Use the Rele.to access impevalues if needed for this questionThe following initial rate data are for the reaction of UO,* with hydrogen ion in aqueous solution:2 UO,* + 4 Ht+ U0,* -+ 2 H2O[UO,],, M1.39x10-32.78×103Experiment[H*]o, MInitial Rate, M s-111.35×1040.4500.4505.39x1042.2.70x1041.08×10-331.39x10-30.900142.78x10-30.900Complete the rate law for this reaction in the box below.Use the form k[A]™[B]" , 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 isM?s!. The reaction of hypochlorite ion with iodide ion in 1 M aqueous hydroxide solutionOCr +I OI + CIis first order in OCI and first order in I.Complete the rate law for this reaction in the box below.Use the form k[A]™[B]"... , where 'l' is understood for m, n ...(don't enter 1) and concentrations taken to the zero power do not appear.Rate =In an experiment to determine the rate law, the rate constant was determined to be 86.4 M's. Using this value for the rate constant, the rate of the reaction when[OCr] = 2.36x10-3 M and [I] = 3.83×10-3 M would be|Msl.

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Answered: The following initial rate data are for…

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter11: Chemical Kinetics: Rates Of Reactions

Section: Chapter Questions

Problem 113QRT

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The following experimental data were obtained for the reaction of \'I14* and NOf in acidic solution. NH/(aq) + NO2-(aq) — N;(g) + 2 H,O(f) INH/I (mol L1) [NO21 (mol L-1, Rate = A[NJ/At (mol L-1 s’) 0.0092 0.098 3.33 X IO"7 0.0092 0.049 1.66 X 10‘7 0.0488 0.196 3.51 X 10"6 0.0249 0.196 1.80 X 10-6 Determine the rate law for this reaction and calculate the rate constant.
The reaction of hypochlorite ion with iodide ion in 1 M aqueous hydroxide solutionOCl- + I- -----> OI- + Cl-is first order in OCl- and second order overall.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, n ... (don't enter 1) and concentrations taken to the zero power do not appear.Rate = __________
Consider the reaction Mn+ + ne- ⇌ M. If ΔG*c = ΔG* + (1-α)nFE and η = E – Eeq, prove that ic = io exp[-(1-α)nFηa)/RT)].
The progress of the reaction between Iodine ions and potassium iodate(V) can be followed by withstanding samples of the reaction mixture at various times, quenching and then titrating with standard thiosulphate solution. The reaction equation is: I(aq) + IO3(aq) + 6H+(aq) + 4e ➡ I2(aq) + 3H2O(l) In one such experiment the following data were obtained. (see figure below) Determine the order of the reaction with respect to I(aq) and IO3(aq) ions Write the rate expression for the reaction.
Derive integrated rate law expressions for half-, one and a half-, and third-order reactions of the form A ® products where k is the rate constant. Also, deduce the graphical linear relations, units of rate constant k, and expression for half-life, t1/2 , for all cases. Assume that at t = 0 only A is present with an initial concentration of [A]0. Fill in the table below by following the example given for first-order reaction1. Show all your work. order Integrated Rate Law Graphical Linear Relation Unit of k Half-life 1 ln[A][A]0=−?? ln[A] vs t ⇒ slope = −k , y-intercept = ln[A]0 1? ?12⁄=ln2? 1/2 3/2 3 1Atkins’ Physical Chemistry, Atkins and de Paula, 10th Ed., 2014, OUP, pp. 827-828.
The following results were found after following the procedure Part B in the experiment: 0.053 M I- and 0.041 M H2O2 were used Temperature (oC) Calculated Reaction Rate (M/s) 12 0.031 30 0.119 88 0.797 Assuming the Rate Law = k[I-]2[H2O2] 2 Calculate the value of k at temperature 88oC. Give your answer to 1 place after the decimal.
The reaction of hypochlorite ion with iodide ion in 1 M aqueous hydroxide solutionOCl- + I-OI- + Cl-is first order in OCl- and first order in I-.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, n ... (don't enter 1) and concentrations taken to the zero power do not appear. Rate = In an experiment to determine the rate law, the rate of the reaction was determined to be 1.39×10-3 Ms-1 when [OCl-] = 5.51×10-3 M and [I-] = 2.65×10-3 M. From this experiment, the rate constant is ___________ M-1s-1.
The reaction of hypochlorite ion with iodide ion in 1 M aqueous hydroxide solutionOCl- + I-OI- + Cl-is first order in OCl- and first order in I-.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, n ... (don't enter 1) and concentrations taken to the zero power do not appear. Rate = In an experiment to determine the rate law, the rate constant was determined to be 90.6 M-1s-1. Using this value for the rate constant, the rate of the reaction when [OCl-] = 5.13×10-3 M and [I-] = 7.53×10-3 M would be
The reaction of hypochlorite ion with iodide ion in 1 M aqueous hydroxide solution OCI I OI+ CIT is first order in OCI and first order in I Complete the rate law for this reaction in the box below. Use the form k[A]" [B]", where '1' is understood for m, n ... (don't enter 1) and concentrations taken to the zero power do not appear. Rate = for this question. In an experiment to determine the rate law, the rate of the reaction was determined to be 1.29 x 10 [OCI] = 0.00169 M and [IT] = 0.00843 M. From this experiment, the rate constant is
Part B: Integrated rate law expressions for zero- and half-order reactionsDerive integrated rate law expressions for half-, one and a half-, and third-order reactions of the form A  products where k is the rate constant. Also, deduce the graphical linear relations, units of rate constant k, and expression for half-life, t1/2 , for all cases. Assume that at t = 0 only A is present with an initial concentration of [A]0. Fill in the table below by following the example given for first-order reaction1.
Using the data in the table, determine the rate constant of the reaction and select the appropriate units. A+2B⟶C+D Trial [?] (?) [?] (?) Rate (M/s) 1 0.340 0.210 0.0204 2 0.340 0.420 0.0204 3 0.680 0.210 0.0816 ?=
The below reaction is studied using the flooding method. A+B⟶C with rate constant k and rate=k[A]a[B]a The reaction is flooded in B, and the concentration of A as a function of time is measured. The reaction is discovered to be first order in A. At [B] = 0.081 M, kobs = 2.5 x 10-4, and when [B] is tripled, kobs = 2.25 x 10-3. What is value of k? Do not include units when entering your answer. Enter your answer with 3 decimal places.

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