Rate data were collected for the following reaction at a particular temperature. (C2H5)2(NH)2 + 12 = (C2H5)2N2 + 2HI Expt Initial [(C2H5)2(NH)2], Initial [12], mol/L Reaction Rate, Ms-1 mol/L 1 0.10 0.10 0.0090 2 0.20 0.10 0.036 3 0.10 0.20 0.018 4 0.10 0.30 0.027 Write the overall rate law expression and determine the order of reaction of (a) (C2H5)2(NH)2, (b) 12, (c) overall order of reaction, and (d) the rate constant.

Rate data were collected for the following reaction at a particular temperature. (C2H5)2(NH)2 + 12 = (C2H5)2N2 + 2HI Expt Initial [(C2H5)2(NH)2], Initial [12], mol/L Reaction Rate, Ms-1 mol/L 1 0.10 0.10 0.0090 2 0.20 0.10 0.036 3 0.10 0.20 0.018 4 0.10 0.30 0.027 Write the overall rate law expression and determine the order of reaction of (a) (C2H5)2(NH)2, (b) 12, (c) overall order of reaction, and (d) the rate constant.

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...

See similar textbooks

Similar questions

Arrange the following compounds in order of increasing reaction rate with HNO3/H2SO4. 1. C6H5CH=O II. C6H5OCH3 III. C6H5Br IV. C6H5CH3 O I
Which rate law fits with this mechanism? 2NO --> N2O2 fast step 1 N2O2 + H2 --> N2O + H2O slow step 2 N2O + H2 --> N2 + H2O fast step 3 Question 9 options: rate = k [NO] [N2O2] [H2] rate = k [NO] rate = k [NO]2 [N2O2] [H2] rate = k [NO] [H2] rate = k [NO]2 rate = k [N2O2] [H2] rate = k [NO]2 [H2] [N2O2] rate = k [NO]2 [H2]
When fitting data to a best fit line, a correlation coefficient (R2) is determined and used to evaluate the quality of fit. The best fit of the data will have an R² value closest or equal to zero (0). closest or equal to one (1). equal to the rate of the reaction occurring. equal to the rate constant of the reaction occurring.
Please help me with question 3 and 4. Thank you.
Please explain how to find rate constant (k) if reaction rate = 3.40*10^-7 I^- molar = .00200 (reaction order 1) BrO3^- molar = .00800 (reaction order 1) H^+ molar = .0400 (reaction order 2)
The following initial rate data are for the reaction of tertiary butyl bromide with hydroxide ion at 55 °C: (CH3)3CB + OH → (CH3)3COH + Br Experiment [(CH3)3CB1],, M [OH], M Initial Rate, Ms-1 1 0.890 1.50x10-3 1.50x10-3 3.01x10-3 3.01x10-3 0.118 0.118 2 1.78 0.890 1.78 3 0.237 4 0.237 Complete the rate law for this reaction in the box below. Use the form k[A]j™[B]" , where '1' is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or n Rate = From these data, the rate constant is
Please answer all parts
Do d(iii) as fast as possible. I upvote
The reaction mechanism is given below. elementary step 1 : Br2 ⇋ 2Br fast elementary step 2: H2 + Br à HBr + H slow rate determining step elementary step 3: H + Br2 à HBr + Br fast Overall reaction is H2 + Br2 à 2HBr k1 is the forward reaction rate constant of step 1, k-1 reverse reaction rate constant of step 1, k2 for reaction rate constant of step 2 and k3 for reaction rate constant of step 3. What is the molecularity of step 2? Give the chemical formula of the intermediate(s) in the reaction Deduce the rate law in terms of the reagents for the reaction using the elementary steps.
2NO2(g) + F2(g) -> NO2F(g) H°rxn = -284 kJ/molrxn NO2(g) and F2(g) can reactto produce NO2F(g), as represented above. A proposed mechanism for the reaction has two elementary steps, as shown below. Step 1: NO2 + F2 -> NO2F + F (slow) Step 2: NO2 + F -> NO2F (fast) a.) Write a rate law for the overall reaction that is consistent with the proposed mechanism. b.) On the incomplete reaction energy diagram below, draw a curve that shows the following two details. The relative activation energies for the two elementary steps The enthalpy change of the overall reaction Can all of them be solved please, and thank you very much!
Given the following data for the NH4+ + NO2- → N2 + 2H2O reaction Trial [NH4+] [NO2-] Rate 1 0.015 M 0.020 M 0.020 M/s 2 0.030 0.020 0.040 3 0.015 0.010 0.005 If the rate of formation of NO2 is 5.5 x 10-4, the rate of the reaction is _________.
0 State what rate law you would expect from this mechanism (Rate = k[Acetone]"[H*]"[[₂]') • Compare the expected rate law from the mechanism to the rate law you got from the Method of Initial rates and the Method of Isolation. If they are different, suggest 1-2 valid, specific, experimental reasons why they might be different. (fast, equilibrium) CH3 ソース H3C ག་ CH3 + H* = H3C H3C H. + H (slow) CH3 H3C CH2 + ↳2 Т + HI