**Transcript for Educational Website:**---**Chemical Kinetics Problem:**This question has multiple parts. Work all the parts to get the most points.**a.** The rate law for the reaction\[ 2 \text{NOBr}(g) \rightarrow 2 \text{NO}(g) + \text{Br}_2(g) \]at some temperature is\[ \text{Rate} = -\frac{\Delta [\text{NOBr}]}{\Delta t} = k[\text{NOBr}]^2 \]If the half-life for this reaction is 2.00 s when \([\text{NOBr}]_0 = 0.90 \, \text{M}\), calculate the value of \(k\) for this reaction.\[ k = \, \_\_\_ \, \text{L/mol·s} \]**Options:**- **Submit**: Submit your answer.- **Retry Entire Group**: Retry the entire group of questions. 9 more group attempts remaining. - **Show Hint**: Click to get a hint.*Note: This example is from Cengage Learning's online platform, OWLv2.*_Email Instructor_ link is available for further queries.--- This transcription provides essential information about solving the kinetics problem, focusing on calculating the rate constant \(k\) given the rate law and half-life data.

Answered: Image /qna-images/answer/cc6ac048-7586-443e-8763-21a986af7608.jpg

a The rate law for the reaction rogress 2NOBr(g) → 2NO(g) + Br2 (g) at some temperature is ΔΙΝΟΒ Rate = - = k[NOB1]² At If the half-life for this reaction is 2.00 s when [NOB1]o= 0.90 M, calculate the value of k for this reaction. k = L/mol·s Submit

a The rate law for the reaction rogress 2NOBr(g) → 2NO(g) + Br2 (g) at some temperature is ΔΙΝΟΒ Rate = - = k[NOB1]² At If the half-life for this reaction is 2.00 s when [NOB1]o= 0.90 M, calculate the value of k for this reaction. k = L/mol·s Submit

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

3. The rate equation for the decomposition of N2O5(g) (forming NO2(g)) is: A[NO2]/At = k[N2O5]. The value of k is 5.0 × 10-4 s-' for the reaction at a particular temperature. a) Calculate the half-life of N2Os(g) at that temperature. b) How long does it take for [N2O5] to decrease to one tenth of its original value?
Consider this reaction: →H2CO3aq+H2OaqCO2aq At a certain temperature it obeys this rate law.rate =·0.0579M−1s−1H2CO32 Suppose a vessel contains H2CO3 at a concentration of 0.820M. Calculate the concentration of H2CO3 in the vessel 280.seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. =___M
In aqueous solution, CIO reacts to produce CIO3 and CI", according to the following chemical equation. 3 CIÓ (ag) → CIO3¯ (ag) + 2 CI- (aq) A plot of 1/[CIO ] vs. time is linear, with a slope equal to 0.056 M-1s-1. If the initial concentration of CIO- is 0.56 M, how long will it take for half of the ClIO to react? 27 sec O 12 sec O 32 sec O 0.036 sec O 7.1 sec
Please help with HW problem.
5.) For the reaction X + Y ↓ Z; the reaction rate is found to depend only upon the concentration of X. A plot of 1/[X] verses time gives a straight line. What is the rate law for this reaction?
Consider this reaction: 2NH, (g) - N2 (g) +3H, (g) At a certain temperature it obeys this rate law. rate =(0.0103 s")[NH,] S Suppose a vessel contains NH, at a concentration of 0.170M. Calculate the concentration of NH, in the vessel 68.0 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. OM x10
A certain reaction has the following rate law: rate = k[X]³[Y]² Which of the following are the correct units for k? Select one: L³mol-3s-1 Ms-1 M³s O L?mol2s1 L5mol 5s1 Lmol-'s mol³L-3s-1 M's-1 L*mol-4s-1 mol?L-2s1
Question 17 of 23 Submit Butadiene reacts to form a dimer according to the equation 2C,H6(g) → C3H12(g) The reaction obeys the second order rate law, Rate = k[C,H,]?, with a rate constant k = 3.68 M-'min at a certain temperature. Starting with an initial concentration of [C,H] = 0.0500 M, what will be the butadiene concentration after 31.0 min? | M 1 2 3 C 7 9. +/- x 10 0 LO 00
Consider this reaction: 2N,03 (g) → 2N,04 (g) + O, (g) At a certain temperature it obeys this rate law. rate = (0.0268 M.s)[N,0 S. Suppose a vessel contains N,0, at a concentration of 1.00M. Calculate how Ol long it takes for the concentration of N,0, to decrease to 0.130M. You may assume no other reaction is important. Round your answer to 2 significant digits. ]x10
Question is attached.