6.01 kJ/mol, and Hvap = 40.67 kJ/mol. A) 12.28 B) 6.16 C) 3870 D) 7.21 E) 9.88 Register to View AnswerDiff: 4 Page Ref: 11.7 79) The fluorocarbon C2Cl3F3 has a normal boiling point of 47.6C. 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 the compound from the liquid at 5.0C to the gas at 80.0C is __________ kJ. A) 8.19 B) 1454 C) 30.51 D) 3031 E) 10.36 Register to View AnswerDiff: 4 Page Ref: 11.7 18 Copyright (c) 2011 Pearson Education, Inc. 80) Ethanol (C2H5OH) melts at -114C. The enthalpy of fusion is 5.02 kJ/mol. The specific heats of solid and liquid ethanol are 0.97 J/gK and 2.3 J/gK, respectively. How much heat (kJ) is needed to convert 25.0 g of solid ethanol at -135C to liquid ethanol at -50C? A) 207.3 kJ B) -12.7 kJ C) 6.91 kJ D) 4192 kJ E) 9.21 kJ Register to View AnswerDiff: 4 Page Ref: 11.7 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? A) 8.18 kJ B) 341 kJ C) 528 kJ D) 3410 kJ Register to View AnswerDiff: 4 Page Ref: 11.7 82) How much heat is released when 105 g of steam at 100.0C is cooled to ice at -15.0C? The 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). A) 54.8 kJ B) 273 kJ C) 319 kJ D) 347 kJ Register to View AnswerDiff: 4 Page Ref: 11.7 19 Copyright (c) 2011 Pearson Education, Inc. 83) How much energy is required to heat 36.0 g H2O from a liquid at 65C to a gas at 115C? The following physical data may be useful. Hvap = 40.7 kJ/mol Cliq = 4.18 J/gC Cgas = 2.01 J/gC Csol = 2.09 J/gC Tmelting = 0C Tboiling = 100C A) 63.5 kJ B) 87.7 kJ C) 10.9 kJ D) 52.7 kJ E) 91.7 kJ Register to View AnswerDiff: 5 Page Ref: 11.7 84) How much energy must be removed from a 125 g sample of benzene (molar mass= 78.11 g/mol) at 425.0 K to liquify the sample and lower the temperature to 335.0 K? The following physical data may be useful. Hvap = 33.9 kJ/mol Hfus = 9.8 kJ/mol Cliq = 1.73 J/gC Cgas = 1.06 J/gC Csol = 1.51 J/gC Tmelting = 279.0 K Tboiling = 353.0 K A) 38.9 kJ B) 95.4 kJ C) 67.7 kJ D) 54.3 kJ E) 74.4 kJ Register to View AnswerDiff: 5 Page Ref: 11.7 20 Copyright (c) 2011 Pearson Education, Inc. 85) How much energy is required to heat 87.1 g acetone (molar mass=58.08 g/mol) from a solid at -154.0C to a liquid at -42.0C? The following physical data may be useful. Hfus = 7.27 kJ/mol Cliq = 2.16 J/gC Cgas = 1.29 J/gC Csol = 1.65 J/gC Tmelting = -95.0C A) 8.48 kJ B) 18.5 kJ C) 32.2 kJ D) 29.4 kJ E) 9.97 kJ Register to View AnswerDiff: 5 Page Ref: 11.7 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. Hvap = 33.9 kJ/mol Hfus = 9.8 kJ/mol Cliq = 1.73 J/gC Cgas = 1.06 J/gC Csol = 1.51 J/gC Tmelting = 279.0 K Tboiling = 353.0 K A) 17.6 kJ B) 11.8 kJ C) 70.2 kJ D) 10.5 kJ E) 29.4 kJ Register to View AnswerDiff: 5 Page Ref: 11.7 87) Identify triple point. A) The temperature, pressure, and density for a gas. B) The temperature at which the boiling point equals the melting point. C) The temperature and pressure where liquid, solid, and gas are equally stable and are in equilibrium. D) The temperature that is unique for a substance. E) The temperature at which the solid and liquid co-exist. Register to View AnswerDiff: 1 Page Ref: 11.8 21 Copyright (c) 2011 Pearson Education, Inc. 88) Assign the appropriate labels to the phase