1|Page
ACS Gen Chem 2 Final Exam Study Guide 2026 |
Complete Questions and Guide Answers, 100%
Verified Graded A+
1. A reaction has a rate law of Rate=k[A]2[B]\text{Rate}=k[A]^2[B]. If
the concentration of AA is doubled while the concentration of BB
remains constant, how will the initial reaction rate change?
A. It will increase by a factor of 2.
B. It will increase by a factor of 4.
C. It will increase by a factor of 6.
D. It will remain unchanged.
Answer: B
2. For a reaction that follows first-order kinetics, which mathematical
relationship should produce a straight line when experimental data are
plotted?
A. [A][A] versus time
B. 1/[A]1/[A] versus time
C. ln[A]\ln[A] versus time
D. ln(1/[A])\ln(1/[A]) versus 1/t1/t
Answer: C
3. A first-order reaction has a half-life of 18.0 minutes. If the initial
concentration is 0.800 M, what concentration remains after 54.0
minutes?
A. 0.400 M
B. 0.200 M
C. 0.100 M
D. 0.050 M
,2|Page
Answer: C
4. Increasing the temperature of a reaction substantially increases its
rate. Which explanation is most consistent with collision theory?
A. Increasing temperature decreases the activation energy of every
reaction.
B. Increasing temperature increases the fraction of molecules possessing
energy equal to or greater than the activation energy.
C. Increasing temperature necessarily increases the equilibrium constant.
D. Increasing temperature changes an endothermic reaction into an
exothermic reaction.
Answer: B
5. A catalyst is added to a chemical reaction at equilibrium. Which
statement correctly describes its effect?
A. It increases the equilibrium constant.
B. It shifts equilibrium toward the products.
C. It shifts equilibrium toward the reactants.
D. It decreases the activation energy for both forward and reverse
reactions without changing the equilibrium constant.
Answer: D
6. Consider the equilibrium:
N2(g)+3H2(g)⇌2NH3(g)N_2(g)+3H_2(g)\rightleftharpoons2NH_3(g)
If additional H2H_2 is introduced while temperature remains constant,
what will happen?
A. The equilibrium shifts toward reactants.
B. The equilibrium shifts toward products.
C. The equilibrium constant decreases.
,3|Page
D. No change occurs because H2H_2 is not part of the equilibrium
expression.
Answer: B
7. For the equilibrium
2SO2(g)+O2(g)⇌2SO3(g)2SO_2(g)+O_2(g)\rightleftharpoons2SO_3(g)
which expression correctly represents KcK_c?
A. [SO2]2[O2][SO3]2\frac{[SO_2]^2[O_2]}{[SO_3]^2}
B. [SO3][SO2][O2]\frac{[SO_3]}{[SO_2][O_2]}
C. [SO3]2[SO2]2[O2]\frac{[SO_3]^2}{[SO_2]^2[O_2]}
D. [SO3]2[SO2][O2]2\frac{[SO_3]^2}{[SO_2][O_2]^2}
Answer: C
8. A reaction has K=4.5×10−8K=4.5\times10^{-8}. What does this
value most strongly indicate about the equilibrium mixture?
A. Products are strongly favored.
B. Reactants are strongly favored.
C. Reactants and products must be present in exactly equal
concentrations.
D. The reaction cannot occur.
Answer: B
9. A reaction has K=2.0×105K=2.0\times10^5. If the reaction quotient
QQ is initially 4.0×1024.0\times10^2, in which direction will the
reaction proceed to reach equilibrium?
A. Toward products
B. Toward reactants
C. It is already at equilibrium
D. The direction cannot be determined from QQ and KK
, 4|Page
Answer: A
10. A weak acid has Ka=1.8×10−5K_a=1.8\times10^{-5}. Which
statement best describes this acid compared with a strong acid?
A. It completely ionizes in water.
B. It establishes an equilibrium in which only a fraction of the acid
molecules ionize.
C. It cannot donate protons.
D. Its conjugate base must also be a strong acid.
Answer: B
11. What is the approximate pH of a 1.0×10−31.0\times10^{-3} M
solution of a strong monoprotic acid?
A. 1.00
B. 2.00
C. 3.00
D. 11.00
Answer: C
12. A solution has a pH of 11.50 at 25°C. What is its approximate pOH?
A. 2.50
B. 11.50
C. 12.50
D. 14.00
Answer: A
13. A buffer contains significant concentrations of
CH3COOHCH_3COOH and CH3COO−CH_3COO^-. A small amount
of HCl is added. What occurs primarily?
