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10. Consider the reaction that takes place via the mechanism below; STEPI: 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)...
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)
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....
If the mechanism behind the reaction NO2(g) + CO(g) Ó NO(g) + CO2(g) is : 1-...
If the mechanism behind the reaction NO2(g) + CO(g) Ó NO(g) + CO2(g) is : 1- 2NO2(g) à 2NO(g) + O2(g) (slow) 2- NO(g) + CO(g) + O2(g) à NO2(g) + CO2(g) (fast) Then its rate law is: A) Rate = k [NO2] . [CO] B) Rate = k [NO2] . [CO2] C) Rate = k [NO 212 D) Rate = k [co]2
The reaction 2 NO2 --> 2 N2 + O2 follows the mechanism: Step 1: NO2 --NO...
The reaction 2 NO2 --> 2 N2 + O2 follows the mechanism: Step 1: NO2 --NO NO3 NO2 SLOW + + Step 2: NO3 CO FAST NO2 CO2 -> + What is the intermediate in the reaction? none of these NO2 ONO3 OOOO
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.
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)...
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...
The thermal decomposition of NO2: 2 NO2(g) → 2 NO(g) + O2(g) takes place in two steps: (1)...
The thermal decomposition of NO2: 2 NO2(g) → 2 NO(g) + O2(g) takes place in two steps: (1) 2 NO2(g) → NO3(g) + NO(g) (slow) (2) NO3 → NO(g) + O2(g) (fast) Which of the following statements is true? a. Rate = k [NO2] b. The reaction is second order in NO2. c. The reaction is first order in O2. d. Increasing [NO2] has no effect on reaction rate. e. All the above.
For the reaction 2 NO(g) + Cl2(g) → 2 NOCl(g) a possible mechanism is (1) NO...
For the reaction 2 NO(g) + Cl2(g) → 2 NOCl(g) a possible mechanism is (1) NO + Cl2 ⇆ NOCl2 fast (2) NOCl2 + NO → 2 NOCl slow What is the rate law for this mechanism? (Enter an answer in the form k[A][B]^2^, where the appropriate chemical species replace A and B, and the correct orders are indicated.) Enter a formula by surrounding subscripts with underscore "_" and superscripts with carat "^" characters. For example, H3O+ would be entered...
The reaction rate of CO and NO2 in the reaction CO(g) + NO2(g) → CO2(g) +...
The reaction rate of CO and NO2 in the reaction CO(g) + NO2(g) → CO2(g) + NO(g) is measured using the initial rates method. The results are tabulated below. [CO] (mol/L) NO2 (mol/L) -([CO]/Δt (mol/L·s) 8.00 10-4 5.50 10-4 8.40 10-8 8.00 10-4 7.78 10-4 1.68 10-7 1.60 10-3 5.50 10-4 1.68 10-7 Determine the rate expression and calculate the rate constant for the reaction.
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)
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....
If the mechanism behind the reaction NO2(g) + CO(g) Ó NO(g) + CO2(g) is : 1- 2NO2(g) à 2NO(g) + O2(g) (slow) 2- NO(g) + CO(g) + O2(g) à NO2(g) + CO2(g) (fast) Then its rate law is: A) Rate = k [NO2] . [CO] B) Rate = k [NO2] . [CO2] C) Rate = k [NO 212 D) Rate = k [co]2
The reaction 2 NO2 --> 2 N2 + O2 follows the mechanism: Step 1: NO2 --NO NO3 NO2 SLOW + + Step 2: NO3 CO FAST NO2 CO2 -> + What is the intermediate in the reaction? none of these NO2 ONO3 OOOO
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