diagram shown below. A) A = liquid, B = solid, C = gas, D = critical point B) A = gas, B = solid, C = liquid, D = triple point C) A = gas, B = liquid, C = solid, D = critical point D) A = solid, B = gas, C = liquid, D = supercritical fluid E) A = liquid, B = gas, C = solid, D = triple point Register to View AnswerDiff: 1 Page Ref: 11.8 89) Consider the phase diagram shown. Choose the statement below that is TRUE. A) The triple point of this substance occurs at a temperature of 31C. B) At 10 atm of pressure, there is no temperature where the liquid phase of this substance would exist. C) The solid phase of this substance is higher in density than the liquid phase. D) The line separating the solid and liquid phases represents the Hvap. E) None of the above are true. Register to View Answer22 Copyright (c) 2011 Pearson Education, Inc. Diff: 1 Page Ref: 11.8 90) Consider the phase diagram below. If the dashed line at 1 atm of pressure is followed from 100 to 500C, what phase changes will occur (in order of increasing temperature)? A) condensation, followed by vaporization B) sublimation, followed by deposition C) vaporization, followed by deposition D) fusion, followed by vaporization E) No phase change will occur under the conditions specified. Register to View AnswerDiff: 1 Page Ref: 11.8 91) Why is water an extraordinary substance? A) Water has a low molar mass, yet it is a liquid at room temperature. B) Water is the main solvent within living organisms. C) Water has an exceptionally high specific heat capacity. D) Water has strong hydrogen bonding. E) All of the above. Register to View AnswerDiff: 1 Page Ref: 11.9 92) Identify the compound with the highest boiling point. A) CH4 B) NH3 C) HF D) H2S E) H2O Register to View AnswerDiff: 1 Page Ref: 11.9 23 Copyright (c) 2011 Pearson Education, Inc. 93) Give the coordination number for a body-centered cubic cell. A) 4 B) 6 C) 8 D) 10 E) 12 Register to View AnswerDiff: 1 Page Ref: 11.9 94) Determine the radius of an Al atom (in pm) if the density of aluminum is 2.71 g/cm 3. Aluminum crystallizes in a face centered cubic structure with an edge length of 2 2 r. A) 143 pm B) 227 pm C) 96 pm D) 172 pm E) 193 pm Register to View AnswerDiff: 5 Page Ref: 11.11 95) A metal crystallizes in a face centered cubic structure and has a density of 11.9 g/cm3. If the radius of the metal atom is 138 pm, what is the identity of the metal? A) At B) Pd C) Mn D) Fe E) Cr Register to View AnswerDiff: 5 Page Ref: 11.11 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/ 3 . A) 3.06 g/cm3 B) 12.2 g/cm3 C) 6.11 g/cm3 D) 2.77 g/cm3 E) 8.46 g/cm3 Register to View AnswerDiff: 5 Page Ref: 11.11 97) Which of the following is considered a molecular solid? A) Cu B) NH4NO3 C) I2 D) Xe E) None of these is a molecular solid. Register to View AnswerDiff: 1 Page Ref: 11.12 24 Copyright (c) 2011 Pearson Education, Inc. 98) Which of the following is considered an ionic solid? A) (NH4)2CO3 B) CCl4 C) SeBr2 D) XeF4 E) None of these is an ionic solid. Register to View AnswerDiff: 1 Page Ref: 11.12 99) Which of the following is considered an atomic solid? A) Br2 B) CsCl C) N2 D) Nb E) None of these is an atomic solid. Register to View