CHEM134 C003 ADVANCED GENERAL
CHEMISTRY FINAL EXAM QUESTIONS
AND ANSWERS WITH VERIFIED
SOLUTIONS 2026/2027 UPDATE. JUST
RELEASED
1. Calculate the molar solubility of Ag2CrO4 in a solution that is 0.10 M in AgNO3. (Ksp of
Ag2CrO4 = 1.1 x 10^-12)
A. 1.1 x 10^-11 M
B. 3.3 x 10^-9 M
C. 1.1 x 10^-10 M
D. 5.5 x 10^-11 M
Answer: C
Conceptual Explanation: Due to the common ion effect, [Ag+] = 0.10 M. Ksp =
[Ag+]^2[CrO4^2-]. Thus, 1.1 x 10^-12 = (0.10)^2 * S, which gives S = 1.1 x 10^-10 M.
2. Which of the following molecules has the largest bond angle?
A. BeCl2
,B. NH3
C. H2O
D. CH4
Answer: A
Conceptual Explanation: BeCl2 is linear (180 degrees), while the others are tetrahedral
derivatives with angles less than or equal to 109.5 degrees.
3. For a second-order reaction, what are the units of the rate constant k if concentration is in
M and time is in seconds?
A. M^-2 s^-1
B. s^-1
C. M s^-1
D. M^-1 s^-1
Answer: D
Conceptual Explanation: Rate = k[A]^2. M/s = k * M^2, so k = 1/(M*s) = M^-1 s^-1.
4. What is the pH of a 0.15 M solution of NH4Cl? (Kb for NH3 = 1.8 x 10^-5)
A. 5.04
B. 8.96
C. 4.74
, D. 9.26
Answer: A
Conceptual Explanation: NH4+ is the conjugate acid. Ka = Kw/Kb = 10^-.8x10^-5 =
5.56x10^-10. [H+] = sqrt(Ka * C) = sqrt(5.56x10^-10 * 0.15) = 9.13x10^-6. pH = -log[H+] =
5.04.
5. A reaction has a positive delta H and a positive delta S. When is this reaction spontaneous?
A. At all temperatures
B. At low temperatures
C. At high temperatures
D. Never spontaneous
Answer: C
Conceptual Explanation: Delta G = Delta H - T * Delta S. If both are positive, Delta G
becomes negative only when T * Delta S is larger than Delta H, which occurs at high
temperatures.
6. Determine the bond order of the O2+ ion according to Molecular Orbital Theory.
A. 2.0
B. 2.5
C. 1.5
D. 3.0
CHEMISTRY FINAL EXAM QUESTIONS
AND ANSWERS WITH VERIFIED
SOLUTIONS 2026/2027 UPDATE. JUST
RELEASED
1. Calculate the molar solubility of Ag2CrO4 in a solution that is 0.10 M in AgNO3. (Ksp of
Ag2CrO4 = 1.1 x 10^-12)
A. 1.1 x 10^-11 M
B. 3.3 x 10^-9 M
C. 1.1 x 10^-10 M
D. 5.5 x 10^-11 M
Answer: C
Conceptual Explanation: Due to the common ion effect, [Ag+] = 0.10 M. Ksp =
[Ag+]^2[CrO4^2-]. Thus, 1.1 x 10^-12 = (0.10)^2 * S, which gives S = 1.1 x 10^-10 M.
2. Which of the following molecules has the largest bond angle?
A. BeCl2
,B. NH3
C. H2O
D. CH4
Answer: A
Conceptual Explanation: BeCl2 is linear (180 degrees), while the others are tetrahedral
derivatives with angles less than or equal to 109.5 degrees.
3. For a second-order reaction, what are the units of the rate constant k if concentration is in
M and time is in seconds?
A. M^-2 s^-1
B. s^-1
C. M s^-1
D. M^-1 s^-1
Answer: D
Conceptual Explanation: Rate = k[A]^2. M/s = k * M^2, so k = 1/(M*s) = M^-1 s^-1.
4. What is the pH of a 0.15 M solution of NH4Cl? (Kb for NH3 = 1.8 x 10^-5)
A. 5.04
B. 8.96
C. 4.74
, D. 9.26
Answer: A
Conceptual Explanation: NH4+ is the conjugate acid. Ka = Kw/Kb = 10^-.8x10^-5 =
5.56x10^-10. [H+] = sqrt(Ka * C) = sqrt(5.56x10^-10 * 0.15) = 9.13x10^-6. pH = -log[H+] =
5.04.
5. A reaction has a positive delta H and a positive delta S. When is this reaction spontaneous?
A. At all temperatures
B. At low temperatures
C. At high temperatures
D. Never spontaneous
Answer: C
Conceptual Explanation: Delta G = Delta H - T * Delta S. If both are positive, Delta G
becomes negative only when T * Delta S is larger than Delta H, which occurs at high
temperatures.
6. Determine the bond order of the O2+ ion according to Molecular Orbital Theory.
A. 2.0
B. 2.5
C. 1.5
D. 3.0
