Solution Found!
The proposed mechanism for a reaction is(1) [fast](2)
Chapter 16, Problem 61P(choose chapter or problem)
The proposed mechanism for a reaction is
(a) What is the overall equation?
(b) Identify the intermediate(s), if any.
(c) What are the molecularity and the rate law for each step?
(d) Is the mechanism consistent with the actual rate law: \(\text { rate }=k[\mathrm{~A}][\mathrm{B}][\mathrm{C}]\)?
(e) Is the following one-step mechanism equally valid:
\(\mathrm{A}(g)+\mathrm{B}(g)+\mathrm{C}(g) \longrightarrow \mathrm{D}(g) ?\)
Equation Transcription:
rate = 𝑘[A][B][C]
Text Transcription:
rate=k[A][B][C]
A(g)+B(g)+C(g) rightarrow D(g)
Questions & Answers
QUESTION:
The proposed mechanism for a reaction is
(a) What is the overall equation?
(b) Identify the intermediate(s), if any.
(c) What are the molecularity and the rate law for each step?
(d) Is the mechanism consistent with the actual rate law: \(\text { rate }=k[\mathrm{~A}][\mathrm{B}][\mathrm{C}]\)?
(e) Is the following one-step mechanism equally valid:
\(\mathrm{A}(g)+\mathrm{B}(g)+\mathrm{C}(g) \longrightarrow \mathrm{D}(g) ?\)
Equation Transcription:
rate = 𝑘[A][B][C]
Text Transcription:
rate=k[A][B][C]
A(g)+B(g)+C(g) rightarrow D(g)
ANSWER:Solution 61P
Step 1
Here we have to write the overall equation.
(1) A(g) + B(g) ⇆ X(g) [fast]
(2) X(g) + C(g) → Y(g) [slow]
(3) Y(g)→ D(g) [fast]
In order to write the overall reaction, we have to add all the three equations.
(1) A(g) + B(g) ⇆ X(g) [fast]
(2) X(g) + C(g) → Y(g) [slow]
(3) Y(g)→ D(g) [fast]
A(g) + B(g) + X(g) + C(g) +Y(g) → X(g) + Y(g) + D(g)
Thus the overall reaction is,
A(g) + B(g)+ C(g) →D(g)