AnswerDiff: 1 Page Ref: 11.12 100) Which of the following is considered a nonbonding atomic solid? A) Ne B) Fe C) I2 D) Ca E) Li Register to View AnswerDiff: 1 Page Ref: 11.12 101) Identify the type of solid for AgCl. A) metallic atomic solid B) ionic solid C) nonbonding atomic solid D) molecular solid E) networking atomic solid Register to View AnswerDiff: 1 Page Ref: 11.12 102) Identify the type of solid for ice. A) metallic atomic solid B) ionic solid C) nonbonding atomic solid D) molecular solid E) networking atomic solid Register to View AnswerDiff: 1 Page Ref: 11.12 25 Copyright (c) 2011 Pearson Education, Inc. 103) Identify the type of solid for gold. A) metallic atomic solid B) ionic solid C) nonbonding atomic solid D) molecular solid E) networking atomic solid Register to View AnswerDiff: 1 Page Ref: 11.12 104) Identify the type of solid for diamond. A) metallic atomic solid B) ionic solid C) nonbonding atomic solid D) molecular solid E) networking atomic solid Register to View AnswerDiff: 1 Page Ref: 11.12 105) Identify the type of solid for argon. A) metallic atomic solid B) ionic solid C) nonbonding atomic solid D) molecular solid E) networking atomic solid Register to View AnswerDiff: 1 Page Ref: 11.12 106) Which of the following substances should have the highest melting point? A) CO2 B) SrS C) Xe D) F2 E) MgO Register to View AnswerDiff: 1 Page Ref: 11.12 107) Which of the following substances should have the highest melting point? A) Fe B) Ne C) Xe D) N2 E) CO Register to View AnswerDiff: 1 Page Ref: 11.12 26 Copyright (c) 2011 Pearson Education, Inc. Algorithmic Questions 1) What is the edge length of a face-centered cubic unit cell made up of atoms having a radius of 128 pm? A) 181 pm B) 362 pm C) 512 pm D) 1020 pm Register to View AnswerDiff: 5 Page Ref: 11.11 2) Nickel has a face-centered cubic structure and has a density of 8.90 g/cm3. What is its atomic radius? A) 125 pm B) 249 pm C) 353 pm D) 997 pm Register to View AnswerDiff: 5 Page Ref: 11.11 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? A) 204 pm B) 288 pm C) 333 pm D) 407 pm Register to View AnswerDiff: 5 Page Ref: 11.11 4) Cesium has a radius of 272 pm and crystallizes in a body-centered cubic structure. What is the edge length of the unit cell? A) 314 pm B) 385 pm C) 544 pm D) 628 pm Register to View AnswerDiff: 5 Page Ref: 11.11 5) Lithium crystallizes in a body-centered cubic structure. What is the coordination number of each atom? A) 4 B) 6 C) 8 D) 12 Register to View AnswerDiff: 5 Page Ref: 11.11 27 Copyright (c) 2011 Pearson Education, Inc. 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? A) 1 Na+ ion and 1 Cl- ion B) 2 Na+ ions and 2 Cl- ions C) 4 Na+ ions and 4 Cl- ions D) 8 Na+ ions and 8 Cl- ions Register to View AnswerDiff: 5 Page Ref: 11.11 7) How many H- ions are around each Na+ ion in NaH, which has a cubic unit cell with Hions on each corner and each face? A) 1 B) 4 C) 6 D) 8 Register to View AnswerDiff: 5 Page Ref: 11.11 8) Which of the following forms a molecular solid? A) NH4NO3 B) C6H4Cl2 C) SiO2 D) copper Register to View AnswerDiff: 1 Page Ref: 11.12 9) Which of the following forms an ionic solid? A) Ag B) C7H15NH2 C) Rb I D) S O3 