lmine the rate law for the production of nitrosyl fluoride (NO,F) that occurs according to the following balanced chemical equation: 2 NO, (g) + F2 (g) > 2 NO,F (B) The following data were obtained from varying the concentrations of the reactants: [NO.) (M) 0.00130 0.00259 Initial Rate (M/s) 2.16 х 101 4.30 x 104 2.61 х 104 5.22 x 10 [F] (M) Run 1 0.00479 Run 2 0.00479 Run 3 0.00612 0.00123 Run 4 0.00612 0.00246 (A) Rate = k (NO] [F2] Rate = k (NO2)'(Fa] Rate = k (NO2) Rate - k (NO,J'(F]05 Rate = k (NO2] [F10s (E)

lmine the rate law for the production of nitrosyl fluoride (NO,F) that occurs according to the following balanced chemical equation: 2 NO, (g) + F2 (g) > 2 NO,F (B) The following data were obtained from varying the concentrations of the reactants: [NO.) (M) 0.00130 0.00259 Initial Rate (M/s) 2.16 х 101 4.30 x 104 2.61 х 104 5.22 x 10 [F] (M) Run 1 0.00479 Run 2 0.00479 Run 3 0.00612 0.00123 Run 4 0.00612 0.00246 (A) Rate = k (NO] [F2] Rate = k (NO2)'(Fa] Rate = k (NO2) Rate - k (NO,J'(F]05 Rate = k (NO2] [F10s (E)

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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The differential rate laws for the balanced chemical reaction: aA(aq) + bB (aq) + CC (aq) → product is given by: raterxn = k [A]³[C]³ [B]³ What are the order in each chemical, as well as the overall order of the chemical kinetics? Place your answer in each box, respectively! Provide detailed solution (The order of kinetics in A) = (The order of kinetics in B) = (The order of kinetics in C) = (The overall order of kinetics) =
Consider this reaction: 2N₂O5 (g) → 2N₂O4 (g) + O₂(g) At a certain temperature it obeys this rate law. = (0.291 M¹s¹) [N₂0₂] rate Suppose a vessel contains N₂O, at a concentration of 0.230 M. Calculate how long it takes for the concentration of N₂O to decrease to 23.0% of its initial value. You may assume no other reaction is important. Round your answer to 2 significant digits. ? Subm Continue Ⓒ2022 McGraw Hill LLC. All Rights Reserved. Terms of Use Privacy Cente 80°F Partly sunny ^ pe here to search B X G
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Consider the hypothetical reaction: A + B + 20 → 2D + E where the rate law is Rate = -AL4 = k[AJ[B]2 At An experiment is carried out where [A]o = 7.200 x 102 M, [B]o = 2.500 M and [C], = 2.500 M. The reaction is started, and after 11.60 seconds, the concentration of A is 2.200 x 10° M. Calculate the value of k for this reaction in units of M²sª. Answer: 37.987 The correct answer is: 0.04811
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In a study of the decomposition of hydrogen iodide on a gold surface at 150 °C HI(g)% H2(g) + ½ I½(g) the concentration of HI was followed as a function of time. It was found that a graph of [HI] versus time in seconds gave a straight line with a slope of -1.91×10-4 Ms and a y-intercept of 0.235 M. Based on this plot, the reaction is reaction is order in HI and the rate constant for the Ms!
2 A(aq) + 3 B(aq) A2B3(aq) An experiment is conducted at 25 C and the rate of appearance of the product ABa(aq) is measured as the concentrations of the reactants were varied. Data from the trials are shown below. Initial Rate of Trial [A] (M) [B] (M) Appearance of A2B3 (M/s) 5.0 x 10 4.5 x 10 1.0 x 10 0.200 0.300 0.200 0.900 0.400 0.300 4 0.135 0.225 ??? Determine the rate law for the reaction. Justify your answer. Determine the value of k, including units. Determine the rate of Trial 4. a. b. с. d. Determine the initial rate of disappearance of A for trial 2. A possible reaction mechanism has a 1" elementary step as shown below: e. A +BAB Could this first step be the rate determining step? Explain your reasoning. In the reaction mechanism the compound MnO2 appears. A student makes the claim f. "The order of MnO2 must be zero since it does not appear in the overall balanced equation". Do you agree or disagree with the student? Explain your reasoning. g. In trial 1, 10 mL of A and 10…
T = Chemical reactions produce one or more product substances from one or more reactant substances. If x molecules of reactant X combine with y molecules of reactant Y to produce z molecules of product Z, we write xX+yY→ ZZ. The reaction rater is the rate of change of concentration of 1 dz 1 dX one of the products over time; for this example, r = 1 dy z dt x dt dY dt dX dt Nitrogen gas N₂ and hydrogen gas H₂ combine to produce ammonia NH3 according to dY dX dt 1N₂ + 3H₂ → 2NH3. Find r, and if ammonia is being produced at a rate of 5 moles dt per liter per hour. = esc T M Question Help: Message instructor Submit Question K 8366-SUMMER2023 / June 5- June 11 / Practice: Derivative mol Lh mol Lh → # C - $ y dt M % O Oll