Consider the following two-step mechanism for a reaction: NO2(g)+Cl2(g)⟶k1ClNO2(g)+Cl(g) Slow NO2(g)+Cl(g)⟶k2ClNO2(g) Fast Part A What is...
Consider the following two-step mechanism for a reaction:
NO2(g)+Cl2(g)⟶k1ClNO2(g)+Cl(g)
Slow
NO2(g)+Cl(g)⟶k2ClNO2(g)
Fast
Part A
What is the overall reaction?
Express your answer as a chemical equation. Identify all of the phases in your answer.
Homework Answers
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Consider the following two-step mechanism for a reaction:
NO2(g)+Cl2(g)⟶k1ClNO2(g)+Cl(g)
Slow
NO2(g)+Cl(g)⟶k2ClNO2(g)
Fast
Part A
What is...
Consider the following two-step mechanism for a reaction: NO2(g)+Cl2(g)→ClNO2(g)+Cl(g)Slow N O 2 ( g ) +...
Consider the following two-step mechanism for a reaction: NO2(g)+Cl2(g)→ClNO2(g)+Cl(g)Slow N O 2 ( g ) + C l 2 ( g ) → C l N O 2 ( g ) + C l ( g ) S l o w NO2(g)+Cl(g)→ClNO2(g)Fast a)What is the overall reaction? Express your answer as a chemical equation. Identify all of the phases in your answer. b)Identify the intermediates in the mechanism. Check all that apply. Check all that apply. NO2(g), ClNO2(g), Cl2(g) ,Cl(g)...
2NO2 +Cl2 ----> 2NO2Cl mechanism: NO2 +Cl2 -----> NO2Cl +Cl (Slow step) NO2 +Cl -----> NO2Cl...
2NO2 +Cl2 ----> 2NO2Cl mechanism: NO2 +Cl2 -----> NO2Cl +Cl (Slow step) NO2 +Cl -----> NO2Cl (fast step) using the mechanism, draw and energy profile of the reaction showing the relative energy of the reactants and products (this reaction is exothermic), both transition states, intermediates, activation energy for both steps, and the overall change in enthalpy for the reaction (Delta H of the reaction).
Consider the following three step mechanism for a reaction Cl2 > 2Cl Fast Cl+CHCl3 > HCl+CCl3...
Consider the following three step mechanism for a reaction Cl2 > 2Cl Fast Cl+CHCl3 > HCl+CCl3 Slow Cl+CCl3 > CCl4 Fast What is the predicted rate law? How do you do it? The answer is rate=K[Cl2]^.5 [CHCl3]
2. Consider this two step mechanism for a reaction… Step 1 NO2 + O3 --> NO3 ...
2. Consider this two step mechanism for a reaction… Step 1 NO2 + O3 --> NO3 + O2 slow; rate determining step Step 2 NO3 + NO2 --> N2O5 fast a. What is the overall reaction? b. Identify the intermediates in the mechanism. c. Write the rate law expression for each step of the mechanism including any reversible reactions. c. What is the predicted rate law expression? Be sure to only list reactants from the overall equation and not intermediates...
Predict the overall reaction from the following two-step mechanism: 2 A→A 2(fast) A2+B→A2B(slow) Express your answer...
Predict the overall reaction from the following two-step mechanism: 2 A→A 2(fast) A2+B→A2B(slow) Express your answer as a chemical equation. Predict the rate law from the following two-step mechanism: 2A⇌ A2 (fast) A2+B→A2B (slow)
A proposed mechanism for a reaction is as follows: NO2(g) + NO2(g) + N204(8) Fast/Equilibrium Step...
A proposed mechanism for a reaction is as follows: NO2(g) + NO2(g) + N204(8) Fast/Equilibrium Step N2048) -> NO(g) + NO3(g) Slow NO3(g) NO) + O2(g) Fast The target rate law is rate = k (NO2)2 The target reaction is 2NO2(e) 2NON + O2) A. Write the rate law expected for this mechanism: B. What is the rate-determining step? C. What is the overall balanced equation for this mechanism? D. If there is/are a reactive intermediate(s), which is/are they? E....
Part A Given the following proposed mechanism, predict the rate law for the overall reaction. 2...
Part A 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 Answer Choices: Rate =...
A three-step mechanism has been suggested for the formation of carbonyl chloride: Step 1: Cl2 ===> 2 Cl (fast equlibrium) Step 2: Cl + CO ===> COCl (fast equilibrium) Step 3: COCl + Cl2 ===> COCl2 + Cl (slow) What is the molecularit
1. A three-step mechanism has been suggested for the formation of carbonyl chloride: Step 1: Cl2 ===> 2 Cl (fast equlibrium) Step 2: Cl + CO ===> COCl (fast equilibrium) Step 3: COCl + Cl2 ===> COCl2 + Cl (slow) What is the molecularity of the rate-determining step? unimolecular bimolecular termolelcular none of these 2. The elementary reaction representing the formation of ozone, O2(g) + O(g) + M(g) ===> O3(g) + M*(g) is an example of a _________ reaction. unimolecular...
10. Consider the reaction that takes place via the mechanism below; STEP I: NO2(g) + CO(g) - NO(g) + CO2(e) (fast)...
10. Consider the reaction that takes place via the mechanism below; STEP I: NO2(g) + CO(g) - NO(g) + CO2(e) (fast) STEP II: NO) + Cl2(e) - NOC12(e) (slow) Determine; (a) The reaction intermediate(s) (2 points) command (b) The rate determining step (2 points)
The proposed mechanism for a reaction is Cl2 => Cl+ + Cl- Slow Cl- + H2S...
The proposed mechanism for a reaction is Cl2 => Cl+ + Cl- Slow Cl- + H2S => HCl + HS- Fast Cl+ + HS- => HCl + S Fast Which of the following would be a rate law for the reaction? A. rate = k[Cl2] B. rate = k[Cl2][H2S] C. rate = k[Cl2]1/2[H2S] D. rate = k[Cl-][H2S] E. rate = [Cl+][Cl-]
A proposed mechanism for a reaction is as follows: NO2(g) + NO2(g) + N204(8) Fast/Equilibrium Step N2048) -> NO(g) + NO3(g) Slow NO3(g) NO) + O2(g) Fast The target rate law is rate = k (NO2)2 The target reaction is 2NO2(e) 2NON + O2) A. Write the rate law expected for this mechanism: B. What is the rate-determining step? C. What is the overall balanced equation for this mechanism? D. If there is/are a reactive intermediate(s), which is/are they? E....
10. Consider the reaction that takes place via the mechanism below; STEP I: NO2(g) + CO(g) - NO(g) + CO2(e) (fast) STEP II: NO) + Cl2(e) - NOC12(e) (slow) Determine; (a) The reaction intermediate(s) (2 points) command (b) The rate determining step (2 points)
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