Consider the reaction of peroxydisulfate ion (S2Og-) with iodide ion (I¯) in aqueous solution: S,03- (aq) + 31 (aq) → 2 So?-(aq) + I5 (aq) At a particular temperature, the initial rate of disappear- ance of S20- varies with reactant concentrations in the following manner: Experiment [S,0,-](M) [I](M) Initial Rate (M/s) 0.018 0.036 2.6 x 106 0.027 0.036 3.9 x 106 3 0.036 0.054 7.8 x 106 0.050 0.072 1.4 x 10-5 (a) Determine the rate law for the reaction and state the units of the rate constant. (b) What is the average value of the rate constant for the disappearance of S,0,- based on the four sets of data? (c) How is the rate of dis- appearance of S2O3- related to the rate of disappearance of I ? (d) What is the rate of disappearance ofI when [S,0,2-] = 0.025 M and [I-] = 0.050 M? 2.

Consider the reaction of peroxydisulfate ion (S2Og-) with iodide ion (I¯) in aqueous solution: S,03- (aq) + 31 (aq) → 2 So?-(aq) + I5 (aq) At a particular temperature, the initial rate of disappear- ance of S20- varies with reactant concentrations in the following manner: Experiment [S,0,-](M) [I](M) Initial Rate (M/s) 0.018 0.036 2.6 x 106 0.027 0.036 3.9 x 106 3 0.036 0.054 7.8 x 106 0.050 0.072 1.4 x 10-5 (a) Determine the rate law for the reaction and state the units of the rate constant. (b) What is the average value of the rate constant for the disappearance of S,0,- based on the four sets of data? (c) How is the rate of dis- appearance of S2O3- related to the rate of disappearance of I ? (d) What is the rate of disappearance ofI when [S,0,2-] = 0.025 M and [I-] = 0.050 M? 2.

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

Related questions

Q: the following data was obtained for the reaction below at 25.0°C 2 NO(g) + O2(g) --> 2 NO2(g) (see…

Q: Consider the following reactions: A -> B (1) B + M -> C (2) Assume M is present in great excess.…

A: The rate equation derives the relationship between rate of forward reaction to the rate constant and…

Q: Does the instantaneous rate increase, decrease, or remainthe same as the reaction…

A: It is given that, instantaneous rate at time t = slope of tangent to the line at time t Slope of…

Q: the rate at

Q: For the reaction: Bro3 (aq) + 5Br (aq) + 8H*(aq) 3Br2(0) + H20(6) The initial rate of the reaction…

Q: A suggested mechanism for the gas phase decomposition of nitrous oxide is: step 1 slow: N20 –→ N2 +…

A: 1. According to the given mechanism, the overall reaction can be derived by adding two equations:…

Q: None

Q: 3b

A: Given chemical reaction: Average rate of reaction is given by:

Q: The activation energy Ea for a particular reaction is 42.2 kJ/mol. How much faster is the reaction…

A: Answer: This question is based on the Arrhenius equation that gives us relation between activation…

Q: For the reaction at 25.0 oC: N2(g) + H2(g) --- NH3(g) (unbalanced) The rate of disappearance of H2…

Q: a) The concentration of the starting substance A in a reaction A → products decreases according to…

A: OrderRate LawIntegrated Rate LawPlotsSlopeZerothrate = k[A]o - [A]t = kt[A] vs t-kFirstrate =…

Q: C3Hg + 502 →→ 3 CO2 + 4 H2O which of the following is a valid expression for the reaction rate? O…

Q: The data below were collected for the following reaction: 2 NO2 (g) + F2 (g) - 2 NO2F (9) Expt (NO2]…

A: We have to calculate the rate law.

Q: What is the rate constant k (with the correct unit) for the reaction having the same kinetic data as…

A: Consider the given reaction as; H2O2 aq + 3I- aq + 2 H+ aq → I3- aq + 2H2O l Rate =k H2O2α I-β H+γ…

Q: k 3) For the reaction NO2+ C0 → NO + CO2, the dependence of the rate constant 4 on temperature is…

A: The graph lnk vs 1/T is shown below.

