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Exam 1
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Questions in this quiz (32)
1Choose the statement below that is TRUE.
- AA solution will form between two substances if the solute-solvent interactions are of comparable strength to the solute-solute and solvent-solvent interactions.
- BA solution will form between two substances if the solute-solvent interactions are small enough to be overcome by the solute-solute and solvent-solvent interactions.
- CA solution will form between two substances if the solute-solute interactions are strong enough to overcome the solvent-solvent interactions.
- DA solution will form between two substances only if the solvent-solvent interactions are weak enough to overcome the solute-solvent interactions.
- ENone of the above are true.
2Which enthalpies are always positive?
- A△H solute & △H solvent
- B△H solute & △H solute
- C△H solvent & △H solvent
- DNone of the above
3Which of the following compounds will be most soluble in ethanol (CH3CH2OH)?
- Atrimethylamine (N(CH3)3)
- Bacetone (CH3COCH3)
- Cethylene glycol (HOCH2CH2OH)
- Dhexane (CH3CH2CH2CH2CH2CH3)
- ENone of these compounds should be soluble in ethanol.
4Which of the following statements is TRUE?
- AIn general, the solubility of a solid in water decreases with increasing temperature.
- BIn general, the solubility of a gas in water decreases with increasing temperature.
- CThe solubility of a gas in water usually increases with decreasing pressure.
- DThe solubility of an ionic solid in water decreases with increasing temperature.
- ENone of the above statements are true.
5Determine the Henry's law constant for ammonia in water at 25°C if an ammonia pressure of 0.022 atm produces a solution with a concentration of 1.3 M.
- A59 M/atm
- B0.017 M/atm
- C0.029 M/atm
- D35 M/atm
- E0.038 M/atm
6A sealed container contains 0.352 L of water with an atmosphere of oxygen gas. What is the concentration of O2 in the water if the external pressure is 4.24 atm given that kH for O2 is 1.66 × 10-6 M/mm Hg at this temperature?
- A5.34 × 10-3 M
- B1.53 × 10-3 M
- C9.46 × 10-2 M
- D5.34 × 10-2 M
- E3.82 × 10-4 M
7Which of the following concentration units are temperature dependent?
- Amole fraction
- Bmolality
- Cmass percent
- Dmolarity
- Enone of the above
8What mass (in g) of NH3 must be dissolved in 475 g of methanol to make a 0.250 m solution?
- A2.02 g
- B4.94 g
- C1.19 g
- D8.42 g
- E1.90 g
9A solution is prepared by dissolving 98.6 g of NaCl in enough water to form 875 mL of solution. Calculate the mass % of the solution if the density of the solution is 1.06 g/mL.
- A11.3%
- B12.7%
- C9.4%
- D10.6%
- E11.9%
10A solution is prepared by dissolving 1.928 g of KNO3 into enough water to make 651 mL. What is the molarity of the solution?
- A0.159 M
- B0.381 M
- C0.0293 M
- D2.48 M
- E0.0832
11A solution is prepared by dissolving 38.6 g sucrose (C12H22O11) in 495 g of water. Determine the mole fraction of sucrose if the final volume of the solution is 508 mL.
- A4.09 × 10^-3
- B7.80 × 10^-2
- C1.28 × 10^-3
- D7.23 × 10^-2
- E2.45 × 10^-3
12A solution is prepared by dissolving 76.3 g NaI in 545 g of water. Determine the mole fraction of NaI if the final volume of the solution is 576 mL.
- A6.04 × 10^-3
- B1.65 × 10^-2
- C1.40 × 10^-3
- D1.32 × 10^-2
- E8.84 × 10^-2
13Calculate the freezing point of a solution of 500.0 g of ethylene glycol (C2H6O2) dissolved in 500.0 g of water. Kf = 1.86°C/m and Kb = 0.512°C/m.
- A30.0°C
- B-30.0°C
- C8.32°C
- D-8.32°C
- E70.2°C
14Calculate the boiling point of a solution of 500.0 g of ethylene glycol (C2H6O2) dissolved in 500.0 g of water. Kf = 1.86°C/m and Kb = 0.512°C/m. Use 100°C as the boiling point of water.
- A108°C
- B92°C
- C130°C
- D70°C
- E8.3°C
15The vapor pressure of a solution is always ______ that of the pure solvent
- Aequal to
- Btwice
- Cone half
- Dhigher than
- Elower than
16Give the reason that antifreeze is added to a car radiator.
