Question

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 molecularity of the first step?

(E) If step 1 were the rate determining, the slowest step, what would be the rate law for this reaction?

(F) If step 2 were the rate determining, the slowest step, what would be the rate law for this reaction?

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

A. adding step 1 and step 2 we have:

Br + O3 + BrO + O → BrO + O2 + Br + O2

Eliminating Br and BrO from both side we get

O3 + O → O2 + O2

Or, O3 + O → 2O2   This is overall reaction.

B. Here in step 1 BrO is produced which destroyed in step 2. So BrO is the intermidiate.

C. In step 1 Br reacts with O3 and at the end of the reaction at step 2, Br is reproduced. So Br is the catalyst.

D. Molecularity is the total number of coefficient of reactant. So molecularity of step 1 is 2. [2 reactants]

E. If step 1 is the rate determining step, then rate = K1 [Br] [O3] , where K1 is rate constant of step 1 and [X] is the concentration of X.

F. If step 2 is the rate determining step, then rate = K2 [BrO] [O] , where K2 is rate constant of step

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
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]?
Experimental data show that the homogeneous decomposition of ozone proceeds with a rate r   =   k...
Experimental data show that the homogeneous decomposition of ozone proceeds with a rate r   =   k [O3]2 [O2]‒1 Suggest a mechanism to explain this rate. [Hint: the first step is reaction of ozone with an “initiator” molecule (M) to form an M•O complex.]
A suggested mechanism for the gas phase decomposition of nitrous oxide is: step 1 slow:   N2O...
A suggested mechanism for the gas phase decomposition of nitrous oxide is: step 1 slow:   N2O --> N2 + O step 2 fast:   N2O + O --> N2 + O2 (1) What is the equation for the overall reaction? Use the smallest integer coefficients possible. (2) Which species acts as a catalyst? Enter formula. (3) Which species acts as a reaction intermediate? Enter formula. (4) Complete the rate law for the overall reaction that is consistent with this mechanism. (Use...
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,...
The iodide-catalyzed decomposition of hydrogen peroxide is thought to proceed by a four-step mechanism: H2O2(aq) +...
The iodide-catalyzed decomposition of hydrogen peroxide is thought to proceed by a four-step mechanism: H2O2(aq) + I-(aq) --> HOI(aq) + OH-(aq) (slow) HOI(aq) + OH-(aq) --> H2O(l) + OI-(aq) OI-(aq) + H2O2(aq) --> HOOI(aq) + OH-(aq) HOOI(aq) + OH-(aq) --> H2O(l) + O2(g) + I-(aq) (a) If the first step of this mechanism is rate-determining (slow), choose the correct rate law for the overall process. oRate = k [H2O2]2 oRate = k [I-] [H2O2] oRate = k [H2O2] [H2O2] oRate...
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...
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 = __________________________
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 = __________________________
Using the reaction mechanism below, answer the following questions: 1. Cl2 -> 2Cl 2. Cl +...
Using the reaction mechanism below, answer the following questions: 1. Cl2 -> 2Cl 2. Cl + CHCl3 -> HCl + CCl3 3. Cl + CCl3 -> CCl4 a. What is the chemical equation for the overall reaction? b. If the first step was the slowest step, what is the rate law for the overall reaction? What is the overall order of the reaction? c. If the second step was the slowest step, what is the rate law for the overall...
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.
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT