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:
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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
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...
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...
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-]
y courses CHEM 1C-A-M20 Week 6 Cumulative Exa ered 5.00 Consider the following reaction mechanism: 2 NO,CI = clo, + N2O + Clo fast N20 + clo, = NO2 + NOCI fast NOCI + ClO – NO, + Cl2 slow tion What is the rate law for this reaction mechanism? Select one: a. rate = k [N,0] [C10,] (CIO) [No,j' b. rate = k [Noci) [NO_ch? (cio,' [N,01" c. none of the listed answer choices d. rate = k [NO_ch?(no,j?...
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]
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...
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 =...
consider the aqueous reaction of Cl2 + H2S -> S + 2HCL . It may happen by the following mechanism 1: Cl2-> <- 2Cl fast 2: Cl+H2S -> <- HCl + HS fast 3: HS +Cl --> --< HCl + S slow DERIVE a rate law for overall reaction using the given mechanism and rate determining step without using intermediates in the rate law.
At 35°C, K =2.0 x 10-8 for the reaction 2 NOCI(9) = 2 NO(g) + Cl2(9) Calculate the concentrations of all species at equilibrium for each of the following original mixtures. a. 2.2 moles of pure NOCI in a 2.0-L flask [NOCI) = M [NO] = | М [Cl] = M b. 1.0 mole of NOCI and 1.0 mole of NO in a 1.0-L flask [NOCI) = M [NO] = M (Cl2] = 1 M c. 2.0 mole of NOCl...