ACS Gen Chem 2 Final Exam Study Guide 2026 |
Complete Questions and Guide Answers, 100%
Verified Graded A+
1. A reaction has a rate law of Rate=k[A]2[B]\text{Rate}=k[A]^2[B]. If
the concentration of AA is doubled while the concentration of BB
remains constant, how will the initial reaction rate change?
A. It will increase by a factor of 2.
B. It will increase by a factor of 4.
C. It will increase by a factor of 6.
D. It will remain unchanged.
Answer: B
2. For a reaction that follows first-order kinetics, which mathematical
relationship should produce a straight line when experimental data are
plotted?
A. [A][A] versus time
B. 1/[A]1/[A] versus time
C. ln[A]\ln[A] versus time
D. ln(1/[A])\ln(1/[A]) versus 1/t1/t
Answer: C
3. A first-order reaction has a half-life of 18.0 minutes. If the initial
concentration is 0.800 M, what concentration remains after 54.0
minutes?
A. 0.400 M
B. 0.200 M
C. 0.100 M
D. 0.050 M
,2|Page
Answer: C
4. Increasing the temperature of a reaction substantially increases its
rate. Which explanation is most consistent with collision theory?
A. Increasing temperature decreases the activation energy of every
reaction.
B. Increasing temperature increases the fraction of molecules possessing
energy equal to or greater than the activation energy.
C. Increasing temperature necessarily increases the equilibrium constant.
D. Increasing temperature changes an endothermic reaction into an
exothermic reaction.
Answer: B
5. A catalyst is added to a chemical reaction at equilibrium. Which
statement correctly describes its effect?
A. It increases the equilibrium constant.
B. It shifts equilibrium toward the products.
C. It shifts equilibrium toward the reactants.
D. It decreases the activation energy for both forward and reverse
reactions without changing the equilibrium constant.
Answer: D
6. Consider the equilibrium:
N2(g)+3H2(g)⇌2NH3(g)N_2(g)+3H_2(g)\rightleftharpoons2NH_3(g)
If additional H2H_2 is introduced while temperature remains constant,
what will happen?
A. The equilibrium shifts toward reactants.
B. The equilibrium shifts toward products.
C. The equilibrium constant decreases.
,3|Page
D. No change occurs because H2H_2 is not part of the equilibrium
expression.
Answer: B
7. For the equilibrium
2SO2(g)+O2(g)⇌2SO3(g)2SO_2(g)+O_2(g)\rightleftharpoons2SO_3(g)
which expression correctly represents KcK_c?
A. [SO2]2[O2][SO3]2\frac{[SO_2]^2[O_2]}{[SO_3]^2}
B. [SO3][SO2][O2]\frac{[SO_3]}{[SO_2][O_2]}
C. [SO3]2[SO2]2[O2]\frac{[SO_3]^2}{[SO_2]^2[O_2]}
D. [SO3]2[SO2][O2]2\frac{[SO_3]^2}{[SO_2][O_2]^2}
Answer: C
8. A reaction has K=4.5×10−8K=4.5\times10^{-8}. What does this
value most strongly indicate about the equilibrium mixture?
A. Products are strongly favored.
B. Reactants are strongly favored.
C. Reactants and products must be present in exactly equal
concentrations.
D. The reaction cannot occur.
Answer: B
9. A reaction has K=2.0×105K=2.0\times10^5. If the reaction quotient
QQ is initially 4.0×1024.0\times10^2, in which direction will the
reaction proceed to reach equilibrium?
A. Toward products
B. Toward reactants
C. It is already at equilibrium
D. The direction cannot be determined from QQ and KK
, 4|Page
Answer: A
10. A weak acid has Ka=1.8×10−5K_a=1.8\times10^{-5}. Which
statement best describes this acid compared with a strong acid?
A. It completely ionizes in water.
B. It establishes an equilibrium in which only a fraction of the acid
molecules ionize.
C. It cannot donate protons.
D. Its conjugate base must also be a strong acid.
Answer: B
11. What is the approximate pH of a 1.0×10−31.0\times10^{-3} M
solution of a strong monoprotic acid?
A. 1.00
B. 2.00
C. 3.00
D. 11.00
Answer: C
12. A solution has a pH of 11.50 at 25°C. What is its approximate pOH?
A. 2.50
B. 11.50
C. 12.50
D. 14.00
Answer: A
13. A buffer contains significant concentrations of
CH3COOHCH_3COOH and CH3COO−CH_3COO^-. A small amount
of HCl is added. What occurs primarily?