Register to View AnswerDiff: 1 Page Ref: 11.12 10) Which type of bonding does Sr form upon solidification? A) covalent network B) ionic C) metallic D) molecular Register to View AnswerDiff: 2 Page Ref: 11.12 28 Copyright (c) 2011 Pearson Education, Inc. Matching Questions Match the following. A) H2 + H2O B) dispersion forces C) hydrogen bonding D) ion-dipole forces E) ionic bond F) dipole-dipole forces 1) LiI Diff: 1 Page Ref: 11.3 2) CH3OH Diff: 1 Page Ref: 11.3 3) CH3CH3 Diff: 1 Page Ref: 11.3 4) CH2F2 Diff: 1 Page Ref: 11.3 5) LiI + H2O Diff: 1 Page Ref: 11.3 Answers: 1) E 2) C 3) B 4) F 5) D Short Answer Questions 1) Why do O, F and N, when bonded to H, form such strong intermolecular attractions to neighboring molecules? Make sure to be specific. Answer: Oxygen, fluorine and nitrogen are all very small and highly electronegative elements. When they bond to hydrogen they form extremely polar bonds. These extremely polar bonds formed between small atoms can get very close to interact with other molecules. The closer the molecules get, the more strongly they can interact. In addition, these three elements usually have lone pair electrons which make the attractions to other molecules even stronger. Diff: 1 Page Ref: 11.3 2) Define viscosity. Answer: Viscosity is the resistance of a liquid to flow. Diff: 2 Page Ref: 11.4 29 Copyright (c) 2011 Pearson Education, Inc. 3) Why does the temperature of a substance stay constant during a phase change such as vaporization? Answer: 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). Diff: 1 Page Ref: 11.5 4) Define volatile. Answer: Liquids that vaporize easily. Diff: 1 Page Ref: 11.5 5) Define boiling point of a liquid. Answer: The temperature at which the vapor pressure equals the external pressure. Diff: 1 Page Ref: 11.5 6) Define dynamic equilibrium. Answer: Dynamic equilibrium is when the rate of condensation equals the rate of vaporization. Diff: 2 Page Ref: 11.5 7) Why is the Hvap higher than Hfus for a given compound? Answer: Vaporizing a substance requires the complete "breaking" of all intermolecular attractions, whereas the melting of a substance only requires the breaking of a portion of the intermolecular attractions. Diff: 1 Page Ref: 11.6 8) Sketch the phase diagram of benzene. Make sure to label the axes and the different phases of benzene. Use the physical data provided below. melting point = 279 K boiling point = 353 K Tc = 562 K Pc = 48.4 atm Triple Point = 0.05 atm, 279 K Answer: Sketch should include all given information showing fusion and vaporization curves. Diff: 3 Page Ref: 11.8 9) Give the edge length in terms of r for a simple cubic cell. Answer: 2r Diff: 1 Page Ref: 11.9 10) Describe the difference between the conduction band and the valence band. Answer: The valence band is the group of highest energy occupied orbitals in the solid. The conduction band is the set of empty orbitals that are higher in energy than the valence band. In metals the difference in energy between the valence band and conduction band is fairly small, making it easy for electrons to move from the valence band to the conduction band. Diff: 2 Page Ref: 11.12 30 Copyright (c) 2011 Pearson Education, Inc.

