Quiz: Can You Solve The Chemistry Exam Test?
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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
Questions: 10 | Attempts: 40293 | Last updated: Aug 26, 2021
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