Quiz: Can You Solve The Chemistry Exam Test?

27 Questions | By Clynnbass | Last updated: Mar 21, 2022 | Total Attempts: 1285

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Quiz: Can You Solve The Chemistry Exam Test? - Quiz

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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.

Calculate the percent by mass of potassium nitrate in a solution made from 45.0g KNO3 and 295 mL of water. Density of water is 0.997 g/mL.
- 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