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Worksheetsreaction mechanisms
Total questions: 28
Worksheet time: 16mins
Based on this reaction mechanism, which of the following are intermediates?
A
B
C
D
E
What is the molecularity for step 1?
Unimolecular
Bimolecular
Termolecular
What is the molecularity for step 2?
Unimolecular
Bimolecular
Termolecular
Tetramolecular
What is the overall equation for the reaction with these elementary steps?
2A + 2B + D -> 2B + 2C + D + E
A -> 2B
A + B -> C + D
2A -> 2C + E
If this is the correct mechanism for the reaction, which is the rate-limiting step?
1
2
3
What is the rate law for step 1 of this reaction?
rate = k1[A]
rate = k1[B]2
rate = k1[2B]/[A]
rate = k1[A]/[B]2
What is the overall rate law for this full reaction?
rate = k1[A]
rate = k1[B]2
rate = k1[2B]/[A]
rate = k1[A]/[B]2
What is the molecularity of step 1?
Unimolecular
Bimolecular
Termolecular
What is the molecularity of step 2?
Unimolecular
Bimolecular
Termolecular
What is the overall reaction equation?
A -> B + C
D + B -> 2E
A + D -> C + 2E
A + D + B -> B + C + 2E
What is the rate-determining step?
1
2
What are the intermediate(s) in this reaction?
A
B
C
D
E
What is the forward rate law for step 1?
rate = k1[A]
rate = k-1[B][C]
rate = k2[B][D]
rate = k-2[E]2
What is the reverse rate law for step 1?
rate = k1[A]
rate = k-1[B][C]
rate = k2[B][D]
rate = k-2[E]2
What is the forward rate law for step 2?
rate = k1[A]
rate = k-1[B][C]
rate = k2[B][D]
rate = k-2[E]2
Recalling that k1[A] = k-1[B][C] and rate = k2[B][D], what is the overall rate law of this reaction?
rate = k[A]
rate = k[B][A][D]
rate = k[C][A][D]
rate = k[B][D]
The decomposition of nitrous oxide :
2N2O(g) → 2N2(g) + O2(g)
is believed to occur by two-step mechanism
N2O(g) → N2(g) + O(g) (slow)
N2O(g) + O(g) → N2(g) + O2(g) (fast)
the consistent rate equation based on the mechanism above is ____
rate = k [N2O]2
rate = k [N2O]
rate = k [N2O]2 [N2]
rate = k
Reaction :
2A + B → C + D
is proposed to have reaction mechanism shown below :
A + B → AB + D (slow)
A + AB → C (fast)
the consistent rate equation with the reaction mechanism above is ____
rate = k [A]2 [B]
rate = k [A]2 [B]2
rate = k [A] [B]
rate = k [A] [B]2
The minimum energy particles must have to react is the
acting energy
active energy
activation energy
Which letter shows the activation energy
A
B
C
Step 1: Cl(g) + O3(g) → ClO(g) + O2(g)
Step 2: ClO(g) + O(g) → Cl(g) + O2(g)
A proposed mechanism for destruction of ozone gas in the stratosphere is represented above. Which of the following is evidence that the mechanism is occurring?
The presence of Cl(g) increases the rate of the overall reaction.
The presence of Cl(g) decreases the rate of the overall reaction.
The presence of Cl(g) increases the equilibrium constant of the overall reaction.
The presence of Cl(g) decreases the equilibrium constant of the overall reaction.
The particle models shown above represent a proposed two-step mechanism for the destruction of ozone (O3) in the upper atmosphere.
Based on the proposed mechanism, which of the following best describes the concentration ClO represented above as the reaction occurs?
The concentration is larger than that of reactant or product.
The concentration is very low for the duration of the reaction.
The concentration increases steadily as the reaction proceeds.
The concentration fluctuates between high and low during the reaction.
the reaction between gaseous iodine monochloride, ICl, and gaseous hydrogen :
H2(g) + 2ICl (g) → I2(g) + 2HCl (g)
has a rate equation : k [ICl] [H2]
Which one IS TRUE based on information above?
unimolecular reaction probably take places in rate-determining step
H2 molecules only involved in fast step reaction
It's likely that only 1 molecule of ICl is involved in rate-determining step
The reaction doesn't depends on the concentration of H2
Step 1: NO(g) + O3(g) → NO2(g) + O2(g)
Step 2: NO2(g) + O(g) → NO(g) + O2(g)
A reaction mechanism for the destruction of ozone, O3(g), is represented above. In the overall reaction, NO(g) is best described as
an inhibitor
a catalyst
a reactant
an intermediate
a product
The particle models shown above represent a proposed two-step mechanism for the destruction of ozone (O3O3) in the upper atmosphere.
Based on the models, which of the following represents a species that acts as a catalyst for the reaction?
Step 1: Ce4+ + Mn2+ → Ce3+ + Mn3+
Step 2: Ce4+ + Mn3+ → Ce3+ + Mn4+
Step 3: Mn4+ + Tl+ → Tl3+ + Mn2+
The proposed steps for a catalyzed reaction between Ce4+ and Tl+ are represented above. The products of the overall catalyzed reaction are
Ce4+ and Tl+
Ce3+ and Tl3+
Ce3+ and Mn3+
Ce3+ and Mn4+
Tl3+ and Mn2+
The particle models shown above represent a proposed two-step mechanism for the destruction of ozone (O3O3) in the upper atmosphere.
Based on the proposed mechanism, what is the balanced chemical equation for the overall reaction?
O3 + Cl → O2 + ClO
2 O3 + 2 Cl → 2 O2 + 2 ClO
O3 + Cl + ClO → 2 O2 + Cl2
2 O3 → 3 O2
