7. How did the reaction below happen? Use catalytic circle to describe the mechanism, assuming the catalyst is the complex [CpRu(CH,CN),][BAr] 1a مهمه + MeO 2A OMe Catalyst CH₂Cl₂ (0.5 M) 60 °C, 6 h CO₂Me CO₂Me 3aA

7. How did the reaction below happen? Use catalytic circle to describe the mechanism, assuming the catalyst is the complex [CpRu(CH,CN),][BAr] 1a مهمه + MeO 2A OMe Catalyst CH₂Cl₂ (0.5 M) 60 °C, 6 h CO₂Me CO₂Me 3aA

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter18: Chemical Kinetics

Section: Chapter Questions

Problem 73AP

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Similar questions

For each of the following reaction diagrams, estimate the activation energy (Ea) of the reaction:
The oxidation of iodide ion by the hypochlorite ion in the presence of hydroxide ions I(aq) + ClO(aq) IO(aq) + Cl(aq) was studied at 25 C, and the following initial rates data (Y. Chia and R. E. Connick, Journal of Physical Chemistry, Vol. 63, p. 1518, 1959) were collected: (a) Determine the rate law for this reaction. (b) One mechanism that has been proposed for this reaction is the following: Show that the rate law predicted by this mechanism matches the experimentally determined rate law in part a. (Note that when writing the expression for K the equilibrium constant, [H2O] is not involved. See Chapter 15.)
What is the activation energy of a reaction, and how is this energy related to the activated complex of the reaction?
Write the mechanism for this
Please help
he activation energy for the gas phase isomerization of cyclobutene is 136 kJ.(CH2)2(CH)2CH2=CHCH=CH2The rate constant at 428 K is 2.88×10-4 /s. The rate constant will be 3.08×10-3 /s at K.
Under certain conditions the reaction H2O2 + 3I + 2H*→ I3¯ + 2H2O occurs by the following series of steps: ki Step 1. H2O2+H* =H;O2" + with K (equilibrium constant) = k1/k-1 Step 2. H3O2* +I→ H2O + HOI (slow, rate constant k2) Step 3. HỘI + I→ OH¯ +I2 (fast, rate constant k3) Step 4. OH + H*→ H2O (fast, rate constant k4) Step 5. I2 + I→ 13 (fast, rate constant k5) Use approximations (RDS, eq, steady-state) if necessary The rate constant k for the reaction would be given by
8) In the reversible reaction [Co(H20)s]"(aq) + 4CI (aq) E>[Co(H20)2CI4]* (aq) + 4H20(1), the initial color of the reaction mixture was pink. When concentrated HCl (aq) was added to the reaction mixture, the color changed to purple. Which reactant is purple and why? a) [Co(H2O)s]*(aq) is purple because it is a cobalt compound b) [Co(H20)s]**(aq) is purple because adding CI (as HCI) shifted the reaction towards products c) HCl is purple because adding it turned the reaction purple d) [Co(H2O),Cl4]*(aq) is purple because adding Cl (as HCI) shifted the reaction towards products 9) In the reversible reaction Fe * (aq) + SCN (aq) E → FESCN2* (aq), the reactants are yellowish and the product is red. Why are iron (III) nitrate and potassium thiocyanate used to create this reaction mixture? a) iron and thiocyanate are spectator ions b) iron and thiocyanate are colorless c) nitrate and potassium are spectator ions d) nitrate and potassium are purple
What is the full mechanism
Cc.80.
The activation energy for the gas phase isomerization of cis-cyanostyrene is 193 kJ. cis-C,H5CH=CHCN- →trans-C,H5CH=CHCN The rate constant at 678 K is 5.20x10-4 /s. The rate constant will be 3.97x10-3 /s at К.
Cr.