Quiz: Can You Solve The Chemistry Exam Test?

27 Questions

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Quiz: Can You Solve The Chemistry Exam Test?

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Questions and Answers
  • 1. 
    Helium atoms do not combine to form He2 molecules, yet He atoms do attract one another weakly through?
    • A. 

      Dispersion forces

    • B. 

      Ion-dipole forces

    • C. 

      Dipole-dipole forces

    • D. 

      Hydrogen bonding

  • 2. 
    Which one of the following substances should exhibit hydrogen bonding in the liquid state?
    • A. 

      H2

    • B. 

      He

    • C. 

      H2S

    • D. 

      H2O

  • 3. 
    In which one of the following substances will the individual molecules experience both London forces and dipole-dipole forces?
    • A. 

      BCL3

    • B. 

      HCl

    • C. 

      Br2

    • D. 

      CO2

  • 4. 
    Which of the following substances should have the highest boiling point?
    • A. 

      CH4

    • B. 

      Cl 2

    • C. 

      N2

    • D. 

      CH3OH

  • 5. 
    Which of the following liquids should have the highest viscosity at the same temperature?
    • A. 

      CH3OCH3

    • B. 

      CH3Cl2

    • C. 

      HOCH2CH2OH

    • D. 

      CH3Br

  • 6. 
    Which of the following substances would be expected to have the lowest vapor pressure at room temperature?
    • A. 

      Ethanol bp=78 degrees celsius

    • B. 

      Methanol bp=65 degrees celsius

    • C. 

      Water bp=100 degrees celsius

    • D. 

      Acetone bp=56 degrees celsius

  • 7. 
    Which one of the following substances should exhibit hydrogen bonding in the liquid state?
    • A. 

      CH3COOH

    • B. 

      CH4

    • C. 

      PH3

    • D. 

      He

  • 8. 
    The lattice points in a crystal lattice may be occupied by?
    • A. 

      Ions

    • B. 

      Neutral atoms

    • C. 

      Neutral molecules

    • D. 

      Any of the above

  • 9. 
    Platinum has a face-centered cubic crystal structure with a unit cell length of 392pm. What is the radius of the platinum atom?
    • A. 

      69pm

    • B. 

      98pm

    • C. 

      277pm

    • D. 

      139pm

  • 10. 
    The vapor pressure of a liquid in a closed container depends upon?
    • A. 

      The amound of liquid

    • B. 

      The surface area of the liquid

    • C. 

      The volume of the container

    • D. 

      The temperature

  • 11. 
    Which one of the following would be immiscible with water?
    • A. 

      S=C=S

    • B. 

      C2H5OH

    • C. 

      CH3OH

    • D. 

      NH3

  • 12. 
    Calculate the amount of heat needed to melt 2.0 kg of iron at its melting point (1809K) given that? delta Hfus=133.80kJ/mol.
    • A. 

      494 kJ

    • B. 

      27.6 kJ

    • C. 

      25,000 kJ

    • D. 

      27,600 kJ

  • 13. 
    Which of the following compounds will be soluble in CCl4?
    • A. 

      NaCl

    • B. 

      H2O

    • C. 

      C8H18

    • D. 

      NaOH

  • 14. 
    Which of the following usually represents the strongest type of intermolecular force?
    • A. 

      Ion-dipole

    • B. 

      H-bonds

    • C. 

      Dispersion

    • D. 

      Dipole-dipole

  • 15. 
    What is the percent CdSO4 by mass in a 1.0 molal aqueous solution (MW of CdSO4 =208.46 g/mol)?
    • A. 

      0.10%

    • B. 

      17.2%

    • C. 

      20.8%

    • D. 

      24.4%

  • 16. 
    • A. 

      15.2%

    • B. 

      1.51%

    • C. 

      7.57%

    • D. 

      13.3%

  • 17. 
    Calculate the molality of a solution containing 14.3 g of NaCl in 42.2 g of water.
    • A. 

      2.45 x 10-4 m

    • B. 

      5.80 x 10-4 m

    • C. 

      2.45 x 10-1 m

    • D. 

      5.79 m

  • 18. 
    Which of the following solution would have the highest boiling point?
    • A. 

      0.1 m glucose in water

    • B. 

      0.1m glycerol in water

    • C. 

      0.1m NaCl in water

    • D. 

      Pure water

  • 19. 
    What is the approximate Na+ ion concentration in a 0.75 M Na2CO3 solution? Na2CO3 is a salt which will fully dissociate
    • A. 

      1.50M

    • B. 

      0.375 M

    • C. 

      0.75M

    • D. 

      1.25M

  • 20. 
    Calculate the mole fraction of CH3CH2OH ethanol(molar mass=46.0 g/mol), in a solution that contains 46g of ethanol and 64g of CH3OH.
    • A. 

      0.33

    • B. 

      0.42

    • C. 

      0.50

    • D. 

      0.67

  • 21. 
    As a non-volatile solute is added to a pure solvent, which of the following statements is true?
    • A. 

      As the solute is added, the boiling point will decrease and the freezing point will increase

    • B. 

      As the solute is added, the boiling point will increase and the freezing point will decrease

    • C. 

      As the solute is added, both the boiling point and the freezing point will decrease

    • D. 

      As the solute is added, both the boiling point and the freezing point will increase

  • 22. 
    Calculate the amount of heat theat must be absorbed by 10.0 g of ice at -20 degrees C to convert it to liquid water at 60.0 degrees C. Given: Specific heat (ice)=2.1 J/g degrees C Specific heat (water) =4.18 J/g degrees C delta Hfus=6.0 kJ/mol
    • A. 

      6.112 kJ or 6,112 J

    • B. 

      6.26 kJ or 6,261 J

    • C. 

      5.26 kJ or 5,260 J

    • D. 

      4.36 kJ or 4,360 J

  • 23. 
    The vapor pressure of ethanol is 400 mmHg at 63.5 degrees C. Its molar heat of vaporization is 39.3 kJ/mol. What is the vapor pressure of ethanol in mmHg at 34.9 degrees C? The gas constant R, equals 8.314 J/mol*K
    • A. 

      P2=105.5 mmHg

    • B. 

      P2=103.5 mmHg

    • C. 

      P2=108.5 mmHg

    • D. 

      P2=117.2 mmHg

  • 24. 
    Acetic acid has a heat of fusion of 10.8 kJ/mol and a heat of vaporization of 24.3 kJ/mol. What is the expected value of the heat of sublimation of acetic acid?
    • A. 

      22.1 kJ/mol

    • B. 

      32.1 kJ/mol

    • C. 

      35.1 kJ/mol

    • D. 

      40.1 kJ/mol

  • 25. 
    What is the molarity of a solution that is 22.3 % by mass sulfuric acid (H2SO4,MW 98.08 g/mol) and that has a density of 1.136 g/mL?
    • A. 

      1.23 mol/L

    • B. 

      1.55 mol/L

    • C. 

      2.58 mol/L

    • D. 

      2.254 mol/L

  • 26. 
    What is the freezing point of a solution that contains 162.0 g of glucose (C6H12O6,MW=182.0 g/mol) in 500g of H2O? Kf=1.86 degrees C/O
    • A. 

      -2.21 degrees C

    • B. 

      3.31 degrees C

    • C. 

      -3.31 degrees C

    • D. 

      -1.12 degrees C

  • 27. 
    Which of the following characteristics indicates the presence of strong intermolecular forces in a liquid?
    • A. 

      A high heat of vaporization

    • B. 

      A high vapor pressure

    • C. 

      A low critical temperature

    • D. 

      A high boiling point