Solvent: 50:50 water:isopropyl alcohol (v/v)Temperature:Volume of pure t-BuCl sample: \, 06 ML(3 sig figs.)Initial volume, V, of t-BuCl solution: |0l m(3 sig figs.)Calculated initial concentration of t-BuCl, [t-BuCl],: ¶. SI mol (3 sig figs.)Molarity of NaOH: . I50 m(3 sig figs.)TIMEBURETREADINGTOTAL VOLUMEOF NAOH ADDEDV, NAOH (mL)EXPIREDCALCULATEDTIME OF DAYIn[t-BuCl],(SECONDS)[t-BuCl],t9.81 M 22ss M16.1mL420 sec 18.2ml19.3 mL0.0 mL6:43O sec21 me 9.613.25.36.665762.262.252.332222212202.202192186:506:567:029.509.3114021.9 mL22.6 mLB.124.225.1mL7:0714401740204023409946994626.59.209119064.977:127:17mL7:227:777:32mL9.010.2426.326.5 m6.598.876 218mL27:3710.4 v13246Experimental Data B. Calculation of the rate of reaction at selected times.Calculate the rate of the reaction at each time indicated in the table. Express the ratein units of M/sec. Show the calculation of the 1000 second values.chemicai ledctianTIME (IN SECONDS)[t-BuC],RATE,t-Qucl+H201000thuoH + HCI20003000K= 3.1 10 sec-!

Answered: Image /qna-images/answer/0ee89092-9399-4ff0-918a-372fa1f27790.jpg

B. Calculation of the rate of reaction at selected times. Calculate the rate of the reaction at each time indicated in the table. Express the rate in units of M/sec. Show the calculation of the 1000 second values. chemicai leaction TIME (IN SECONDS) [t-BuCl], RATE, t-Qucl + H20 1000 thuoH + HCI 2000 3000 K = 3.1 10 sec! -5 1-

B. Calculation of the rate of reaction at selected times. Calculate the rate of the reaction at each time indicated in the table. Express the rate in units of M/sec. Show the calculation of the 1000 second values. chemicai leaction TIME (IN SECONDS) [t-BuCl], RATE, t-Qucl + H20 1000 thuoH + HCI 2000 3000 K = 3.1 10 sec! -5 1-

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...

See similar textbooks

Similar questions

For the reaction mechanism below answer the questions. Fast equilibrium OH- + O2NNH2 --> O2NNH- + H2O Slow O2NNH- --> N2O + OH- c. What is the predicted rate law?
The rate of a certain reaction was studied at various T(K) k (s-1) temperatures. The table shows temperature (T) and rate 400 0.000108 constant (k) data collected during the experiments. Plot the 420 0.000626 data to answer the questions. 440 0.00310 What is the value of the activation energy, E, for 460 0.0134 this reaction? 480 0.0511 500 0.175 520 0.547 E, = kJ - mol- 1108.79 540 1.57 560 4.18 Incorrect 580 10.4 What is the value of the pre-exponential factor (sometimes called the frequency factor), A, for this reaction? A = 140 6.79 x10 Incorrect
Units of M s-1 please
The reaction 2 N205(g) → 4 NO2(g) + O2(g) was studied and the rate of change of the concentration of O2 was found to be 3.65 mol L 15-1. Calculate the reaction rate (in mol L1s1). Reaction rate = i mol L-1s-1. eTextbook and Media Save for Later Attempts: 0 of 3 used Submit Answer
A reaction has a rate constant of 0.248 min ^ -1 at 347 K and a rate constant of 0.805 min -1 at 751 K . Calculate the activation e kJ/mol. Calculate the rate constant for the reaction at 581 K.
O KINETICS AND EQUILIBRIUM Using a second-order integrated rate law to find concentration... -1-1 At a certain temperature the rate of this reaction is second order in Cl,0, with a rate constant of 103.Ms: 2Cl,0; (g) 2Cl, (g) +50, (g) → Suppose a vessel contains Cl,0, at a concentration of 0.130M. Calculate the concentration of Cl,0, in the vessel 0.550 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. OM x10 Check Explanation Terms of Use | Privacy Center Accessibility 2021 McGraw Hill LLC. All Rights Reserved. II
23 II. An experiment followed the decomposition. of nitregen dioxide to nitregen monoxide & oxygen gas. Given the following data, what order is the reaction for nitrogen dioxide? Given an initial concentration of nitrogen dioxide of 0.0400 M, what's the concentration of this reactant after a half hour? show all grapers & calcs to determine answers. (sec) Time |[NO₂] (M) 0.0 50.0 100.0 200.0 300.0 0.01000 0.00787 0.00649 0.00481 0.00380 M G 2 XX 6.5 Hoa X019 201 2(x) = 2 (1.86) (3 (9)
5.00 mL 4.50 M acetone + 10.0 mL 1.15 M HCl + 10.0 mL 0.00200 M I2 + 25.0 mL H2O A student found that it took 146 seconds for the color of the I to disappear. a. What was the rate of the reaction? Hint: First find the initial concentration of Iz in the reaction mixture, [I2]o. Then use the equation Rate At t M/s b. Write the rate equation. (Abbreviate acetone to ace, H* ion to H", and iodine to I2. Represent the order of reaction with respect to acetone as m, the order of reaction with respect to iodine as n, and the order of reaction with respect to H* as p). c. Select all the unknown variables in the equation in part (b). Rate O[Ace] (Previous Next