(^20) › STEP 2. Determine Your Test Readiness
- Aluminum metal reacts with gaseous HCl to
produce aluminum chloride and hydrogen gas.
What volume of hydrogen gas, at STP, is pro-
duced when 13.5 g of aluminum is mixed with
an excess of HCl?
(A) 22.4 L
(B) 33.6 L
(C) 11.2 L
(D) 16.8 L - A sample containing the gases carbon dioxide,
carbon monoxide, and water vapor was analyzed
and found to contain 4.5 mol of carbon dioxide,
4.0 mol of carbon monoxide, and 1.5 mol of
water vapor. The mixture had a total pressure
of 1.2 atm. What was the partial pressure of the
carbon monoxide?
(A) 0.48 atm
(B) 0.18 atm
(C) 5.4 atm
(D) 0.54 atm - An ideal gas sample weighing 0.548 g at 100°C
and 0.993 atm has a volume of 0.237 L.
Determine the molar mass of the gas.
(A) 71.3 g/mol
(B) 143 g/mol
(C) 19.1 g/mol
(D) 0.0140 g/mol - If a sample of He effuses at a rate of 30 mol
per hour at 45°C, which of the gases below will
effuse at approximately one-half the rate under
the same conditions?
(A) CH 4
(B) O 3
(C) N 2
(D) H 2 - The average kinetic energy of nitrogen molecules
changes by what factor when the temperature is
increased from 30°C to 60°C?
(A) (333 - 303)
(B) 2
(C) 1 ⁄ 2
(D)^303 −^333
Chapter 9
- Which of the following is the required energy to
produce a gaseous cation from a gaseous atom in
the ground state?
(A) free energy
(B) lattice energy
(C) kinetic energy
(D) ionization energy - The average ____ is the same for any
ideal gas at a given temperature.
(A) free energy
(B) lattice energy
(C) kinetic energy
(D) ionization energy - Which of the following is the maximum energy
available for useful work from a spontaneous
reaction?
(A) free energy
(B) lattice energy
(C) kinetic energy
(D) ionization energy - The energy required to completely separate the
ions from a solid is which of the following?
(A) free energy
(B) lattice energy
(C) kinetic energy
(D) ionization energy - Oxidation of ClF by F 2 yields ClF 3 , an important
fluorinating agent formerly used to produce the
uranium compounds in nuclear fuels:
ClF(g) + F 2 (g) → 2 ClF 3 (l)
Use the following thermochemical equations to
calculate DH°rxn for the production of ClF 3 :- 2 ClF(g) + O 2 (g) DH° = 167.5 kJ
→ Cl 2 O(g) + OF 2 (g) - 2 F 2 (g) + O 2 (g) DH° = - 43.5 kJ
→ 2 OF 2 (g) - 2 ClF 3 (l) + 2 O 2 (g) DH° = 394.1 kJ
→ Cl 2 O(g) + 3 OF 2 (g)
(A) +270.2 kJ
(B) -135.1 kJ
(C) 0.0 kJ
(D) -270.2 kJ
- 2 ClF(g) + O 2 (g) DH° = 167.5 kJ