The reaction of peroxydisulfate ion (S₂O) with iodide ion (I) is S₂O3(aq) + 31¯(aq) → 2SO3(aq) + 13(aq) rom the following data collected at a certain temperature, determine the (a) rate law, (b) overall order of the action and (c) calculate the rate constant (Show your complete solution and use the data from Experiment Experiment [S₂0²¯] (M) [T](M) Initial Rate (M/s) 1 0.080 0.034 2.2 × 10-4 2 0.080 0.017 1.1 x 10-4 3 0.16 0.017 2.2 x 10-4 nswers: b). overall order of the reaction: second-order ote: answer for letter a will be provided by the student. c.) 8.1 x 102 /M-s

The reaction of peroxydisulfate ion (S₂O) with iodide ion (I) is S₂O3(aq) + 31¯(aq) → 2SO3(aq) + 13(aq) rom the following data collected at a certain temperature, determine the (a) rate law, (b) overall order of the action and (c) calculate the rate constant (Show your complete solution and use the data from Experiment Experiment [S₂0²¯] (M) [T](M) Initial Rate (M/s) 1 0.080 0.034 2.2 × 10-4 2 0.080 0.017 1.1 x 10-4 3 0.16 0.017 2.2 x 10-4 nswers: b). overall order of the reaction: second-order ote: answer for letter a will be provided by the student. c.) 8.1 x 102 /M-s

Chemistry

10th Edition

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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The reaction of peroxydisulfate ion (S,03-) with iodide ion (I) is S,03 (ag) + 31 (aq) → 2s0,7 (aq) + I3 (aq) From the following data collected at a certain temperature, determine the rate law and calculate the rate constant. Experiment [S,0g](M) M) Initial Rate [M/s] 1 0.0500 0.0480 4.80 x 104 2 0.0500 0.0240 2.40 x 104 3 0.1000 0.0240 4.80 x 10-4 (a) Which of the following equations represents the rate law for this reaction? A. rate = k[S,Og]ŋ B. rate = k[S,Og O. C. rate = k[S,Og]n D. rate = k[S,Og?o² овос OD (b) What is the rate constant for the reaction? k= M's
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Determine the rate law
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The hydrolysis of the sugar sucrose to the sugars glucose and fructose can be described as follows. C12H22011 + H20 → C;H1206 + CgH1206 This reaction follows a first-order rate equation for the disappearance of sucrose: rate = k [C,,H,,0,1] (The products of the reaction, glucose, and fructose, have the same molecular formulas but differ in the arrangement of the atoms in their molecules, i.e. they are 22 isomers.) 1.8x10-11 Arrhenius equation at this temperature). (Enter unrounded values.) (a) In neutral solution, k at 26°C and 8.5x10-11 -1 at 37°C. Determine the activation energy (in kJ/mol), the frequency factor (in s), and the rate constant (in s) for this equation at 48°C (assuming the kinetics remain consistent with the activation energy 108 kJ/mol frequency factor rate constant X s-1 (b) When a solution of sucrose with an initial concentration of 0.130 M reaches equilibrium, the concentration of sucrose is 1.40x10 M. How long (in s) will it take the solution to reach equilibrium…
The rearrangement of ammonium cyanate to urea in aqueous solution at 50 NH,NCO(aq)–(NH,),CO(aq) is second order in NH,NC0 with a rate constant of 1.10×10 ² M1 min. If the initial concentration of NH,NCO is 0.904 M, the concentration of 4 NH,NCO will be M after 247 minutes have passed.
Chlorine monoxide accumulates in the stratosphere above Antarctica each winter and plays a key role in the formation of the ozone hole above the South Pole each spring. Eventually, CIO decomposes according to the equation: 2Cio(g) Cl,(g) + 0,(g) The second-order rate constant for the decomposition of ClO is 7.08×10° M-1s=1 at a particular temperature. Determine the half-life of CIO when its initial concentration is 1.11x10-8 M.
a)The activation energy of a certain reaction is 48.9 kJ/mol. At 27 ∘C , the rate constant is 0.0160s ^−1 . At what temperature in degrees Celsius would this reaction go twice as fast? Express your answer with the appropriate units. b)Given that the initial rate constant is 0.0160s ^−1at an initial temperature of 27 ∘C , what would the rate constant be at a temperature of 200. ∘C for the same reaction described in Part A? Express your answer with the appropriate units.
Nitrite ion reacts with ozone in aqueous solution, producing nitrate ion and oxygen: NO, (aq) +O3(g) → NO, (aq) +O,(g) The following data were collected for this reaction at 298 K. Calculate the average reaction rate between 0 and 100 us (microseconds) and between 200 and 300 µs. Time (us) [03] (M) 1.193x10-2 100 9.952x10-3 200 8.797x10-3 300 8.163x10-3
The differential rate laws for the balanced chemical reaction: aA(aq) + bB (aq) + CC (aq) → product is given by: raterxn = k [A]³[C]³ [B]³ What are the order in each chemical, as well as the overall order of the chemical kinetics? Place your answer in each box, respectively! Provide detailed solution (The order of kinetics in A) = (The order of kinetics in B) = (The order of kinetics in C) = (The overall order of kinetics) =
At a certain temperature the rate of this reaction is first order in C1₂O5 with a rate constant of 0.0699 s ! 2C1₂O5 (g) → 2Cl₂ (g) +50₂ (g) Suppose a vessel contains Cl₂05 at a concentration of 0.910M. Calculate the concentration of C1₂05 in the vessel 11.0 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. M x10 X Ś
In the presence of excess thiocyanate ion, SCN-, the following reaction is first order in iron(III) ion, Fe3+; the rate constant is (1.37x10^0)/s. Fe3+(aq) + SCN-(aq) → Fe(SCN)2+(aq). What is the half-life, in seconds, of the reaction? Express your answer to three significant figures.