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 as H_3_O^+^.
Homework Answers
The fast step (equilibrium step) is
The equilibrium constant 
Rearrange above equilibrium constant expression
... ...(1)
The slow step (rate determining step) is
The rate law expression is
rate 
... ...(2)
Substitute equation (1) in equation (2)
rate 
rate 
rate 
where 
Hence, the answer is
rate =k' [NO]^2[Cl_2]^2
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For the reaction 2 NO(g) + Cl2(g) → 2 NOCl(g) a possible
mechanism is (1) NO...
Consider the reaction 2 NO + Cl2 → 2 NOCI A possible mechanism is: Cl2 ⇄...
Consider the reaction 2 NO + Cl2 → 2 NOCI A possible mechanism is: Cl2 ⇄ 2 Cl (fast) Cl + NO → NOCl (slow) If this is correct, the rate law will be: A. rate = k [NO]0.5[Cl] B. rate = k [NO]2[Cl2] C. rate = k [NO][Cl2] D. rate = k [NO][Cl]2 E. rate = k [NO][Cl2]0.5
At 300 K, the following reaction is found to obey the rate law of Rate =...
At 300 K, the following reaction is found to obey the rate law of Rate = k[NOCl]^2: 2 NOCl(g) 2 NO(g) + Cl2(g) The following reaction mechanism has been proposed for the reaction above: Proposed Mechanism: NOCl(g) ->NO(g) + Cl(g) slow Cl(g) + NOCl(g) -> NOCl(g) fast NOCl2(g) -> NO(g) + Cl2(g) fast 21. The suggested rate law in the mechanism is Rate = k[NOCl]. (T) 22. The reaction mechanism is plausible. (F) 23. NOCl2 is a catalyst in...
Consider the reaction 2 NO + Cl2 + 2 NOCI A possible mechanism is: Cl2 =...
Consider the reaction 2 NO + Cl2 + 2 NOCI A possible mechanism is: Cl2 = 2 CI (fast) CI + NO NOCI (slow) If this is correct, the rate law will be: O A. rate = k [NO]?[C12] B. rate = k [NO][C12] C. rate = k [NO][CIT? D. rate = k [NO][C1270.5 E. rate = k [NO]0.5[CI] Reset Selection
NOCl decomposes by the following reaction: 2NOCl (g) --> 2 NO (g) + Cl2 (g). THe...
NOCl decomposes by the following reaction: 2NOCl (g) --> 2 NO (g) + Cl2 (g). THe table below is collected at the same temperature. Time (s) 0 10 20 30 40 [NOCl] 0.0800 M 0.0606 M 0.0488 M 0.0408 M 0.0350 M how would you find the rate law for this reaction and what is the rate law? also what is the concentration of NOCl after 60 seconds?
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)...
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; STEPI: NO2(g) + CO(g) → NO(g) + CO2(e) (fast) STEP II: NO(8) + Cl2(e) → NOCl2(g) (slow) Determine; (a) The reaction intermediate(s) (2 points) (b) The rate determining step (2 points)
The equilibrium constant, Kc, for the reaction 2 NOCl (g) ⇄ 2 NO (g) + Cl2...
The equilibrium constant, Kc, for the reaction 2 NOCl (g) ⇄ 2 NO (g) + Cl2 (g) is 2.4 x 10-7. What is the equilibrium constant for the reaction Cl2 (g) + 2 NO (g) ⇄ 2 NOCl
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)
5. The reaction 2NO+ Cl2 → 2NOCI is thought to occur in two steps, as shown...
5. The reaction 2NO+ Cl2 → 2NOCI is thought to occur in two steps, as shown by the following proposed mechanism: O NO + Cl2 NOCI (fast, at equilibrium) (i) NO + NOCI, → 2NOCI (slow) What rate law does this mechanism predict? Select the best choice by circling it. a. rate = ** [NO]?[NOCI] rate = *, [NO]2 C. rate = [NOCL] d. rate = kek [NO](C1,12 rate = [NO] f. rate = kaka [NO]+[C12] g. rate = kak2...
A compare? rate Coastant at 1.000 x 10k, and 2. The reaction CO(g) + Cl2 →...
A compare? rate Coastant at 1.000 x 10k, and 2. The reaction CO(g) + Cl2 → COCl2(g) Has the reaction mechanism Cl + CO=COCI fast Cl2 + COCl → COC12 + Cl slow a. List the intermediates in the reaction mechanism. b. The order of the overall reaction is 5/2. Determine the rate law for the reaction. (Many steps are required)
Consider the reaction 2 NO + Cl2 + 2 NOCI A possible mechanism is: Cl2 = 2 CI (fast) CI + NO NOCI (slow) If this is correct, the rate law will be: O A. rate = k [NO]?[C12] B. rate = k [NO][C12] C. rate = k [NO][CIT? D. rate = k [NO][C1270.5 E. rate = k [NO]0.5[CI] Reset Selection
10. Consider the reaction that takes place via the mechanism below; STEPI: NO2(g) + CO(g) → NO(g) + CO2(e) (fast) STEP II: NO(8) + Cl2(e) → NOCl2(g) (slow) Determine; (a) The reaction intermediate(s) (2 points) (b) The rate determining step (2 points)
5. The reaction 2NO+ Cl2 → 2NOCI is thought to occur in two steps, as shown by the following proposed mechanism: O NO + Cl2 NOCI (fast, at equilibrium) (i) NO + NOCI, → 2NOCI (slow) What rate law does this mechanism predict? Select the best choice by circling it. a. rate = ** [NO]?[NOCI] rate = *, [NO]2 C. rate = [NOCL] d. rate = kek [NO](C1,12 rate = [NO] f. rate = kaka [NO]+[C12] g. rate = kak2...
A compare? rate Coastant at 1.000 x 10k, and 2. The reaction CO(g) + Cl2 → COCl2(g) Has the reaction mechanism Cl + CO=COCI fast Cl2 + COCl → COC12 + Cl slow a. List the intermediates in the reaction mechanism. b. The order of the overall reaction is 5/2. Determine the rate law for the reaction. (Many steps are required)
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