Intermolecular Forces
Unit Cell
Gas Laws
Thermodynamics
100
Select all species capable of hydrogen bonding among themselves:
a. C2H6
b. NH3
c. HI
d. KF
e. CH3COOH
b. NH3 and e. CH3COOH
100
If a cubic unit cell of an ionic compound has M cations at the corners and X anions in the centers of the edges, what is the formula unit (or empirical formula) of the compound?
a. M2X3
b. M2X
c. M3X
d. MX3
e. MX2
d. MX3
100
The valve between a 5.0L tank containing a gas at 9 atm and a 10.0L tank containing a gas at 6 atm is opened at constant temperature. Calculate the final pressure of the tanks.
a. 7 atm
b. 3 atm
c. 4 atm
d. 15 atm
e. None of these
a. 7 atm
100
A battery does 35 KJ of work (driving an electric motor) and 7 KJ of heat are released. What is the change in internal energy of the system?
a. -42 KJ
b. -35 KJ
c. +42 KJ
d. +28 KJ
e. -28 KJ
a. -42 KJ
200
What are all of the intermolecular forces that must be overcome in converting liquid CH3OCH3 to a gas?
a. London dispersion forces, hydrogen bonding, and dipole-dipole forces
b. London dispersion forces
c. London dispersion forces and hydrogen bonding
d. Dipole-dipole forces
e. Dipole -dipole forces and London dispersion forces
e. Dipole -dipole forces and London dispersion forces
200
4
200
The empirical formula of a gas is CH3O. If 2.77 g of the gas occupies 1.00 L at exactly 0°C at a pressure of 760 torr, what is the molecular formula of the gas?
a. CH3O
b. C5H15O5
c. C3H9O3
d. C4H12O4
e. C2H6O2
e. C2H6O2
200
Which molecules of the following gasses will have the greatest average kinetic energy?
a. H2 at 0.5 atm and 298K
b. N2 at 1 atm and 298K
c. CO2 at 1 atm and 298K
d. CO at 0.1 atm and 298K
e. All the molecules have the same kinetic energy
e. All the molecules have the same kinetic energy
300
Arrange the following compounds in order of increasing boiling point: RbF, CO2, CH3OH, CH3Br.
CO2<CH3Br<CH3OH<RbF
300
a. 0.621 g*cm^-3
b. 0.115 g*cm^-3
c. 2.19 g*cm^-3
d. 1.50 g*cm^-3
e. 2.41 g*cm^-3
e. 2.41 g*cm^-3
300
When ammonium nitrate [NH4NO3(s)\ is heated it decomposes to form N2O(g) and H2O(g). A sample of ammonium nitrate was decomposed in an evacuated reaction vessel and the measured gas pressure was 900 torr. What is the partial pressure of H2O(g)?
a. 900 torr
b. 600 torr
c. 675 torr
d. 450 torr
e. 300 torr
b. 600 torr
300
Gaseous ethylene oxide (C2H4O) reacts according to the balanced equation shown below. If a total of 7650 kJ of heat is produced in a reaction, how many mols of C2H4O are consumed?
2C2H4O(g) + 5O2(g) —> 4CO2(g) + 4H2O(l) ΔH = -2528.0 kJ/mol
a. 6.05 mols
b. 3.03 mols
c. 0.330 mols
d. 2.00 mols
e. 0.661 mols
a. 6.05 mols
400
Which of the following statements is true?
a. CCl4 has a higher boiling point than CBr4
b. Isobutane, (CH3)3CH, has a higher boiling point than n-butane, CH3CH2CH2CH3
c. I2 has a lower boiling point than Br2
d. N-propane, CH3CH2CH3, has a higher boiling point than n-pentane, CH3CH2CH2CH2CH3
e. CBr3H has a higher boiling point than CCl3H
e. CBr3H has a higher boiling point than CCl3H
400
Aluminum crystallizes with a face-centered cubic unit cell. The radius of an aluminum atom is 143 pm. Calculate the density of solid crystalline aluminum in g/cm3
d= 2.708 g/cm3
400
A mixture of oxygen gas and helium gas is 92.3% by mass oxygen. What is the partial pressure of the oxygen gas if the total pressure is 745 torr?
a. 333 torr
b. 299 torr
c. 412 torr
d. 447 torr
e. 688 torr
d. 447 torr
400
Determine the value of 𝚫Gº for the combustion reaction of acetylene at room temperature:
C2H2(g) + 5/2 O2(g) → 2CO2(g) + H2O(l)
-1235 kJ