(a)Consider the following reaction:[Cr(H2O)5CN]Cl2 + H20--> [Cr(H2O)6]3+ + 2 Cl + CN-(CrCN)The rate law at 25°C in water for this reaction is:-d[CrCN]/dt = ki [CrCN] + k2 [C•CN][OH-] + k3 [CrCN][H+]. Identify k1, k2 andk3 with specific steps in your mechanisms. what steps were taken to get to this answer? I do mot understand.Practice Balance the EquationH,O, + KI + H,SO,→ K,SO, +I, + H,O%3D+1 -1+1 -1 +1 +6-2+1 +6 -2+1 -2oxidationreduction2 I1→ I, + 2e-!H,O, + 2e-l +2 H* → 2 H,O2 I-l + H,O, + 2 H*→ I, + 2 H,Oox:red:tot1 H,O, + 2 KI + H,SO4 → K,SO, +1 I, + 2 H,0

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Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter19: Transitition Metals, Coordination Chemistry And Metallurgy

Section: Chapter Questions

Problem 19.69QE

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Rate information was obtained for the following reaction at 25°C and 33°C; Cr(H2O)6 3+ + SCN¯ ---> Cr(H2O)5NCS2+ + H2O(l) Initial Rate [Cr(H2O)6 3+] [SCN-] @ 25°C 2.0x10-11 1.0x10-4 0.10 2.0x10-10 1.0x10-3 0.10 9.0x10-10 2.0x10-3 0.15 2.4x10-9 3.0x10-3 0.20 @ 33°C 1.4x10-10 1.0x10-4 0.20 a) Write a rate law consistent with the experimental data. b) What is the value of the rate constant at 25°C? c) What is the value of the rate constant at 33°C? d) What is the activation energy for this reaction? e) Can a 4th order reaction occur?
Rate information was obtained for the following reaction at 25°C and 33°C; Cr(H2O)6 3+ + SCN¯ ---> Cr(H2O)5NCS2+ + H2O(l) Initial Rate [Cr(H2O)6 3+] [SCN-] @ 25°C 2.0x10-11 1.0x10-4 0.10 2.0x10-10 1.0x10-3 0.10 9.0x10-10 2.0x10-3 0.15 2.4x10-9 3.0x10-3 0.20 @ 33°C 1.4x10-10 1.0x10-4 0.20 Can a 4th order reaction occur?
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
7. How did the reaction below happen? Use catalytic circle to describe the mechanism, assuming the catalyst is the complex [CpRu(CH;CN);[BAr] Catalyst CO2ME + MeO OMe ċO,Me N2 CH2CI2 (0.5 M) 60 °C, 6 h 1a 2A 3aA
The data below was collected from three trials of the following reaction: 2ClO2 (aq) + 2OH- (aq) --> ClO3- (aq) + ClO2- (g) + H2O (l) [ClO2]o (M) [OH-]o (M) Initial Rate (M/s) 1 0.0500 0.100 5.75 x 10-2 2 0.100 0.100 2.30 x 10-1 3 0.100 0.0500 1.15 x 10-1 If the initial concentrations were as follows, [ClO2]o= 0.25 M and [OH- ]o = 0.095 M, what would the initial rate be?
1. Reaction S: Cr(CO)s+ PH3 Cr(CO)s(PH3) + CO Reaction T: Mo(CO)s + Cl- Mo(CO):CI + CO (i) Choose the reaction that likely to proceed via associative mechanism. (ii) Explain your answer by elaborating the factors that favor the mechanism.
In the Courdinaten Compound Pt(NHe)zClz], the OXication nmber A Pt s +2 CoCrclination nimber is
The data below was collected from three trials of the following reaction: 2ClO2 (aq) + 2OH- (aq) --> ClO3- (aq) + ClO2- (g) + H2O (l) [ClO2]o (M) [OH-]o (M) Initial Rate (M/s) 1 0.0500 0.100 5.75 x 10-2 2 0.100 0.100 2.30 x 10-1 3 0.100 0.0500 1.15 x 10-1 a) What is the generic rate law for this reaction? b) What is the order for each reactant? What is the order for the overall reaction? c) What is the complete rate law for this reaction? d) If the initial concentrations were as follows, [ClO2]o = 0.25 M and [OH- ]o = 0.095 M, what would the initial rate be?
takeAssigimen [References) Use the References to access important values if needed for this question. The following initial rate data are for the oxidation of arsenate ion by cerium(IV) ion in aqueous solution: As033 + 2 Ce4+ + H20 As043 + 2 Ce3+ + 2 H+ Experiment [As033 lo, M [Ce1*Jo, M Initial Rate, Ms 102 א 4.91 0.461 5.74x10 3 9.82x10-2 0.461 1.15x10 2 4.91x10-2 0.922 2.30x10 2 4 9.82x10-2 0.922 4.59x10 2 Complete the rate law for this reaction in the box below. Use the form k[A]m[B]n, where '1' is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or n. Rate = From these data, the rate constant is M-25-1 Submit Answer Try Another Version 3 item attempts remaining Cengage Learning Cengage Technical Sunnort
First three sub-parts are solved Rate information was obtained for the following reaction at 25°C and 33°C; Cr(H2O)6 3+ + SCN¯ ---> Cr(H2O)5NCS2+ + H2O(l) Initial Rate [Cr(H2O)6 3+] [SCN-] @ 25°C 2.0x10-11 1.0x10-4 0.10 2.0x10-10 1.0x10-3 0.10 9.0x10-10 2.0x10-3 0.15 2.4x10-9 3.0x10-3 0.20 @ 33°C 1.4x10-10 1.0x10-4 0.20 a) Write a rate law consistent with the experimental data. b) What is the value of the rate constant at 25°C? c) What is the value of the rate constant at 33°C? d) What is the activation energy for this reaction? e) Can a 4th order reaction occur?
(d) M=? [M(CO),]+ (e) M=? H3CM(CO)5
Under dissolving indium chloride (InCℓ) in hydrochloric acid (HCℓ), In+ (aq) undergoes disproportionation reaction according to the following unbalanced equation. In+ (aq) = In (s) + In3+ (aq) This disproportionation follows a first – order kinetics with a half-life of 667 s.(a) What is the concentration of In+(aq) after 1.25 hours if the initial solution of In+ (aq) was prepared by dissolving 2.38 g InCℓ (s) in 5.00 x 102 mL of dilute hydrochloric acid?(b) What mass of In (s) is formed after 1.25 hours? (c) Determine the rate constant k, for this reaction. (d) Sketch a graph of [In+] versus time (sec) over a period of 3 hours.

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