CHM 1046

Test #1

Chang: chapters 11 and 12

 

  1. Which of the following compounds is a solid at room temperature?

    2. a. CF4 b. CS2 c. C2H6 d. LiF e. CCl4

     

  2. Which of the following compounds is not a solid at room temperature?

    3. a. C3H8 b. SrBr2 c. SrS d. LiF e. MgBr2

     

  3. Which of the following solids is held together primarily by network covalent bonding?

    4. a. NaNO3 b. SrS c. ice (H2O) d. MgCl2 e. SiO2

     

  4. Which of the following solids is not held together by ionic bonding? 

    5. a. Al2O3 b. CaO c. NH4NO3 d. NH4Cl e. Mg

      

  5. Which of the following solids is held together primarily by intermolecular forces?

    6. a. Na b. C10H8 c. LiCl d. CsI e. SiC

     

  6. Which of the following would be expected to have the highest boiling point?

    7. a. F2 b. Cl2 c. Br2 d. I2

     

  7. Which of the following would be expected to have the highest boiling point?
    a. HF b. HCl c. HBr d. HI

 

  1. Which of the following compounds would be expected to have the lowest London (dispersion) force?

    2. a.H2O b. H2S c. H2Se d. H2Te

     

  2. Which of the following would be expected to have the highest boiling point?

    3. a.H2O b. Li2O c. H2Se d. H2Te

     

  3. Which of the following would be expected to have the highest boiling point?

    4. a.CH3OCH3 b. CH3CH2OH c. CH3CH3 d. CH3CH2CH3

     

  4. Which of the following liquids has the strongest intermolecular forces?

a. ethanol bp 78° C

b. diethyl ether bp 35° C

c. methanol bp 65° C

d. octane bp 126° C

12. The heat capacity for liquid water is 4.18 J/g° C and the heat of vaporization is 40.7kJ/mole. How many kJ of heat must be provided to convert 20 g of liquid water at 10° C into 20 g of steam at 100° C?

  1. 53 b. 45 c. 72 d. 2.4 e. 31

 

13. Which of these represents a hydrogen bond?

 

14. What kind of attractive forces must be overcome in order to melt ice?

  1. covalent bonds
  2. dispersion forces
  3. hydrogen bonds
  4. both dispersion forces and hydrogen bonds

15. A solid has a very high melting point and as a liquid does not conduct electricity. The solid is

    a. molecular b. metallic c. ionic d. covalent network

 

16. Which of the following is most soluble in water? 

  1. C
  2. CH3CH2CH2CH2CH2CH2OH
  3. CH3OH
  4. CH4
  5. Cu

 

17. Which of the following solvents would be best for dissolving gasoline? 

  1. H2O b. NH3(l) c. C6H6 d. CH3OH

 

 

18. On the phase diagram B is

a. the gas state b. the liquid state c. the triple point d. the normal boiling point e. the critical point

 

19.E is

  1. the solid state
  2. the liquid state
  3. the triple point
  4. the normal boiling point
  5. the critical point

20.D is

  1. the gas state
  2. the liquid state
  3. the triple point
  4. the normal boiling point
  5. the critical point

21.The normal boiling point is

  1. 70° b. 100° c. 130° d. 180° e. 207°

22. When the external pressure is 2.0 atm the boiling point is

    a. 70° b. 100° c. 130° d. 180° e. 207

23. On going from 3.0 atm and 75° C to 0.4 atm and 75° substance first _______ and then _______.

  1. condenses, freezes
  2. melts, boils
  3. freezes, sublimes
  4. sublimes, condenses
  5. remains a solid

24. Which of the following solvents would be best for dissolving Cu(NO3)2?

  1. H2O b. CS2 c. ether d. C6H6

25. What is the mole fraction of C2H5OH (FM = 46.1) in a solution containing 200 g of C2H5OH and 100 g of water?

    a. 0.250 b. 0.213 c. 0.281 d. 0.438 e. 0.667

 

 

 

 

26. What is the molarity of 82.6% HNO3 (FM = 63.0) that has a density of 1.51 g/mL.

a. 13.1 b. 19.8 c. 12.0 d. 4.2 e. 7.1

 

 

 

 

27. Assume 9.62 g of BaCl2 (FM = 208) are dissolved per liter of solution. What is the molarity of chloride ions?

  1. 0.0463 b. 0.0925 c. 0.139 d. 0.185

 

 

 

 

28. How is the solubility of CO2(g) in water affected by a increase in temperature?

    a. increase b. decrease c. no change

 

29. Which has the lowest freezing point?

a. pure H2O   b. 0.15 m AlCl3  c. 0.15 m CaCl2      d. 0.15 m CH3COOH    e. 0.15 m CH3OH

30. What is the molecular weight of an unknown compound, Z, if 1.63 g of Z dissolved in 20.2 g of benzene causes the freezing point to be reduced to 3.91° C?

For benzene, F.P. = 5.50° C and Kf = 4.90 ° C/m.

  1. 150 b. 130 c. 250 d. 74 e. 44

 

31. When sucrose is added to water the vapor pressure _____, the freezing point _____, and the boiling point ______.

    a. increases, increases, increases

    b. decreases, decreases, decreases

    c. increases, decreases, increases

    d. decreases, increases, increases

    e. decreases, decreases, increases

 

32. If the intermolecular forces in a liquid increase, the vapor pressure

    a. increases b. decreases c. does not change

 

33. If the surface area of a liquid increases, the equilibrium vapor pressure 

        a. increases b. decreases c. does not change

34. What is the main attractive force that must be overcome in order to melt aluminum metal?

a. dispersion force b. hydrogen bond c. covalent bond

d. dipole-dipole force e. metallic bond

 

35. What is the main attractive force that must be overcome in order to dissociate N2 into N atoms?

a. dispersion force b. hydrogen bond c. covalent bond

d. dipole-dipole force e. metallic bond

 

36. What is the major force between C2H5OH and H2O when they form a solution?

a. H-bond b. dipole-dipole c. dispersion d. covalent e. ion-dipole

37. A solution of 0.0727 g of a hormone in 100.0 mL of aqueous solution has an osmotic pressure of 12.6 mmHg at 22° C. What is the molecular mass of the hormone?

a. 77.7 b. 106 c. 943 d. 1060 e. 2.32 x 105

 

 

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