Term
| The Clausius-Clapeyron equation applies to |
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Definition
| The liquid gas line of a pressure-temperature phase diagram. |
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Term
Which of the following has the listed intermolecular interactions arranged from
smallest interaction energy to largest interaction energy? |
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Definition
| Dipole-induced dipole < dipole-dipole |
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Term
| The dominant intermolecular interaction between molecules of CO2 is |
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Definition
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Term
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Definition
A condition in which two opposing processes simultaneously
occur at equal rates. |
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Term
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Definition
| The equilibrium pressure of vapor above the surface of a liquid at a specified temperature. |
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Term
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Definition
| The amount of heat needed to increase the temperature of 1 gram of material by 1°C. |
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Term
| Provide the relationship between boiling point and strength of intermolecular interactions |
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Definition
The boiling point of a liquid increases as the strength of the intermolecular interactions
between liquid phase molecules increases. |
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Term
| Describe the significance of a line in a pressure-temperature phase diagram |
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Definition
A line of a pressure-temperature phase diagram corresponds to temperatures and
pressures at which the two phases on either side of the line are in equilibrium. |
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Term
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Definition
Molarity(M) =
mole solute/liter solution |
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Term
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Definition
molality (m) =
mole solute/kilogram solvent |
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Term
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Definition
parts per million (ppm) =
mass of component/mass sample *106 |
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Term
| The term fluid is used to describe which of the phases of matter? |
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Definition
| The liquid and gas phases. |
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Term
| Describe the slope of the liquid/gas line and how this is related to the temperature dependence of vapor pressure. |
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Definition
The slope of the liquid/gas line is always positive, thus indicating the vapor pressure of all
liquids incresases as the temperature increases. |
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Term
Based on intermolecular interactions, arrange the following from lowest to highest
vapor pressure (vp).
HF, CH4, Br2, PH3, HO-CH2-CH2-OH (ethylene glycol) |
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Definition
Low vp High vp
HO-CH2-CH2-OH HF PH3 Br2 CH4
Vapor pressure increases as the strength of the intermolecular interaction between liquid phase molecules
decreases.
HF Hydrogen bond (strong dipole-dipole) interaction
HO-CH2-CH2-OH Hydrogen bond
Each HF molecule has one hydrogen bonding site, while each HO-CH2-CH2-OH molecule has two sites,
therefore the hydrogen bond interaction of HO-CH2-CH2-OH is stronger than HF.
CH4 Dispersion interaction
Br2 Dispersion interaction
Based on mass, the Br2 dispersion interaction is stronger than the CH4 dispersion interaction.
PH3 dipole-dipole interaction (there is a lone pair of electrons on the central atom) |
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Term
Identify the dominant intermolecular interaction associated with each of the
following pure substances. |
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Definition
BF3 Dispersion interaction. BF3 is a nonpolar molecule (all things bonded to the
central atom are identical and there are no lone pairs on the central atom).
CO Dipole-dipole interaction. CO is a polar molecule.
H2O Hydrogen bond interaction.
NaCl Ion–ion interaction. NaCl is an ionic compound. |
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Term
At 34.1°C the vapor pressure of water is 40.1 torr. What is the vapor pressure of
water at 85.5°C? ΔHvap of water is 40.7 kJ/mol.
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Definition
P2= inv ln(5.976862157)= 394.2 torr
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Term
Determine the amount of heat needed to convert 25.0 grams of liquid benzene
(C6H6) at 22°C to gas phase benzene at 80.1°C. The boiling point of benzene is 80.1°C,
c benzene liquid = 1.74 J/g °, ΔHvap |
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Definition
| Heat require = step 1 + step 2 = 2527.35 J + 10850 J = 13377 J = 13.377 kJ |
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