Option D is the correct answer
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
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?...
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...
step by step Rates of Non-elementary reactions Class Activity Consider the following mechanism: 2NO N202 k-1 NzOz + C12-2+2 NOCI a. What is the net reaction? b. Which of the above species is an intermediate? Why? c. Find the rate of the overall reaction using the steady-state approximation. d. Repeat part (c) using the rate-determining step method, assuming the first-step is fast and at equilibrium and the second step is slow. 2NO N,02 (ast,at equilibrium) k-1 N202 + Cl2-22 NOCI...
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 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-]
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]
select all of the mechanisms that are plausible for a given reaction and it's experimentally determined the rate law. 10.00 points Select all of the mechanisms that are plausible for the given reaction and its experimentally determined rate law. Overall Reaction: 2NO + CI, + 2NOCI Experimentally Determined Rate Law: rate = k[NO][CI] Step 1: NOCI, + NOCI, (slow) Step 2: NOCI, NQ -- 2NÓCI (fast) Step 1: CI, -+ 2Cl (slow) Step 2: 2NO+2CI2NOCI (fast) Step 1: NOCI, NOCI...
23. Consider the reaction: 2 NO (g) C12 (g)-2 NOCI (g) + Suppose a mixture at equilibrium (under standard conditions at 350 K) contains the gases at the following pressures: NO: 0.150 atm Cl2: 0.071 atm NOCI: 14.6 atm Calculate Keq and then use this value to calculate ΔGo at 350 K. 0Jd. -29.2 k e. -14.9 k a. +34.3 kJ b. -34.3 kJ c. -21.0
A reaction mechanism is defined as the sequence of reaction steps that define the pathway from reactants to products. Each step in a mechanism is an elementary reaction, which describes a single molecular event of usually one or two molecules interacting. The rate law for an overall reaction is the rate law for the slowest step in the mechanism, which is directly related to the stoichiometric coefficients of the reactants. The exception to this rule occurs when the slowest step...