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UMiami - CHM - CHM 1045
Chemistry: A Molecular Approach, 2e (Tro) Chapter 12 Solutions Multiple Choice Questions 1) Choose the statement below that is TRUE. A) A solution will form between two substances if the solute-solvent interactions are of comparable strength to the solute
UMiami - CHM - CHM 1045
Chemistry: A Molecular Approach, 2e (Tro)Chapter 13 Chemical KineticsMultiple Choice Questions1) Given the following balanced equation, determine the rate of reaction with respect to [SO 2].2 SO2 (g) + O2(g) 2 SO3(g)1 [SO2 ]2 Dt1 [SO 2 ]B) Rate =
UMiami - CHM - CHM 1045
Chemistry: A Molecular Approach, 2e (Tro) Chapter 15 Acids and Bases Multiple Choice Questions 1) Identify the acid that is in car batteries. A) H2SO4 B) HNO3 C) H2CO3 D) CH3COOH E) HF Answer: A Diff: 1 Page Ref: 15.2 2) Identify the acid that is in vineg
UMiami - CHM - CHM 1045
Chemistry: A Molecular Approach, 2e (Tro) Chapter 16 Aqueous Ionic Equilibrium Multiple Choice Questions 1) Identify a good buffer. A) small amounts of both a weak acid and its conjugate base B) significant amounts of both a strong acid and a strong base
UMiami - CHM - CHM 1045
Chemistry: A Molecular Approach, 2e (Tro)Chapter 17 Free Energy and ThermodynamicsMultiple Choice Questions1) Which of the following statements is TRUE?A) There is a &quot;heat tax&quot; for every energy transaction.B) A spontaneous reaction is always a fast r
UMiami - CHM - CHM 1045
Chemistry: A Molecular Approach, 2e (Tro)Chapter 18 ElectrochemistryMultiple Choice Questions1) Identify oxidation.A) increase in oxidation numberB) loss of electronsC) gain of electronsD) decrease in oxidation numberE) both A and BAnswer: EDiff
UMiami - CHM - CHM 1045
Chemistry: A Molecular Approach, 2e (Tro) Chapter 19 Radioactivity and Nuclear Chemistry Multiple Choice Questions 1) Identify the radioactive green light that glows in the dark. A) phenolphthalein B) radioactivity C) phosphorescence D) desensitivity E) n
UMiami - CHM - CHM 1045
Chemistry: A Molecular Approach, 2e (Tro)Chapter 20 Organic ChemistryMultiple Choice Questions1) Give the number of covalent bonds that a carbon atom can form.A) 1B) 2C) 3D) 4E) 5Answer: DDiff: 1Page Ref: 20.22) Identify the formula for an alk
UMiami - CHM - CHM 1045
Chemistry: A Molecular Approach, 2e (Tro)Chapter 21 BiochemistryMultiple Choice Questions1) What type of lipid is the following compound?A) steroidB) phospholipidC) glycolipidD) fatty acidE) triglycerideAnswer: ADiff: 1Page Ref: 21.22) What ty
UMiami - CHM - CHM 1045
Chemistry: A Molecular Approach, 2e (Tro)Chapter 22 Chemistry of the NonmetalsMultiple Choice Questions1) Which of the following are MAJOR components of Earth's crust?A) oxygen and siliconB) calcium and siliconC) oxygen and ironD) oxygen, hydrogen
UMiami - CHM - CHM 1045
Chemistry: A Molecular Approach, 2e (Tro) Chapter 23 Metals and Metallurgy Multiple Choice Questions 1) Which of the following is NOT generally a property of a metal? A) high resistivity B) good conductor of heat C) malleable D) ductile E) opaque Answer:
UMiami - BIO - bio1011
Chapter 40 - Test Bank: Plant Defense ResponsesChapter 40Test Bank: Plant Defense ResponsesMultiple Choice Questions1. _ occurs when a chemical signal secreted by the roots of one plant blocks thegermination of nearby seeds or inhibits the growth of
UMiami - BIO - bio1011
