Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
expand_more
expand_more
format_list_bulleted
Related questions
Question
Transcribed Image Text:1) Write a basic form of the rate law for the following reaction.
ClO4 + 8Br + 8H* → Cl + 4B12 + 4H2O
Rate
Expert Solution
arrow_forward
Step 1
Reaction: ClO4 + 8Br + 8H+ Cl+ 4Br2 + 4H2O
From rate low of the reaction,
rate = K[ClO4][Br ]8[H+]8
Where, [ClO4] = concentration of the ClO4-
[Br ] = concentration of the Br
[H+] = concentration of the H+
k = rate constant
Step by stepSolved in 2 steps
Knowledge Booster
Similar questions
- For the reaction 2 HI(g)→ H₂(g) + I2(g) at 427 K, the following data are collected. Time (s) [HI] (M) 0 0.20 0.15 0.12 0.10 0.08 0.07 0.06 0.06 0.05 0.05 0.04 1000 2000 3000 4000 5000 6000 7000 8000 9000 10000 Make plots necessary to evaluate if the rate law is zeroth, first or second order.arrow_forwardSuppose also k₁<arrow_forwardSuppose the decomposition of ozone proceeds by the following mechanism: step elementary reaction rate constant 1 03(g) O₂(g) + 0(g) k₁ 2 03(g) + O(g) → 20₂(g) k₂ Suppose also k₁ »k₂. That is, the first step is much faster than the second. Write the balanced chemical equation for the overall chemical reaction: Write the experimentally- observable rate law for the overall chemical reaction. rate = k Note: your answer should not contain the concentrations of any intermediates. Express the rate constant k for the overall chemical reaction in terms of K₁, K2, and (if necessary) the rate constants k.1 and k-2 for the reverse of the two elementary reactions in the mechanism. = 0 k = 00 X 5 S ?arrow_forward
- For the following reaction Mechanism write the overall reaction and write the rate law. H3O++ I- → HI + H2O (fast) H2O2 + HI → H2O + HOI (fast) HOI + H3O++ I- →2H2O + I2 (slow) I2 + I- → I3-(fast)arrow_forwardAt a given temperature, a first-order reaction has a rate constant of 1.5 × 10–3 s–1. What is the time required for the reaction to be 32% completed?arrow_forwardPlease don't provide handwritten solutionarrow_forward
- The reaction described by H, (g) + L,(g) 2 HI(g) has an experimentally determined rate law of rate = k [H2] [I2] Some proposed mechanisms for this reaction are: Mechanism A k1 (1) H,(g) + L,(g) → 2 HI(g) (one-step reaction) Mechanism B k1 =2 I(g) k_1 (1) L(g) ; (fast, equilibrium) k2 (2) H, (g) + 2 I(g) 2 HI(g) (slow) Mechanism C k1 = 2 I(g) (fast, equilibrium) (1) k2 (2) I(g) + H, (g) HI(g) + H(g) (slow) (3) H(g) + I(g) → HI(g) (fast) Question Sourcarrow_forwardConsider the following reaction: 2MnO4–(aq) + 10Br–(aq) + 16H3O+(aq) --> 2Mn2+(aq) + 5Br2(aq) + 24H2O(l) In a reaction under a certain condition, if the rate for the formation of Br2 (D[Br2]/Dt) is 1.0 x 10–5 mol ‧ L–1 ‧ s–1, what is the rate for the disappearance of 2MnO4– (-D[MnO4–]/Dt) in mol ‧ L–1 ‧ s–1 ? (A) 1.0 x 10–5 (B) 4.0 x 10–6 (C) 2.5 x 10–6 (D) 2.5 x 10–5arrow_forwardThe rate law for the reaction: NH4+ + NO₂ N₂ + 2H₂O is rate =k[NH4+][NO₂] It is found that the rate constant for this reaction is 3.05x10-4 M-1s-1. Calculate the rate of the reaction, including units, if [NH4*] is 0.265M and [NO₂] is 0.0803M. Attach File Browse Local Filesarrow_forward
- Suppose the formation of nitrogen dioxide proceeds by the following mechanism: elementary reaction 2NO (g) → N₂O₂ (g) step 1 2 N₂O₂(g) + O₂ (g) Write the balanced chemical equation for the overall chemical reaction. Write the experimentally- observable rate law for the overall chemical reaction. 2NO₂ (g) Suppose also k₁ « k₂. That is, the first step is much slower than the second. << Note: your answer should not contain the concentrations of any intermediates. rate constant 0 k₁ k₂ rate = k 1-0 010 X Sarrow_forwardPlease answer the questionarrow_forward
arrow_back_ios
arrow_forward_ios
Recommended textbooks for you
- ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
ChemistryChemistryISBN:9781259911156Author:Raymond Chang Dr., Jason Overby ProfessorPublisher:McGraw-Hill Education
Principles of Instrumental AnalysisChemistryISBN:9781305577213Author:Douglas A. Skoog, F. James Holler, Stanley R. CrouchPublisher:Cengage Learning 
Organic ChemistryChemistryISBN:9780078021558Author:Janice Gorzynski Smith Dr.Publisher:McGraw-Hill Education
Chemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage Learning
Elementary Principles of Chemical Processes, Bind...ChemistryISBN:9781118431221Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. BullardPublisher:WILEY
Chemistry
Chemistry
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Chemistry
Chemistry
ISBN:9781259911156
Author:Raymond Chang Dr., Jason Overby Professor
Publisher:McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:9781305577213
Author:Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:Cengage Learning
Organic Chemistry
Chemistry
ISBN:9780078021558
Author:Janice Gorzynski Smith Dr.
Publisher:McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:Cengage Learning
Elementary Principles of Chemical Processes, Bind...
Chemistry
ISBN:9781118431221
Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:WILEY