Please please sir solve accurate please For the reaction of the dimerization of 1,3-butadiene, a graph of 1/[H2C=CHCH=CH2] versus timegives a straight line with a slope of 0.0611 Mªs².H,C-CH2HC1/½CHH,C=CHCH=CH,HCCH1,3-butadieneHC– CH,1,5-cyclooctadieneа.Based on the graphical analysis, what is the order for 1,3-butadiene.b. Write the rate law for this reaction.С.What is the rate constant for this reaction?d. How many seconds would it take for the concentration of butadiene to go from 0.0240 M to0.0170 M?

Answered: Image /qna-images/answer/e4986e3c-ffc6-4ab4-879b-04d6b986185c.jpg

For the reaction of the dimerization of 1,3-butadiene, a graph of 1/[H2C=CHCH=CH2] versus time gives a straight line with a slope of 0.0611 M's1. H,C- CH2 H.C HC CH H,C=CHCH=CH, 1,3-butadiene HC CH H.C– CH2 1,5-cyclooctadiene a. Based on the graphical analysis, what is the order for 1,3-butadiene. b. Write the rate law for this reaction. С. What is the rate constant for this reaction? d. How many seconds would it take for the concentration of butadiene to go from 0.0240 M to 0.0170 M?

For the reaction of the dimerization of 1,3-butadiene, a graph of 1/[H2C=CHCH=CH2] versus time gives a straight line with a slope of 0.0611 M's1. H,C- CH2 H.C HC CH H,C=CHCH=CH, 1,3-butadiene HC CH H.C– CH2 1,5-cyclooctadiene a. Based on the graphical analysis, what is the order for 1,3-butadiene. b. Write the rate law for this reaction. С. What is the rate constant for this reaction? d. How many seconds would it take for the concentration of butadiene to go from 0.0240 M to 0.0170 M?

Physical Chemistry

2nd Edition

ISBN:9781133958437

Author:Ball, David W. (david Warren), BAER, Tomas

Publisher:Ball, David W. (david Warren), BAER, Tomas

Chapter20: Kinetics

Section: Chapter Questions

Problem 20.38E: List at least four experimentally determined parameters that you, an experimenter, can define when...

See similar textbooks

Similar questions

Derive the integrated form of a third-order rate law v = kr[A]2[B] in which the stoichiometry is 2 A +B −−→ P and the reactants are initially present in (a) their stoichiometric proportions, (b) with Bpresent initially in twice the amount.
Sucrose (C12H22O11)(C12H22O11), which is commonly known as table sugar, reacts in dilute acid solutions to form two simpler sugars, glucose and fructose, both of which have the formula C6H12O6C6H12O6. At 23 ∘C∘C and in 0.5 M HClM HCl, the following data were obtained for the disappearance of sucrose: Time (min)(min) C12H22O11(M)C12H22O11(M) 0 0.316 39 0.274 80 0.238 140 0.190 210 0.146 What is the rate constant?
True or False: 1. The initial concentration of an intermediate is assumed as 0 when using steady-state approximation. 2. A spontaneous reaction with ΔG = -1070 J/mol happens at 562 K, the Keq of this process is less than 1.
Write down the kinetic equation for a simple reaction in a homogeneous medium 2A + B = 2C. Indicate the general and in relati on to all reactants reaction orders
Derive the integrated form of a third-order rate law v = kr[A]2[B] in which the stoichiometry is 2 A + B → P and the reactants are initially present in (a) their stoichiometric proportions ([B]0 = 12[A]0); (b) with B present initially in twice that amount ([B]0 = [A]0). Express your rate law in terms of [A]0, [B]0, and x, where [A] = [A]0 − 2x.
The decomposition of aqueous sucrose to form the isomers glucose and fructose is a common organic reaction, which requires a strong catalyst: C12H22O11(aq) + H2O(l) → 2C6H12O6(aq). The following data were collected during the process: Time (min) [C12H22O11] (mol/L) 0 0.316 39 0.274 80 0.238 140 0.190 210 0.146 (A) If we performed a new trial with an initial concentration of sucrose of 0.400 mol/L, what concentration would remain after 4.0 h has passed?
Calculate the magnitude of the diffusion-controlled rate constant at 320 K for the recombination of two atoms in benzene, for which η = 0.601 cP. Assuming the concentration of the reacting species is 2.0 mmol dm−3 initially, how long does it take for the concentration of the atoms to fall to half that value? Assume the reaction is elementary.
Calculate the ratio of rates of catalyzed to non-catalyzed reactions at 37°C, given that the Gibbs energy of activation for a particular reaction is reduced from 100 kJ/mol to 10 kJ/mol. Ans: 1.5 x 1015
Consider the reaction N₂O(g) →N₂(g)1/2O₂(g) with Au has catalyst (a) Is the gold a homogeneous or a heterogeneous catalyst?(b) On the same set of axes, sketch the reaction energy dia-grams for the catalyzed and the uncatalyzed reaction
Assuming the rate law for the system is rate = k[I-]x[S2O82-]y, what is the value of x for the system? Explain your answer. What are the steps in obtaining this answer?
The rate law for a reaction was reported as v= k,[A][B][C] with the molar concentrations in moles per cubic decimetre and the time in seconds. What are the units of k,?
Q1.Differentiate between homogenous and heterogeneous catalysis with suitable examples Q2. What are the basic rules use for the nomenclature of co-ordination compounds?