(6 pts.) Consider a kinetics study of the following ligand substitution reaction:trans-[Rh(en)2C12]* + 2 Y¯ ⇒ trans-[Rh(en)2Y2]* + 2 CI¯¯When Y=I, Br, and NO2, the reaction rate constants are 5.2 x 10-5, 4.0 x 10-5, and 4.2 x10-5 M¹ s¹, respectively. By which mechanism does this reaction most likely proceed?Justify your answer.

Step 1: Understand the ReactionThe reaction is:trans-[Rh(en)2Cl2]+ + 2 Y- → trans-[Rh(en)2Y2]+ + 2…

Answered: (6 pts.) Consider a kinetics study of…

Chemistry

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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...

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Consider a kinetics study of the following ligand substitution reaction: trans-[Rh(en)2Cl2] + + 2 Y−  trans-[Rh(en)2Y2] + + 2 Cl− When Y− = I−, Br−, and NO2 −, the reaction rate constants are 5.2 x 10-5 , 4.0 x 10-5 , and 4.2 x 10-5 M-1 s-1 , respectively. By which mechanism does this reaction most likely proceed? Justify your answer.
What is the mechanism by which the following reaction occurs ?: [Ru(NH3)6]2+ + [Fe(H2O)6]3+ → [Ru(NH3)6]3+ + [Fe(H2O)]2+ Select one: a. Dissociative mechanismb. Inner sphere mechanismc. External sphere mechanismd. Associative mechanism
In spite of the high equilibrium constant (K = 1025) for the reaction given here, the reaction proceeds very slowly, reaching equilibrium only after several days at room temperature. [Co(NH3)6]3+ + 6 H3O* = [Co(H20)6]3+ + 6 NH,* The observation is consistent with: the activation energy for the forward reaction being low. [Co(NH3)6]3+ being unstable in strong acid. [Co(NH3)6]3+ being more labile than [Co(H2O)6]3+. the classification of [Co(NH3)6]3+ as an inert complex.
Derive general rate law, organometallic (That's all the info, nothing else) Consider an 18-electron complex (diene) Cr(CO)4. Reaction with a ligand L (such as a phosphine, for example) generally results in complete displacement of the diene ligand to give Cr(CO)4L2; the plausible intermediate where a single L has been added and only one of the diene double bonds remains coordinated reacts much too rapidly with additional L to be isolated (or even observed). Formation of that intermediate could in principle proceed via either a dissociative mechanism or an interchange mechanism. Assuming that both mechanisms operate, use the steady-state approximation to derive the general rate law for the reaction, and sketch what a plot of rate vs. [L] would look like. Then show how the rate law would simplify if only one of the two alternative mechanisms were significant and sketch the corresponding rate vs. [L] plots for each of those cases. OC OC CO DCr(CO)4 OC PEt3 PEt3 OC PEt3 Cr(CO)4L2 CO CO OC.…
For the reaction k1 k2 [Cr(H2O)4Cl2]+(aq) ====è [Cr(H2O)5Cl]2+ =====è [Cr(H2O)6]3+(aq) k1 = 1.78 x10-3/s and k2 = 5.8 x10-5/s for [Cr(H2O)Cl2]+ = 0.0174 mol/L at 0oC a.) Calculate the concentration of species at t =500sec. b.) Calculate the value of t at which the value of [Cr(H2O)5Cl]2+ is a maximum. c.) What is the maximum value of [Cr(H2O)Cl]2+
In 17.5% w/w HCl, the complex ion Ru(NH3)63+ decomposes to a variety of products. The reaction is first order in [Ru(NH3)63+] and has a half-life of 14 h at 25°C. (a)What is the rate constant for this reaction? (b)Under these conditions, how long will it take for the [Ru(NH3)63+] to decrease to 6.25% of its initial value? What is the rate constant in s-1 for a first order reaction with an initial concentration of a 0.600 mol/L if, after 142 s, the concentration is 0.444 mol/L? What is the half-life in seconds for a second order reaction with the rate constant k = 2.74 x 10-1 L/mole∙s if the initial reactant concentration is 0.500 mol/L?
Consider the following reaction: [Cr(H2O)5(SCN)]2+ + Yn- --> [Cr(H2O)5Y](3-n)+ + SCN- Which statement is true if this reaction occurs via a dissociation mechanism? Group of answer choices Changing the incoming ligand, Yn-, will have a large effect on the rate constant. The first step of the mechanism is the addition of the Yn- ligand to form a 7-ccordinate intermediate, [Cr(H2O)5(SCN)Y](2-n)+ Changing the incoming ligand, Yn-, will have very little effect on the rate constant. It is impossible for this reaction to occur via a dissociation mechanism.
1. In aqueous solution, [Co(CN),C1]³ hydrolyses according to: [Co(CN), Cl]³¯ + H₂O → [Co(CN) (H₂O)]²¯ + CI˜¯ The reaction is subject to catalysis by H†, so that: = Rate k₁ {[Co(CN), Cl]³¯}* +k₂[H*]{[Co(CN), CI]³¯}*, in which kɩ and k₂ are rate constants for the uncatalysed and catalyzed pathways, respectively. At pH = 3.00, the two pathways contribute equally to the overall rate, and the data below obtain: 20 30 180 0.057 0.080 300 0.080 Time (min) 0 10 [Co(CN),(H2O)]² (mol/L) 0 0.027 0.045 a. Find the initial concentration of [Co(CN)5C1]³¯, and show that the data are consistent with x = = 1. b. Evaluate k₁ and k₂. c. What is the half-life of [Co(CN)5C1]³¯ at pH = 7.00?
5.62 Predict the products of the following reactions: (a) [Pt(CO)Cl3]+ py→ РУ (6) Cl Cl Pt + NH3 -> H3N NO2 (c) [P+C!3SCN]2-+ H2O - (d) [PtCl3 CN]2-+ NH3 –
8) Bipyridine ligands are known to be redox active. Draw the product of the hypothetical reduction of the following molecule where you assume the bpy is getting reduced and not the metal. Draw a static resonance structure showing the positions of any multiple bonds. What might you look for in the solid- state crystal structure (or even a calculated structure) to determine if a bpy is exhibiting redox-active behavior 120 2e0
1
Q 2. Comment on the Kinetic and thermodynamic stability of metal complexes? (2 marks) (a) Which complex is kinetically labile or inert according to crystal field theory? H₂O OH2 OH2 * H₂O NECHI Mn OH2 OH2 4- 2+ [+] NEC CEN CEN (b) Which complex is most thermodynamically stable and why? Calculate log ẞ to determine stability? H3N 2+ _NH3] 2 [NC-Ag-CN]] NH3 3+ H3N... H3N ,,NH3 Cr NH3 H3N NH3 NH3 K 1.0 x10¹² K 5.4 x 1018 K=2.0 × 105

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