Chemistry Chap 10 set
1. The vapor pressure of ethanol is 400 mmHg at 63.5°C. Its molar heat of vaporization is 39.3 kJ/mol. What is vapor pressure of ethanol, in mmHg, at 34.9°C (R = 8.314 J/K∙mol).
108.5mmHg
The molar enthalpy of vaporization of hexane (C6H14) is 28.9 kJ/mol, and its normal boiling point is 68.73°C at 760 mmHg. What is the vapor pressure of hexane at 25°C (R = 8.314 J/K∙mol)
170.8mmHg
The following data was determined experimentally and plotted. Determine the molar heat of vaporization of chlorine based on the dat given and plotted. R= 8.314 J/mol y= -2634.1x + 17.661
21890 J/mol
Arterial blood contains about 0.25 g of oxygen per liter at 37°C and standard atmospheric pressure. What is the Henry's law constant [mole/(Lxatm)] for O2 dissolution in blood? The mole fraction of O2 in air is 0.209. (Hint: use the mole fraction to calculate the partial pressure of oxygen and then solve for Henry's Law constant.
3.7 x 10^-2mol/(Lxatm)
Find the temperature at which ethanol boils on a day in the mountains when the barometric pressure is 547 mmHg. (Given: The heat of vaporization of ethanol is 39.3 kJ/mol; the normal boiling of ethanol is 78.3°C (R = 8.314 J/K∙mol).)
342.9K
The solubility of O2 in water is 6.5mg/L at an atmospheric pressure of 1 atm and temperature of 40C. Calc the Henry's law constant of O2 at 40C in units of mol/(Lxatm). Mole fraction of O2 in air is 0.209
9.72 x 10^-4 mol/(Lxatm)
Which of the following compounds, CO2, NO2, SO2, or H2S, is expected have the weakest interactions between its molecules?
CO2 has linear geometry and is a non-polar molecule. Therefore, the only type of intermolecular forces present are dispersion forces and CO2 has the weakest interaction of them all.
Can ice be melted merely by applying pressure? Explain your answer
Ice can be melted by applying pressure because, If we look at the phase diagram of water, the solid-liquid line has a negative slope, which means as the pressure is increased (x-axis) the melting point/temperature (y-axis) decreases.
Explain the difference between sublimation and evaporation
Sublimation is the process of a solid directly evaporating into gas, in which the liquid phase is skipped. Evaporation is the process of a liquid evaporating into a gas
Explain how the solid-liquid line in the phase diagram of water differ in character from the solid-liquid line in the phase diagrams of most other substances, such as CO2.
The solid-liquid line for the phase diagram of water has a negative slope, whereas for most other substances, such as CO2, have positive slopes. The negative slope of the solid-liquid line for water indicates that as pressure is increased, the melting point is decreased. With the increase pressure, the higher density phase is favored, which is the liquid phase for water. For most other substances, the higher density phase is a solid. But remember that the solid phase for water is less dense because of the crystal, lattice hydrogen-bonding network formed.
In hydrogen iodide, ____________are the most important intermolecular forces. a. Dipole-dipole forces b. London dispersion forces c. Hydrogen bonding d. Covalent bonds e. Polar covalent bonds
a
What name is given to a quantitative measure of the elastic force in the surface of a liquid? a. Surface tension b. Adhesion c. Polarity d. Capillary action e. Cohesion
a
Which one of the following substances will have both dispersion forces and dipole-dipole forces? a. HCl b. CH3CH2CH3 c. Br2 d. H2 e. CO2
a
for which of the following species are the intermolecular interactions entirely due to dispersion forces a C2H6 b CH3OCH3 c NO2 d H2S e CaNO3
a
which of the following atoms does not participate in hydrogen bonding a S b O c N d F
a
The strongest intermolecular interactions between pentane (C5H12) molecules arise from a. Dipole-dipole forces b. London dispersion forces c. Hydrogen bonding d. Ion-dipole interactions e. Carbon-carbon bonds
b
What type of intermolecular forces exist between hydrogen fluoride molecules? I. London forces II. Dipole-dipole interactions III. Hydrogen bonding IV. Ion-dipole interactions a. II and III b. I, II, and III c. I only d. III only e. I and III
b
Which of the following is defined as the attractive forces between polar molecules? I. Dispersion forces II. Dipole-dipole interactions III. Hydrogen Bonding a. I and III b. II only c. III only d. I, II, and III e. I only
b
1. The strongest intermolecular interactions between ethyl alcohol (CH3CH2OH) molecules arise from a. Dipole-dipole forces b. London dispersion forces c. Hydrogen bonding d. Ion-dipole interactions Carbon-oxygen bonds
c
1. Which of the following involves hydrogen bonding? a. CH4 b. H2C=CH2 c. H2O d. CHCl3 e. CHF3
c
Ammonia's unusually high melting point is the result of a. Dipole-dipole forces b. London dispersion forces c. Hydrogen bonding d. Covalent bonding e. Ionic bonding
c
What is the name given to the attractive forces that hold particles together in the condensed phase? a. Ionic bonds b. Covalent bonds c. Intermolecular forces d. Electronegativity Electron attraction
c
Which of the following properties indicates the presence of strong intermolecular forces in a liquid? a. A low heat of vaporization b. A low critical temperature c. A low vapor pressure d. A low boiling point e. None of the above
c
Which of the following terms refers to the resistance of a liquid to flow? a. Surface tension b. Capillary action c. Viscosity d. Adhesion e. Cohesion
c
what is the intermolecular force that exists between a calcium ion and water a. dipole dipole b london dispersion c ion dipole d covanlent bonding e ion ion
c
1. The vapor pressure is a property of liquids that depends on which of the following? a. A constant atmospheric pressure b. A distinct temperature c. A constant volume d. The viscosity e. Magnitude of intermolecular forces
e
Which of the following factors can contribute to the viscosity for a liquid? a. Temperature b. Hydrogen bonding c. Molecular entanglements (branching) d. London forces e. All of the answers are correct
e
Which of the following substances should exhibit hydrogen bonding in the liquid state? a. PH3 b. He c. H2S d. CH4 e. CH3OH
e
which of the following molecules are the dispersion forces strongest a C4H10 b C5H12 c C6H14 d C7H16 e C8H18
e
