5. The reaction 2NO+ Cl2 → 2NOCI is thought to occur in two steps, as shown...
Select all that apply. The rate law for the reaction 2NO(g) + Cl2(g) → 2NOCI(g) is given by R-k[NO][C121 If the following is the mechanism for the reaction, NO(g) + Cl2(g) → NOC12(g) NOCI,(g) + NO(g) → 2NOCI(g) which of the following statements accurately describes this reaction? Check all that apply. 2nd order reaction The first step is the slow step. Doubling [NO] would quadruple the rate. Cutting (Cl) in half would decrease the rate by a factor of two....
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
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
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...
Chapter 13, Question 9 For the reaction 2NO + Cl2 + 2NOCI, do the following: Express the rate in terms of the disappearance of Cl2. Rate = _ A[cz] Rate=(-)(A[cz] 4) LINK TO TEXT We were unable to transcribe this imageIf Cl2 reacts at a rate of 79 M/s, state how fast NOCI will form. M/s exact number, no tolerance
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
63. At 35°C, K = 1.6 x 10-6 for the reaction 2NOCI(9) = 2NO(g) + Cl2 (9) Calculate the concentrations of all species at equilibrium for each of the following original mixtures. a. 2.0 moles of pure NOCI in a 2.0-L flask Answer b. 1.0 mole of NOCI and 1.0 mole of NO in a 1.0-L flask Answer c. 2.0 moles of NOCI and 1.0 mole of Cl, in a 1.0-L flask
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...
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...
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 =...