Question

A proposed mechanism is given for the reaction O3(g) + O(g) --> 2 O2(g). Determine the...

A proposed mechanism is given for the reaction O3(g) + O(g) --> 2 O2(g). Determine the rate law for this proposed mechanism, showing all work. Also identigy the intermeditate in this mechanism. (this isn't needed, but can you explain briefly how to decipher the intermediate for future reference please?)

Step 1: O3 + NO --> NO2 + O2 (slow)

Step 2: NO2 + O --> NO + O2 (fast)

Rate= __________________________ Intermediate = __________________________

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #2

Given that O3(g) + O(g) ----------> 2 O2 (g)         ------- Eq(1)

Mechanism:

Step 1: O3 + NO --> NO2 + O2 (slow)

Step 2: NO2 + O --> NO + O2   (fast)

Then,

Slowest step is always the rate determining step of the reaction.

Therefore,

rate = k [O3] [NO]

Intermediate:

The species other than reactants and products present in the reaction mechanism are called intermediates.

As per the Eq(1),

O3 , O = reactants

O2 = product

Therefore,

NO2, NO are intermediates.

answered by: anonymous
0 0
Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
A proposed mechanism is given for the reaction O3(g) + O(g) --> 2 O2(g). Determine the...
A proposed mechanism is given for the reaction O3(g) + O(g) --> 2 O2(g). Determine the rate law for this proposed mechanism, showing all work. Also identigy the intermeditate in this mechanism. (this isn't needed, but can you explain briefly how to decipher the intermediate for future reference please?) Step 1: O3 + NO --> NO2 + O2 Step 2: NO2 + O --> NO + O2 Rate= __________________________ Intermediate = __________________________
Original equation of Mechanism O3(g) + O(g) → 2O2(g) Determine rate law. Please include substitution. O3...
Original equation of Mechanism O3(g) + O(g) → 2O2(g) Determine rate law. Please include substitution. O3 (g) + Cl(g)⇌ ClO(g) + O2(g)          (fast, reversible) ClO(g) + O(g) → Cl(g) + O2(g)                 (slow)
One mechanism for the destruction of ozone in the upper atmosphere is 1. O3 +NO --->...
One mechanism for the destruction of ozone in the upper atmosphere is 1. O3 +NO ---> NO2 + O2 slow 2. NO2 + O ---> NO + O2 fast a.) What is the overall balanced equation for this reaction? b.) Write the rate law expected from this mechanism. c.) What order is the overall reaction with respect to [O]?
The following is a proposed mechanism for the reaction NO2 (g) + CO (g) --> NO...
The following is a proposed mechanism for the reaction NO2 (g) + CO (g) --> NO (g) + CO2 (g). The rate law for the reaction is rate = k [NO2]2 a) is this a plausible mechanism? Explain. B) identify the reactants, intermediates, and products. NO2 (g) + NO2 (g)--> NO3 (g) + NO (g) (slow) and NO3 (g) + CO (g) --> NO2 (g) + CO2 (g) (fast)
The following is a proposed mechanism for the reaction NO2 (g) + CO (g) --> NO...
The following is a proposed mechanism for the reaction NO2 (g) + CO (g) --> NO (g) + CO2 (g). The rate law for the reaction is rate = k [NO2]2 a) is this a plausible mechanism? Explain. B) identify the reactants, intermediates, and products. NO2 (g) + NO2 (g)--> NO3 (g) + NO (g) (slow) and NO3 (g) + CO (g) --> NO2 (g) + CO2 (g) (fast)
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]...
The mechanism for the reaction 2 H2O2(aq) à 2 H2O(l) + O2(g) in the presence of...
The mechanism for the reaction 2 H2O2(aq) à 2 H2O(l) + O2(g) in the presence of I–(aq) is proposed to be: Step 1: H2O2(aq) + I–(aq) à H2O(l) + OI–(aq)                                   (slow) Step 2: H2O2(aq) + OI–(aq) à H2O(l) + O2(g) + I–(aq)                       (fast) What is the rate law for the overall reaction?             a. Rate = k[H2O2]2             b. Rate = k[H2O2][I–]             c. Rate = k[H2O2]2[I–]/[H2O]             d. Rate = k[H2O2][OI–]             e. Rate = k[H2O2]
The following three step mechanism has been proposed for this reaction: Step 1: A + B...
The following three step mechanism has been proposed for this reaction: Step 1: A + B <--> G fast Step 2: A + G --> E + D slow Step 3: E + 2C --> 2D + F fast Determine the rate law predicted by the mechanism. Identify any intermediates shown. The experiemental rate law was determined to be Rate = [A]2[B]. Is this mechanism valid?
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...
The Proposed mechanism for the reaction A(g) + B(g) ---> D(g) + E(g) is as follows:...
The Proposed mechanism for the reaction A(g) + B(g) ---> D(g) + E(g) is as follows: Step 1. B(g) ---> 2C(g)   (fast) Step 2. A(g) + C(g) ---> E(g)+ F(g)  (slow) Step 3. C(g) + F(g) ---> D(g) (fast) The overall rate law for the reaction should be A. Rate = k[B] B. Rate = k[A][C] C. Rate = k[A][B][C] D. Rate = k[A][B]1/2 E. Rate = k[A]1/2[B] The correct answer is D but I'm not sure how exactly to get...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT