The reaction of peroxydisulfate ion (S,0g) with iodide ion (I) is S,0, (aq) + 31 (aq)→ 2So, (aq) +I (aq) From the following data collected at a certain temperature, determine the rate law and calculate the rate constant. Experiment [S,0,²](M) Initial Rate [M/s] 0.0300 0.1000 5.60 x 104 2. 0.0300 0.0500 2.80 x 104 3 0.0600 0.0500 5.60 x 104 (a) Which of the following equations represents the rate law for this reaction? A. rate = k[S,OgO B. rate = k[S,O,O C. rate = k[S,OgD D. rate = k[S,Og²T²1? %3D A O BO CO D (b) What is the rate constant for the reaction? k = M's

The reaction of peroxydisulfate ion (S,0g) with iodide ion (I) is S,0, (aq) + 31 (aq)→ 2So, (aq) +I (aq) From the following data collected at a certain temperature, determine the rate law and calculate the rate constant. Experiment [S,0,²](M) Initial Rate [M/s] 0.0300 0.1000 5.60 x 104 2. 0.0300 0.0500 2.80 x 104 3 0.0600 0.0500 5.60 x 104 (a) Which of the following equations represents the rate law for this reaction? A. rate = k[S,OgO B. rate = k[S,O,O C. rate = k[S,OgD D. rate = k[S,Og²T²1? %3D A O BO CO D (b) What is the rate constant for the reaction? k = 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 concentration of SO42– ions in a 70.0 mL sample of seawater is determined by adding a solution of BaCl2 and precipitating the SO42– as BaSO4. After the precipitate is filtered from the solution, it is dried and weighed. If the mass of BaSO4 recovered is 0.539 g, what is the sulfate concentration of the seawater sample? Express your answer in mmol/L. Please answer fast i give you upvote.
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reacting aqueous Pb(NO3)2 with Aqueous KI
Watch the following video, and identify the reaction type. Note: At the end of the video, they test of hydrogen gas, a flammable gas, which makes a popping sound when exposed to flame. There are two products formed. https://www.youtube.com/watch?v=A4XITC225uk&feature=emb_title (1 min 8 sec video)
Using the average molarity of the NaOH solution determined from your results in part A, calculate the molarity and percent by mass of the acetic acid in your vinegar sample and report their average values. H2C2O4•2H2O(s) + 2NaOH (aq)= Na2C2O4 + 4H2O(l) part A Mass of oxalic acid analyzed (g)- trial 1- 0.302 trial 2- 0.305 initial buret reading of NaOH (mL)- trial 1-0.31 trial 2- 23.42 final buret reading of NaOH (mL) trial 1- 23.42 trial 2 -46.73 Part B volume of vinegar analyzed (mL), trial 1- 5.00 , trial 2- 5.00 initial buret reading of NaOH (mL), trial 1 -0.00, trial 2 - 22.73 final buret reading of NaOH (mL) trial 1- 22.73, trial 2- 45.50 There is no molarity of oxalic acid that was used during the experiment given
Background-info: https://drive.google.com/file/d/1G7sPTuESIgWk9wpRdqAnFcsBmOlbBfLv/view?usp=sharing Question: In carrying out Part 1 of this experiment, assume an exces of HCI(aq) reacts with 0.296 g of Mgls). If the volume of the final solution is 69.0 mL, what is the stoichiometric concentration (in mol/L) of MgCl2laq) after the reaction is complete? Report your answer to the correct number of significant figures and only include the numerical answer (no units).
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Quantity Your Data 1. Grams of vinegar sample used for your titration 25.000 g 2. Initial Buret Reading of Sodium Hydroxide solution 10.00 mL 3. Final Buret Reading of Sodium Hydroxide solution 28.00 mL 4. Amount of Sodium Hydroxide Solution used to neutralize the vinegar sample 5. Concentration of NaOH in the NaOH solution 0.050 g/mL 6. Grams of NaOH used to neutralize the vinegar 7. Grams of acetic neutralized by the amount of NaOH 8. Percent acetic acid in the vinegar Hints: For #4, The amount of NaOH used is the difference between the starting buret value and the ending buret value. For #6, Once you calculate the amount of sodium hydroxide used, multiple that value by the concentration of NaOH in the NaOH solution. For #7, Multiply the value obtained in number 6 by the number 1.5. Remember, we learned that every 1 gram of NaOH neutralizes 1.5 grams of acetic acid. For #8, Divide the grams of acetic acid by the grams of vinegar sample and multiply this value by…
K2Cr2O7 + 7H2C2O4·2H2O → 2K(Cr(C2O4)2(H2O)2) + 6CO2 + 17H2O Calculate theoretical yield of: K[Cr(C204)2(H20)2] · 2H2O (3 g of oxalic acid dihydrate (H2C2O4·2H2O) )(1 g of potassium dichromate (K2Cr2O7) )(20 mL of 95% ethanol)