Q: 6. Consider the reaction: 2A +B D This reaction was analyzed in the lab and the following data was…

Q: Dinitrogen pentaoxide, N₂O5, decomposes to nitrogen dioxide, NO2 and oxygen, O₂ as shown in the…

A: We are given the concentration of the reactant, N2O5(g), and initial rate data at 25 oC. Suppose…

Q: Consider the reaction described by the equation C₂H₂Br₂(aq) +31-(aq) - - The rate law is rate =…

Q: 2. Consider the following reactions: A -> B (1) B + M -> C (2) Assume M is present in great…

A: In the given problem we need to first figure out the rate equations. Based on that the relation…

Q: The reaction A(aq) + B(aq) → Products(aq) was studied, and the following data were obtained: [A]o…

A: Answer:The power of the concentration term of a reactant in rate law is equal to the order of…

Q: The differential rate law for the balanced chemical reaction: aA (aq) +bB (aq) + cC (aq) -->…

A: The rate of reaction is given as

Q: Consider the reaction described by the equation C₂H₂Br₂(aq) +31 (aq) → C₂H₂(g) + 2 Br (aq) + 15 (aq)…

A: The objective is to determine the missing entries in the given table.GivenThe reaction is…

Q: For a reaction A products, sicessive half_For a reaction A→ products, successive half-lives are…

A: Step 1: Yield of Aspirin:1. Moles of salicylic acid:Molar mass of salicylic acid: 138.12 g/mol.Mass…

Q: Using the data in the table, determine the rate constant of the reaction and select the appropriate…

A: According to bartleby Q and A guidelines i am answering the first one only, please repost remaing…

Q: Please use the values in the resources listed below instead of the textbook values. Consider the…

A: Th reaction : Rate of disappearance of Br-(aq) =

Q: The following reaction is carried out at a certain temperature, which yields the data below.…

A: Given reaction 2ClO2(aq) + 2 OH–(aq) → ClO3–(aq) + ClO2–(aq) + H2O(l) To calculate the…

Q: In the following reaction, 2A+B – 3C + 2D the rate of appearance of D given by (A[D]/At) may also be…

Q: What exactly is question 2 asking to do?

A: The chemical equation is given as follows:

Q: 16). $) How would you by using the data given in the table for question 15 be able to determine a.…

A: As not specified and also question 15 is already done, I am answering question 16. If you need…

Question

Consider the reaction of peroxydisulfate ion (S2Og-)
with iodide ion (I¯) in aqueous solution:
S,03- (aq) + 31 (aq) → 2 So?-(aq) + I5 (aq)
At a particular temperature, the initial rate of disappear-
ance of S20- varies with reactant concentrations in the
following manner:
Experiment [S,0,-](M) [I](M) Initial Rate (M/s)
0.018
0.036
2.6 x 106
0.027
0.036
3.9 x 106
3
0.036
0.054
7.8 x 106
0.050
0.072
1.4 x 10-5
(a) Determine the rate law for the reaction and state the
units of the rate constant. (b) What is the average value
of the rate constant for the disappearance of S,0,-
based on the four sets of data? (c) How is the rate of dis-
appearance of S2O3- related to the rate of disappearance
of I ? (d) What is the rate of disappearance ofI when
[S,0,2-] = 0.025 M and [I-] = 0.050 M?
2.

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

Step 2

Step 3

Step 4

Step 5

Step 6

Step 7

Trending now

This is a popular solution!

