Question

Deduce the rate law from the mechanism below A2L2 = 2 AL (fast) 2 AL +...

Deduce the rate law from the mechanism below

A2L2 = 2 AL (fast)

2 AL + Q = A2L2Q (fast)

A2L2Q + Z --> ZL2 + A2Q (slow)

A) Rate = k3[A2L2Q][Z]

B) Rate = (k3k2k1)/(k-2k-1)[A2L2][Q][Z]

C) Rate = (k3k2)/k-2[A2L2][Z]

D) Rate = (k1k2k3)/(k-3k-2k-1)[A2L2] 2[Q][Z]

E) none of the above

Homework Answers

Answer #1

rate law depends on the slowest step.

Here slowest step is:

A2L2Q + Z --> ZL2 + A2Q (slow)

so,

rate law is:

rate= k3*[A2L2Q]*[Z]

Here A2L2Q is an intermediate

So, use steady state approximation is step 2:

K2 [AL]^2 [Q] = K-2 [AL2Q]

so,

[AL2Q] = (K2/K-2)* [AL]^2 [Q]

rate law now becomes:

rate= k3*[A2L2Q]*[Z]

rate= k3*(K2/K-2)* [AL]^2 [Q] *[Z]

AL is still an intermediate

So, use steady state approximation is step 1:

K1 [A2L2] = K-1 [AL]^2

so,

[AL]^2 = (K1/K-1)*[A2L2]

rate law now becomes:

rate= k3*(K2/K2b)* [AL]^2 [Q] *[Z]

rate= k3*(K2/K-2)* (K1/K-1)*[A2L2] [Q] *[Z]

Answer: B

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
A proposed mechanism for a reaction is as follows: Step 1 (fast): A + B <=>...
A proposed mechanism for a reaction is as follows: Step 1 (fast): A + B <=> C Step 2 (slow): C --> D + E Determine the rate law predicted by this mechanism A. Rate = k'[C] B. Rate = k'[A] C. Rate = k'[A][B] D. Rate = k'[B][D]
Based on the three step mechanism below, what is the rate law for the reaction 2A...
Based on the three step mechanism below, what is the rate law for the reaction 2A + 2B →E + G? A + B ⇌ D (Fast equilibrium) D + B →E + F ( slow) A + F → G (fast
A reaction mechanism is defined as the sequence of reaction steps that define the pathway from...
A reaction mechanism is defined as the sequence of reaction steps that define the pathway from reactants to products. Each step in a mechanism is an elementary reaction, which describes a single molecular event of usually one or two molecules interacting. The rate law for an overall reaction is the rate law for the slowest step in the mechanism, which is directly related to the stoichiometric coefficients of the reactants. The exception to this rule occurs when the slowest step...
What is the rate law for the following mechanism?                         CH3COOC2H5 + H2O → CH3COOC2H6+...
What is the rate law for the following mechanism?                         CH3COOC2H5 + H2O → CH3COOC2H6+ + OH-                  (Slow)                         CH3COOC2H6+          → CH3COOH + C2H5+                     (Fast)                         C2H5+   +      OH-        → C2H5OH                                   (Fast) A) Rate = k[CH3COOC2H5][H2O]2 B) Rate = k[C2H5OH] C) Rate = k[CH3COOH] D) Rate = k[CH3COOC2H5] E) Rate = k[CH3COOC2H5][H2O] The answer is E, but could you please give a detailed response on how to get to this answer? Thank you.
Given the following proposed mechanism, predict the rate law for the overall reaction. 2 NO2 +...
Given the following proposed mechanism, predict the rate law for the overall reaction. 2 NO2 + Cl2 → 2 NO2Cl (overall reaction) Mechanism NO2 + Cl2 → NO2Cl + Cl slow NO2 + Cl → NO2Cl fast Given the following proposed mechanism, predict the rate law for the overall reaction. 2 NO2 + Cl2 → 2 NO2Cl (overall reaction) Mechanism NO2 + Cl2 → NO2Cl + Cl slow NO2 + Cl → NO2Cl fast Rate = k[NO2][Cl]2 Rate = k[NO2][Cl2]...
How to calculate the overall rate law base on a reaction mechanism that involves 2 steps:...
How to calculate the overall rate law base on a reaction mechanism that involves 2 steps: first step is fast step and the second step is an equilibrium ? First Step: A --> B + C (fast) Second Step: B --> D + E (slow equilibrium)   
Determine the rate law that is consistent with the following mechanism: Step 1: OCl− + H2O...
Determine the rate law that is consistent with the following mechanism: Step 1: OCl− + H2O ⇄ HOCl + OH− (fast) Step 2: I− + HOCl  HOI + Cl− (slow) A) Rate = k[OCl−][H2O] B) Rate = k[I−][HOCl] C) Rate = k[OCl−][H2O][I−] D) Rate = k[OCl−][H2O]/[I−] E) Rate = k[OCl−][H2O]/[OH−] F) Rate = k[OCl−][H2O][I−]/[OH−]
26. The mechanism of a reaction is shown below: NO2C l --> NO2 + Cl (slow)...
26. The mechanism of a reaction is shown below: NO2C l --> NO2 + Cl (slow) NO2Cl + Cl --> NO2 + Cl2 (fast) a) What is the overall reaction? b) What are the intermediates? c)Which is the rate determining step? d) What is the rate law? 27. The mechanism of a reaction is shown below 2NO <--> N2O2 (fast) N2O2 + O2 --> 2NO2 (slow) What is the overall reaction? b) What are the intermediates? c)Which is the rate...
Consider the following mechanism proposed for a reaction: Step 1)     A + 2 B → C    ...
Consider the following mechanism proposed for a reaction: Step 1)     A + 2 B → C     (slow) Step 2)     C + D → E     (fast) Step 3)     E → A + F     (fast) Give the overall reaction that results from this mechanism: Based on the rate limiting step, what is the actual rate law for this mechanism? Select all of the following species that are intermediates in this reaction. E B F C A D Select all of the following...
Consider the following mechanism STEP 1: A <=> B + C (equilibrium) STEP 2: C +...
Consider the following mechanism STEP 1: A <=> B + C (equilibrium) STEP 2: C + D => E (slow) OVER ALL: A + C => B + E Determine the rate law for the overall reaction (where the overall rate constant is represented as k). RATE= k [ ? ] [ ? ]
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT