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 = k[NO2Cl]2 |
| Rate = k[NO2]2[Cl2] |
| Rate = k[NO2][Cl2] |
| Rate = k[NO2Cl][Cl] |
| Rate = k[NO2]2[Cl]2 |
Homework Answers
rate
of reaction depends on the slow step of reaction.The slow step is
also called as rate determining step.In this mechanism of reaction
first step is slow hence rate of overall reaction depends on the
reactants in slow step of reaction.
Add Answer to:
Part A
Given the following proposed mechanism, predict the rate law for
the overall reaction.
2...
Given the following proposed mechanism, predict the rate law for the overall reaction. A_2 + 2B...
Given the following proposed mechanism, predict the rate law for the overall reaction. A_2 + 2B rightarrow 2AB (overall reaction) A) Rate = k[A][B] B) Rate = k[A_2][B] C) Rate = k[A_2][B]^1/2 D) Rate = k[A_2] E) Rate = k[A_2]^1, 2 [B]
1. The following is a proposed mechanism for the gas phase decomposition of nitryl chloride: 2...
1. The following is a proposed mechanism for the gas phase decomposition of nitryl chloride: 2 NO2Cl → 2 NO2 + Cl2. step 1: NO2Cl → NO2+CI step 2: NO2CI+ Cl → NO2 + Cl2 a. (1 pt) Is there an intermediate? If so, what is it? b. (1 pt) Is there a catalyst? If so, what is it? C. (1 pt) Determine the net reaction for the mechanism. d. (2 pt) Use the reaction coordinate diagram below to determine...
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-]
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3. Use the proposed reaction mechanism to answer the following questions; Elementary 1: 2NO2Cl <---> ClO2...
3. Use the proposed reaction mechanism to answer the following questions; Elementary 1: 2NO2Cl <---> ClO2 + N2O + ClO Elementary 2: N2O + ClO2 <---> NO2 + NOCl Elementary 3: NOCl + ClO ---> NO2 + Cl2 a) What is the overall (reduced) reaction? b) Identify any intermediates. c) Determine the rate law expression for each elementary reaction. (fast) (fast) (slow)
For the overall reaction below, which of the following is the correctly written rate law? Overall...
For the overall reaction below, which of the following is the correctly written rate law? Overall reaction: O3(g)+2NO2(g)→N2O5(g)+O2(g) Step 1: O3(g)+NO2(g)→NO3(g)+O2(g) slow Step 2: NO3(g)+NO2(g)→N2O5(g) fast View Available Hint(s) For the overall reaction below, which of the following is the correctly written rate law? Overall reaction: Step 1: slow Step 2: fast A.] Rate=k[O3][NO2]2 B.] Rate=k[O3][NO2] C.] Rate=k[NO3][NO2] D.] Rate=k[O3][NO2]2[N2O5][O2]
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).
The following mechanism has been proposed for the gas-phase reaction of chloroform (CHCl3) and chlorine. Cl2...
The following mechanism has been proposed for the gas-phase reaction of chloroform (CHCl3) and chlorine. Cl2 ⇌ 2Cl (fast, reversible) Cl + CHCl3 → HCl + CCl3 (slow) Cl + CCl3 → CCl4 (fast) What rate law does this mechanism predict? (Choose from the list below and enter your answers in alphabetical order, e.g. ABC ). A)k G) [CHCl3]1/2 M) [CCl3]2 B) [Cl2] H) [CCl3]1/2 N) [HCl]2 C) [Cl] I) [HCl]1/2 O) [Cl2]2 D) [CHCl3] J) [Cl2]1/2 P) [Cl]2 E)...
33 5 points The thermal decomposition of nitryl chloride (NO2Cl) as shown below, 2NO+2NO2 + Cl2...
33 5 points The thermal decomposition of nitryl chloride (NO2Cl) as shown below, 2NO+2NO2 + Cl2 is thought to occur as follows: NO2Cl + NO2 + CI (slow step) NO2CI+ CI+NO2 + Cl2 (fast step) The rate law derived from the above mechanism would be: O rate = k[NO2Cl] O rate = k[NO2Cl][CI] O rate = k[NO2][Cl] o rate = k[NO2Ci] O rate = k[NO21[Cl2] Previous
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)
Given the following proposed mechanism, predict the rate law for the overall reaction. A_2 + 2B rightarrow 2AB (overall reaction) A) Rate = k[A][B] B) Rate = k[A_2][B] C) Rate = k[A_2][B]^1/2 D) Rate = k[A_2] E) Rate = k[A_2]^1, 2 [B]
1. The following is a proposed mechanism for the gas phase decomposition of nitryl chloride: 2 NO2Cl → 2 NO2 + Cl2. step 1: NO2Cl → NO2+CI step 2: NO2CI+ Cl → NO2 + Cl2 a. (1 pt) Is there an intermediate? If so, what is it? b. (1 pt) Is there a catalyst? If so, what is it? C. (1 pt) Determine the net reaction for the mechanism. d. (2 pt) Use the reaction coordinate diagram below to determine...
33 5 points The thermal decomposition of nitryl chloride (NO2Cl) as shown below, 2NO+2NO2 + Cl2 is thought to occur as follows: NO2Cl + NO2 + CI (slow step) NO2CI+ CI+NO2 + Cl2 (fast step) The rate law derived from the above mechanism would be: O rate = k[NO2Cl] O rate = k[NO2Cl][CI] O rate = k[NO2][Cl] o rate = k[NO2Ci] O rate = k[NO21[Cl2] Previous
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