Step by step

Solved in 7 steps with 9 images

SEE SOLUTION Check out a sample Q&A here

Similar questions

Please write every step as clear as possible so I can properly understand
10) The following set of data was obtained by the method of initial rates for the reaction: > 10) BrO3-(aq) + 5 Br-(aq) + 6 H+(ag) – 3 Br2(aq) + 3 H20(1). Calculate the initial rate when BrO3- is 0.30 M, Br- is 0.050 M, and H+ is 0.15 M. Expt | [BrO3-], M| [Br-]M | [H+], M Rate, M/s 0.10 0.10 0.10 8.0 x 10-4 0.20 0.10 0.10 1.6 x 10-3 0.20 0.15 0.10 2.4 x 10-3 4 0.10 0.10 0.25 5.0 x 10-3 A) 6.1 × 10-5 M/s B) 2.7 × 10-3 M/s C) 5.3 × 10-2 M/s D) 8.4 × 10-2 M/s four (4) auestions: The relative initial rates of the reaction A2 + B2 - products in vess 1. 3.
A proposed mechanism for the gas phase reaction between nitrogen monoxide and oxygen is as folloWS: step 1 fast: NO + 0,= NO3 step 2 slow: NO3 + NO – 2 NO2 (1) What is the equation for the overall reaction? Use the smallest integer coefficients possible. If a box is not needed, leave it blank. (2) Which species acts as a catalyst? Enter formula. If none, leave box blank: (3) Which species acts as a reaction intermediate?Lnter formula. If none, leave box blank: (4) Complete the rate law for the overall reaction that is consistent with this mechanism. Use the form k[A]™[B]" , where '1' is understood (so don't write it if it's a '1') for m, n etc. Rate =
For the reaction: Bro3 (aq) + 5Br (aq) + 8H*(aq) → 3Br2(f) + H20(6) The initial rate of the reaction has been measured at the reactant concentrations show: Trial [BrO,] [H'] (mol/L) (mol/L) 0.10 [Br] (mol/L) Initial rate (mol/L-s) 1 0.10 0.10 8.0 0.20 0.10 0.10 16 0.10 0.20 0.10 16 0.10 0.10 0.20 32 The rate law expression will be: 234
complete the table.
5:16 Mon, Oct 2 tv Document Sharing User Settings ⠀⠀⠀ The Arrhenius equation shows the relationship between the rate constant k and the temperature T in kelvins and is typically written as - Ea k = Ac exp RT where R is the gas constant, Ac is a constant called the collison or frequency factor, and Ea is the activation energy for the reaction. When comparing rate constant at distinct temperatures, one can formulate the Arrhenius equation also in the following form: k2 Ea 1 1 会-会(*-*) = 六六一六) k1 R where K₁ and k₂ are the rate constants for a single reaction at two different absolute temperatures (T₁ and T₂). Part A The activation energy of a given reaction is 37.7 kJ/mol. At 30 °C, the rate constant is 0.0170s-¹. At what temperature in degrees Celsius would the rate constant for this reaction increase by a factor of 2? Express your answer with the appropriate units. ► View Available Hint(s) T₂ = Submit Part B μA Value | Units HÅ Given that the initial rate constant is 0.0170s-¹ at an…
The following is the experimental data for the rate of reaction: Q (g) + 2T (g) --> T2Q (g) in some conditions Experiment [Q](M) [T](M) V (M/second) 1 0,1 0,1 0,0125 2 0,2 0,1 0,05 3 0,1 0,2 0,1 if [Q] and [T] are changed to 0.5M each, then the reaction rate (v) at that time is?
At a certain temperature the rate of this reaction is second order in NH,OH with a rate constant of 25.4 M s: NH,OH (aq)NH;(aq)+H,0(aq) Suppose a vessel contains NH,OH at a concentration of 1.33 M. Calculate the concentration of NH, OH in the vessel 0.240 seconds later. You may assum other reaction is important. Round your answer to 2 significant digits. M x10
For a reaction A products, sicessive half_For a reaction A→ products, successive half-lives are observed to be 10.0,20.0 and 40.0 min for an experiment in which the initial concentration of A=0.10M. Calculate the concentration of A(M) after 39.37 minutes. Report your answer to 4 significant fgures.
Don't provide handwitten solution please...
For the reaction: BrO3-(aq) + 5Br (aq) + 8H*(aq) → 3Br2(/) + H201) The initial rate of the reaction has been measured at the reactant concentration show: Trial [BrO;] (mol/L) 1 [H'] [Br ] Initial rat (mol/L) (mol/L) (mol/L-s) 0.10 0.10 0.10 8.0 0.20 0.10 0.10 16 0.10 0.20 0.10 16 4 0.10 0.10 0.20 32 The value for k will be: A L/mol.s Ouestion 13 (1 23
An experiment was carried out to investigate the effect of concentration on the reaction: BrO3(aq) + 5 Br (aq) + 6 H* (aq) = 3 Br₂ (1) + 3 H₂O (1) The following data was obtained: Initial [BrO3] Initial [Br] Initial [H*] Initial Rate Trial (mol/L) (mol/L) (mol/L) (mol/L's) 1 0.10 0.10 0.10 8.0 x 10-4 2 0.20 0.10 0.10 1.6 x 10-3 3 0.20 0.20 0.10 3.2 x 10-3 4 0.10 0.10 0.20 3.2 x 10-3 a) Deduce and state the rate law equation for this reaction. Show your process/reasoning. b) Calculate the value of k, the rate constant with correct units.