Studies have shown that the reaction occurs via the following mechanism. ki 2 ClO2 2 Cl2O4 k-1 k2 Step 1: (fast equilibrium) Step 2: C204 + OH- → CIO3¯+ HC1O2 (slow) k3 Step 3: HC1O2 + OH → ClO2¯+ H2O (fast) Question 5: Identify the intermediate/s and the rate-determining step.

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Chapter1: Chemical Foundations
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Question 4
Calculate the frequency factor (A).
Studies have shown that the reaction occurs via
the following mechanism.
ki
Cl2O4
k-1
Step 1:
2 Cl02
(fast equilibrium)
k2
Step 2:
C2O4 + OH-
→ ClO;¯+HCIO2
(slow)
k3
Step 3:
HCIO2 + OH → ClO2¯+H2O
(fast)
Question 5: Identify the intermediate/s and the
rate-determining step.
ki
2 ClO2 2 C2O4
k-1
Step 1:
(fast equilibrium)
k2
→ ClO3¯+HC1O2
Step 2:
C204 + OH-
(slow)
k3
Step 3:
HC1O2 + OH-
ClO2- + H2O
(fast)
Question 6
Is the proposed mechanism consistent with the
experimentally determined rate law? Show your
solution to justify your answer.
ki
2 ClO2 2 C2O4
k-1
Step 1:
(fast equilibrium)
k2
Step 2:
C204 + OH-
→ ClO3¯+ HCIO2
(slow)
k3
Step 3:
HCIO2 + OH-
→ ClO2-+ H2O
(fast)
Question 7
Draw the transition state for Step 3. Identify the
bond/s forming/breaking.
Transcribed Image Text:Question 4 Calculate the frequency factor (A). Studies have shown that the reaction occurs via the following mechanism. ki Cl2O4 k-1 Step 1: 2 Cl02 (fast equilibrium) k2 Step 2: C2O4 + OH- → ClO;¯+HCIO2 (slow) k3 Step 3: HCIO2 + OH → ClO2¯+H2O (fast) Question 5: Identify the intermediate/s and the rate-determining step. ki 2 ClO2 2 C2O4 k-1 Step 1: (fast equilibrium) k2 → ClO3¯+HC1O2 Step 2: C204 + OH- (slow) k3 Step 3: HC1O2 + OH- ClO2- + H2O (fast) Question 6 Is the proposed mechanism consistent with the experimentally determined rate law? Show your solution to justify your answer. ki 2 ClO2 2 C2O4 k-1 Step 1: (fast equilibrium) k2 Step 2: C204 + OH- → ClO3¯+ HCIO2 (slow) k3 Step 3: HCIO2 + OH- → ClO2-+ H2O (fast) Question 7 Draw the transition state for Step 3. Identify the bond/s forming/breaking.
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