- AThe freezing point is lowered and the boiling point is elevated.
- BThe freezing point is elevated and the boiling point is lowered.
- CThe freezing point and the boiling point are elevated.
- DThe freezing point and the boiling point are lowered.
- ENone of the above.
17Dynamic equilibrium can be defined as:
- Arate of dissolution = rate of deposition.
- Brate of dissolution < rate of deposition.
- Crate of dissolution > rate of deposition.
- Drate of bubbling > rate of dissolving
- Erate of condensing > rate of bubbling
18Place the following solutions in order of increasing osmotic pressure.
I. 0.15 M C2H6O2 II. 0.15 M BaCl2 III. 0.15 M Na I- AIII < I < II
- BII < III < I
- CI < II < III
- DII < I < III
- EI < III < II
19Identify the solute with the lowest van't Hoff factor.
- Anonelectrolyte
- BK I
- CMgSO4
- DAlCl3
20Which of the following statements is TRUE?
- AVapor pressure increases with temperature.
- BHydrogen bonds are stronger than covalent bonds.
- CIntermolecular forces hold the atoms in molecules together.
- DDispersion forces are generally stronger than dipole-dipole forces.
- ENone of the above are true.
21Which of the following statements is FALSE?
- AThe rate of vaporization increases with increasing surface area.
- BThe rate of vaporization increases with decreasing strength of intermolecular forces.
- CThe rate of vaporization increases with increasing temperature.
- DMolecules with hydrogen bonding are more volatile than compounds with dipole-dipole forces.
- ENone of the above are false.
22Which of the following substances would you predict to have the highest ΔHvap?
- AXe
- BC6H6
- CSiF4
- DF2
- EN2
23Which of the following substances would you predict to have the highest ΔHvap?
- ACH3Cl
- BHCl
- CHOCH2CH2OH
- DCH3CH2OH
- ECH3CH2CH2CH3
24Why is water an extraordinary substance?
- AWater has a low molar mass, yet it is a liquid at room temperature.
- BWater is the main solvent within living organisms.
- CWater has an exceptionally high specific heat capacity.
- DWater has strong hydrogen bonding.
- EAll of the above
25What happens when the vapor pressure of a liquid is equal to the external pressure?
- AAn equilibrium exists between the liquid and the solid state.
- BThe liquid freezes.
- CThe intermolecular forces become stronger in the liquid.
- DThe liquid boils.
- EDispersion forces become weaker in the liquid.
26Which of the following must be overcome during the boiling of acetonitrile, CH3CN?
1. dispersion forces
2. dipole-dipole forces
3. hydrogen bonds- A1 only
- B2 only
- C1 and 2
- D1 and 3
- E1, 2, and 3
27Which of the following substances should have the highest melting point?
- ACO2
- BSrS
- CKr
- DF2
- EMgO
28Which of the following substances should have the highest melting point?
- AFe
- BNe
- CXe
- DN2
- ECO
29Identify the place which has the highest boiling point of water.
- ADeath Valley, 282 feet below sea level
- Ba pressurized passenger jet, 35,000 feet
- CNew Orleans, sea level
- DMt. Everest, 29035 feet
- EDenver, Colorado, 5280 feet
30Choose the substance with the highest viscosity.
- Awater at 10°C
- Bwater at 20°C
- Cwater at 30°C
- Dwater at 40°C
- Ewater at 50°C
31List the compounds in decreasing boiling point order.
CH3CH2CH3 Ar CH3CN- ACH3CH2CH3 > CH3CN > Ar
- BAr > CH3CH2CH3 > CH3CN
- CCH3CH2CH3 > Ar > CH3CN
- DCH3CN > CH3CH2CH3 > Ar
- EAr > CH3CN > CH3CH2CH3
32Consider the phase diagram below. If the dashed line at 1 atm of pressure is followed from 100 to 500°C, what phase changes will occur (in order of increasing temperature)?
- Acondensation, followed by vaporization
- Bsublimation, followed by deposition
- Cvaporization, followed by deposition
- Dfusion, followed by vaporization
- ENo phase change will occur under the conditions specified.
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- Quiz on Exam 1, created by Aly McLean on 29/01/2019.
- Author
- Aly McLean
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- English
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