The important industrial chemical hydrazine, N2H4, is produced by the Raschig process. Here is a proposed mechanism for the process:
Step 1 (slow): NH3(aq) + OCl−(aq) ⟶ NH2Cl(aq) + OH−(aq)
Step 2 (fast): NH2Cl(aq) + NH3(aq) ⟶ N2H5+(aq) + Cl−(aq)
Step 3 (fast): N2H5+(aq) + OH−(aq) ⟶ N2H4(aq) + H2O(l)
- Determine which is the rate-limiting step. Describe how this step limits the overall reaction rate.
- Determine the overall reaction equation for the Raschig process.
- Identify all reaction intermediates in the proposed mechanism.
- Another student tells you that the reaction is second-order in ammonia and does not depend on any other concentration. The student says this is consistent with the mechanism written above. Explain why the student is, or is not, correct.
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