Question

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]?

Homework Answers

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
Nitric oxide (NO) can catalyze ozone destruction through the catalytic process described below: NO + O3...
Nitric oxide (NO) can catalyze ozone destruction through the catalytic process described below: NO + O3 > NO2 + O2 (Reaction 1) NO2 + O > NO + O2 (Reaction 2) The reaction rate (how fast the reaction proceeds) is calculated as the product of the reaction rate constant k, and the respective concentrations of the reactants e.g. in the reaction A + B products, the reaction rate is given by Rate = d[A]/dt = d[B]/dt = k[A][B]. The reaction...
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 = __________________________
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)
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 = __________________________
Consider the two-step mechanism for a reaction: Step 1     NO2     +     NO2 -------> NO3     +      NO       &n
Consider the two-step mechanism for a reaction: Step 1     NO2     +     NO2 -------> NO3     +      NO         slow; RDS Step 2     NO3     +     CO -------> NO2     +     CO2         fast a. What is the overall reaction? b. Identify the intermediates in the reaction mechanism. c. What is the predicted rate law expression? Be sure to only list reactants from the overall equation and not intermediates in the rate law expression.
The decomposition of ozone in the stratosphere can occur by the following two-step mechanism:             Step...
The decomposition of ozone in the stratosphere can occur by the following two-step mechanism:             Step 1: Br + O3 → BrO + O2             Step 2: BrO + O → Br + O2 This question has multiple parts. Be sure to answer all of them! (A) What is the overall reaction when steps 1 and 2 are added together? (B) What is the intermediate in this reaction? (C) What is the catalyst in this reaction? (D) What is the...
The ozone layer is a protective layer around the Earth that absorbs UV radiations. Stratospheric ozone...
The ozone layer is a protective layer around the Earth that absorbs UV radiations. Stratospheric ozone is depleted through the reaction of ozone, O3O3, with nitric oxide, NONO. The gaseous emissions from vehicles and industries are responsible for the rapid destruction of this layer. The destruction of the ozone by nitric oxide (NONO) is shown in the video. This is a two-step reaction, called a multistep reaction, involving a catalyst and an intermediate. Nitric oxide (NONO) enhances the reaction rate,...
A mechanism for a naturally occurring reaction that destroys ozone is: Step 1: O3(g) + HO(g)...
A mechanism for a naturally occurring reaction that destroys ozone is: Step 1: O3(g) + HO(g) → HO2(g) + O2(g) Step 2: HO2(g) + O(g) → HO(g) + O2(g) Which species is a catalyst and what type of catalysis is occurring? Select one: A. HO, heterogeneous B. HO2, heterogeneous C. HO2, homogeneous D. HO, homogeneous The relative initial rates of the reaction A2 + B2 → products in vessels (a)-(d) are 1:1:4:4. Unshaded spheres represent A2 molecules, and shaded spheres...
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...
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]...