Chapter 41 - Test Bank: Sensory Systems in PlantsChapter 41Test Bank: Sensory Systems in PlantsMultiple Choice Questions1. If temperatures suddenly rise 5 to 10 C, _ proteins are produced to helpstabilize other proteins.A. denaturedB. photosensitiv
UMiami - BIO - bio1011
Chapter 42 - Test Bank: Plant ReproductionChapter 42Test Bank: Plant ReproductionMultiple Choice Questions1. Which of these characteristics would most likely discourage self pollination in a flowerwith both stamens and pistils?A. many more stamens t
UMiami - BIO - bio1011
Chapter 43 - Test Bank: The Animal Body and Principles of RegulationChapter 43Test Bank: The Animal Body and Principles of RegulationMultiple Choice Questions1. Which of these is not part of loose connective tissue?A. collagenB. elastinC. reticulin
UMiami - BIO - bio1011
Chapter 44 - Test Bank: The Nervous SystemChapter 44Test Bank: The Nervous SystemMultiple Choice Questions1. A(n) _ diffuses across a narrow synaptic cleft between the presynapticaxon and the postsynaptic cell to transmit a nerve impulse.A. neurotra
UMiami - BIO - bio1011
Chapter 45 - Test Bank: Sensory SystemsChapter 45Test Bank: Sensory SystemsMultiple Choice Questions1. All input from sensory neurons to the central nervous system arrives in the same form,as _ propagated by afferent sensory neurons. Perception of th
UMiami - BIO - bio1011
Chapter 46 - Test Bank: The Endocrine SystemChapter 46Test Bank: The Endocrine SystemMultiple Choice Questions1. Homeostasis is achieved through the actions of two major regulatory systems, theendocrine system and the _ system.A. nervousB. circulat
UMiami - BIO - bio1011
Chapter 47 - Test Bank: The Musculoskeletal SystemChapter 47Test Bank: The Musculoskeletal SystemMultiple Choice Questions1. The mammalian jaw is an example of what kind of moveable joint?A. hinge jointB. combination jointC. gliding jointD. ball-a
UMiami - BIO - bio1011
Chapter 48 - Test Bank: The Digestive SystemChapter 48Test Bank: The Digestive SystemMultiple Choice Questions1. Which of these animals has a gastrointestinal tract?A. spongeB. hydraC. flatwormD. earthwormE. salamanderBloom's Level: RememberFig
UMiami - BIO - bio1011
Chapter 49 - Test Bank: The Respiratory SystemChapter 49Test Bank: The Respiratory SystemMultiple Choice Questions1. Most of the primitive phyla of invertebrates obtain their oxygen by diffusion directlyfrom the surroundingA. air.B. water.C. mud.
UMiami - BIO - bio1011
Chapter 50 - Test Bank: The Circulatory SystemChapter 50Test Bank: The Circulatory SystemMultiple Choice Questions1. In a _ circulatory system, the circulating fluid, blood, is always enclosedwithin the blood vessels that transport blood away from an
UMiami - BIO - bio1011
Chapter 51 - Test Bank: Osmotic Regulation and the Urinary SystemChapter 51Test Bank: Osmotic Regulation and the Urinary SystemMultiple Choice Questions1. Nearly two-thirds of every vertebrate's body is composed of _.A. waterB. carbonC. bonesD. mu
UMiami - BIO - bio1011
Chapter 52 - Test Bank: The Immune SystemChapter 52Test Bank: The Immune SystemMultiple Choice Questions1. _ are phagocytes that circulate in the blood.A. B cellsB. macrophagesC. Plasma cellsD. T cellsE. MonocytesFigure: 52.03Section: 52.01Top
UMiami - BIO - bio1011
Chapter 53 - Test Bank: The Reproductive SystemChapter 53Test Bank: The Reproductive SystemMultiple Choice Questions1. _ reproduction is the primary means of reproduction among the protists, cnideria,and tunicates.A. AsexualB. SexualC. AmorphousD
UMiami - BIO - bio1011
Chapter 54 - Test Bank: Animal DevelopmentChapter 54Test Bank: Animal DevelopmentMultiple Choice Questions1. _ is the initial event in development.A. FertilizationB. CleavageC. GastrulationD. OrganogensisBloom's Level: RememberSection: 54.01Top
UMiami - BIO - bio1011
Chapter 55 - Test Bank: Behavioral BiologyChapter 55Test Bank: Behavioral BiologyMultiple Choice Questions1. The name of the study of behavior, behavioral genetics, and comparative psychology is_.A. ethologyB. demographyC. etiologyD. semanicsBlo
UMiami - BIO - bio1011
Chapter 56 - Test Bank: Population EcologyChapter 56Test Bank: Population EcologyMultiple Choice Questions1. Populations of endotherms that live in colder climates tend to have shorter ears and limbsthan populations of the same species in warm climat
UMiami - BIO - bio1011
Chapter 57 - Test Bank: Community of EcologyChapter 57Test Bank: Community of EcologyMultiple Choice Questions1. All organisms living together in a place are called a _.A. communityB. populationC. speciesD. ecosystemBloom's Level: RememberFigure
UMiami - BIO - bio1011
Chapter 58 - Test Bank: Dynamics of EcosystemsChapter 58Test Bank: Dynamics of EcosystemsMultiple Choice Questions1. A _ cycle is a cyclic path that involves both biological and chemicalprocesses of an ecosystem.A. biogeochemicalB. completeC. hydr
UMiami - BIO - bio1011
Chapter 59 - Test Bank: The BiosphereChapter 59Test Bank: The BiosphereMultiple Choice Questions1. As the global concentration of carbon dioxide increases, the world's temperature isrising, with great potential direct impact on the world's _.A. clim
UMiami - BIO - bio1011
Chapter 60 - Test Bank: Conservation BiologyChapter 60Test Bank: Conservation BiologyMultiple Choice Questions1. Scientists estimate that about _ of the world eukaryotic organisms have beendiscovered and given scientific names.A. 1%B. 5%C. 15%D.
TAFE NSW – Sydney Institute - CHEM - 101
TAFE NSW – Sydney Institute - CHEM - 101
TAFE NSW – Sydney Institute - CHEM - 101
TAFE NSW – Sydney Institute - CHEM - 101
TAFE NSW – Sydney Institute - CHEM - 101
TAFE NSW – Sydney Institute - CHEM - 101
TAFE NSW – Sydney Institute - CHEM - 101
TAFE NSW – Sydney Institute - CHEM - 101
TAFE NSW – Sydney Institute - CHEM - 101
TAFE NSW – Sydney Institute - CHEM - 101
Section ITotal Marks (75)Part ATotal marks (15)Attempt Questions 1-15Allow about 30 minutes for this partUse the multiple choice answer sheet.Select the alternative A, B, C or D that best answers the question. Fill in the response square completely
TAFE NSW – Sydney Institute - CHEM - 101
Section ITotal Marks (75)Part ATotal marks (15)Attempt Questions 1-15Allow about 30 minutes for this partUse the multiple choice answer sheet.Select the alternative A, B, C or D that best answers the question. Fill in the response square completely
TAFE NSW – Sydney Institute - CHEM - 101
Section ITotal Marks (75)Part ATotal marks (15)Attempt Questions 1-15Allow about 30 minutes for this partINSTRUCTIONSUse the multiple choice answer sheet on page 6.Select the alternative A, B, C or D that best answers the question. Fill in the res
TAFE NSW – Sydney Institute - CHEM - 101
Section ITotal Marks (75)Part ATotal marks (15)Attempt Questions 1-15Allow about 30 minutes for this partINSTRUCTIONSUse the multiple choice answer sheet below.Select the alternative A, B, C or D that best answers the question. Fill in the respons
TAFE NSW – Sydney Institute - CHEM - 101
Section ITotal Marks (75)Part ATotal marks (15)Attempt Questions 1-15Allow about 30 minutes for this partINSTRUCTIONSUse the multiple choice answer sheet on page 6.Select the alternative A, B, C or D that best answers the question. Fill in the res
TAFE NSW – Sydney Institute - CHEM - 101
Section ITotal Marks (75)Part ATotal marks (15)Attempt Questions 1-15Allow about 30 minutes for this partINSTRUCTIONSUse the multiple choice answer sheet below.Select the alternative A, B, C or D that best answers the question. Fill in the respons
TAFE NSW – Sydney Institute - CHEM - 101
TAFE NSW – Sydney Institute - CHEM - 101
TAFE NSW – Sydney Institute - CHEM - 101
TAFE NSW – Sydney Institute - CHEM - 101
TAFE NSW – Sydney Institute - CHEM - 101
Section ITotal Marks (75)Part ATotal marks (15)Attempt Questions 1-15Allow about 30 minutes for this partINSTRUCTIONSUse the multiple choice answer sheet on page 6.Select the alternative A, B, C or D that best answers the question. Fill in the res
TAFE NSW – Sydney Institute - CHEM - 101
Section ITotal Marks (75)Part ATotal marks (15)Attempt Questions 1-15Allow about 30 minutes for this partINSTRUCTIONSUse the multiple choice answer sheet on page 6.Select the alternative A, B, C or D that best answers the question. Fill in the res
TAFE NSW – Sydney Institute - CHEM - 101
Section ITotal Marks (75)Part ATotal marks (15)Attempt Questions 1-15Allow about 30 minutes for this partINSTRUCTIONSUse the multiple choice answer sheet on page 6.Select the alternative A, B, C or D that best answers the question. Fill in the res
TAFE NSW – Sydney Institute - CHEM - 101
Section ITotal Marks (75)Part ATotal marks (15)Attempt Questions 1-15Allow about 30 minutes for this partINSTRUCTIONSUse the multiple choice answer sheet on page 6.Select the alternative A, B, C or D that best answers the question. Fill in the res
TAFE NSW – Sydney Institute - CHEM - 101
Section ITotal Marks (75)Part ATotal marks (15)Attempt Questions 1-15Allow about 30 minutes for this partINSTRUCTIONSUse the multiple choice answer sheet on page 5JRAHS Chemistry Trial 2005page 1 of 211. When equal volumes of 0.10 mol L 1 HCl an
TAFE NSW – Sydney Institute - CHEM - 101
Section ITotal Marks (75)Part ATotal marks (15)Attempt Questions 1-15Allow about 30 minutes for this partINSTRUCTIONSUse the multiple choice answer sheet on page 5JRAHS Chemistry Trial 2005 ANSWERSpage 1 of 231. When equal volumes of 0.10 mol L
TAFE NSW – Sydney Institute - CHEM - 101
NSW INDEPENDENT TRIAL EXAMS 2006CHEMISTRY (PRELIMINARY EXAM)MARKING GUIDELINESSection I1C2D3A4D5B6C7B8C9B10B11A12D13A14B15CSection IIQuestion 16(a)CriteriaS: 2, 8, 6.Marks1Question 16(b)CriteriaSodium forms ionic
TAFE NSW – Sydney Institute - CHEM - 101
Centre NumberStudent NumberCATHOLIC SECONDARY SCHOOLSASSOCIATION OF NEW SOUTH WALES2006TRIAL HIGHER SCHOOL CERTIFICATEEXAMINATIONChemistryAfternoon SessionFriday 4 August 2006Total marks 100Section IGeneral Instructions Reading time 5 minutes
TAFE NSW – Sydney Institute - CHEM - 101
CATHOLIC SECONDARY SCHOOLS ASSOCIATION2006 TRIAL HIGHER SCHOOL CERTIFICATE EXAMINATIONCHEMISTRY MARKING GUIDELINESThe sample answers indicate features that should be found in a response that receives full marks.For the extended response questions, a s
TAFE NSW – Sydney Institute - CHEM - 101
Section I75 marksPart A 15 marksAttempt Questions 1-15Allow about 30 minutes for this partUse the multiple choice answer sheet on page 7_2006 JRAHS Chemistry Trial ExaminationPage 1 of 211.Consider the following reactions:(i)Ag+ + Cl-(ii)CH4