+ pH and KineticsThe iodate ion, IO3 is reduced by sulfite. SO², according to thefollowing net ionic equation:IO, (aq) + 350,² (aq) + (aq) + 350,² (aq)Part Afound to be first order in IO3, first order in SO3²and first order in H+.If [103] z. [SO₂²]y, and [H¹] = Z, what is the rate law for the reaction terms of z, y, and 2 and the rate constant k?Express the rate in terms of k, z▸ View Available Hint(s)and 2 (e.g., kxy^3z^2).|VL | ΑΣΦThe reactionrate =Submit16 of 43 >Review | Constants | Periodic Table

First we need to write the rate law of given reaction as per orders . Then we would plug the values…

The reaction is found to be first order in 10s first order in SO3² and first order in H¹. If [10₂]=z. [S0₂² 1 y. and H=2, what is the rate law for the reaction in terms of z. y. and 2 and the rate constant k? Express the rate in terms of k, z, y, and z (e.g., kxy^3z^2). View Available Hintis)

The reaction is found to be first order in 10s first order in SO3² and first order in H¹. If [10₂]=z. [S0₂² 1 y. and H=2, what is the rate law for the reaction in terms of z. y. and 2 and the rate constant k? Express the rate in terms of k, z, y, and z (e.g., kxy^3z^2). View Available Hintis)

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter11: Rate Of Reaction

Section: Chapter Questions

Problem 99QAP: The gas-phase reaction between hydrogen and iodine H2(g)+I22HI(g)proceeds with a rate constant for...

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The gas-phase reaction between hydrogen and iodine H2(g)+I22HI(g)proceeds with a rate constant for the forward reaction at 700C of 138 L/moI s and an activation energy of 165 kJ/moI. (a) Calculate the activation energy of the reverse reaction given that H f for HI is 26.48 kJ/moI and H f for I2(g) is 62.44 kJ/mol. (b) Calculate the rate constant for the reverse reaction at 700C. (Assume A in the equation k=AeE a /RT is the same for both forward and reverse reactions.) (c) Calculate the rate of the reverse reaction if the concentration of HI is 0.200 M. The reverse reaction is second-order in HI.
The iodate ion is reduced by sulfite according to the followingreaction:IO3-(aq) + 3 SO32-(aq) -----> I-(aq) + 3 SO42-(aq)The rate of this reaction is found to be first order in IO3-,first order in SO32-, and first order in H+.(a) Write the rate law for the reaction.(b) By what factor will the rate of the reaction change ifthe pH is lowered from 5.00 to 3.50? Does the reactionproceed more quickly or more slowly at the lower pH?(c) Explain how the reaction can be pH-dependent even thoughH+ does not appear in the overall reaction.
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
Upon dissolving InCl(s) in HCl, In+(aq) undergoes a disproportionation reaction according to the following unbalanced equation: In+(aq) = In(s) + In3+(aq) This disproportionation follows first-order kinetics with a half-life of 667 s. What is the concentration of In+(aq) after 1.35 h if the initial solution of In+(aq) was prepared by dissolving 2.38g InCl(s) in dilute HCl to make 5.0x10^2 mL of solution? What mass of In(s) is formed after 1.35 h?
Upon dissolving InCl(s) in HCl, In+(aq) undergoes a disproportionation reaction according to thefollowing balanced equation:3In+ (aq) → 2In(s) + In3+(aq)This disproportionation follows first-order kinetics with a half-life of 667 s.(a) What is the concentration of In+(aq) after 1.22 h if the initial solution of In+(aq) was prepared bydissolving 2.38 g InCl(s) in dilute HCl to make 5.00 x 102 mL of solution? (b) What mass of In(s) is formed after 1.22 h?
A reaction of the form aA Products gives a plot of 1/[A] vs time (in seconds) which is a straight line with a slope of 4.15 x 103. Assuming [A]o 0.100 M, calculate the time (in seconds) required for the reaction to reach 76.9 percent completion. %3D seconds
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
A suggested mechanism for the gas phase decomposition of nitrous oxide is: step 1: NgÐ — Nz + 0 N₂O + O N₂ + O2 step 2: (a) Identify the molecularity of each step in the mechanism. step 1 8 step 2 (b) Write the equation for the net reaction. Use the smallest integer coefficients possible. If a box is not needed, leave it blank. 8 (c) Identify any intemediates and/or catalysts in this mechanism. Catalyst: Enter formula. If none, leave box blank: Intermediate: Enter formula. If none, leave box blank: The following mechanism has been proposed for the gas phase reaction of nitrogen monoxide with bromine. step 1: NO + Br₂ → NOBr₂ NOBr₂ + NO 2 NOBr step 2: (a) Identify the molecularity of each step in the mechanism. step 1 step 2 (b) Write the equation for the net reaction. Use the smallest integer coefficients possible. If a box is not needed, leave it blank. (c) Identify any intermediates and/or catalysts in this mechanism. Catalyst: Enter formula. If none, leave box blank: Intermediate:…
Thiosulfate ions are oxidized by iodine according to the reaction below:2 S2O 33- (aq) + I2 (aq) → S 4O 62- (aq) + 2I -(aq)If 0.0080 mol of S2 O32- is consumed in 1.0 L of solution every second, what isconsumption rate of iodine?
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.
The gas phase reaction between hydrogen and iodine is proposed to occur as follows:.....step 1.....fast:......I2 2 I.....step 2.....slow:....H2 + 2 I 2 HI(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) Enter the formula of any species that acts as a reaction intermediate? If none leave box blank: (3) Complete the rate law for the overall reaction that is consistent with this mechanism.Use the form k[A]m[B]n... , where '1' is understood (so don't write it if it's a '1') for m, n etc. Rate =
[Review Topics] [References] Use the References to access important values if needed for this questi A reaction profile (not to scale!) for the reaction 2 0,→03+O is shown below: E (kJ) O3 + 0 411 392 O2 + O2 Reaction Coordinate This reaction is (exothermic,endothermic) The value of the activation energy for this reaction is kJ and the value of AE is kJ. Submit Answer Retry Entire Group 9 more group attempts remaining Cengage Learning | Cengage Technical Support 98°F Rail