Show your work and be sure to give answer with the correct units.The following rate data was obtained for the reaction:2 CIO2 + 2 OH¯ → CIOз¯ + CIO2 + H2OExperiment #[CIO2][OH-]rate10.0600.0302.48 x 10-220.0200.0302.76 x 10-330.0200.0908.28 x 10-3Determine the reaction order with respect to (1) CIO2 and (2) OH¯, (3) write the rate law andthen (4) determine the value of the rate constant, k.

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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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-1 -1 At a certain temperature the rate of this reaction is second order in HI with a rate constant of 1.0M S 2HI (g) → H₂(g) + 1₂ (g) Suppose a vessel contains HI at a concentration of 1.33M. Calculate the concentration of HI in the vessel 7.50 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. M x10 X Ś ?
Consider the reaction A + 2B = C whose rate at 25 °C was measured using three different sets of initial concentrations as listed in the following table: [A] [B] Rate (M) (M) (M/s) 0.20 0.050 2.4x10-3 0.20 0.100 4.8x10-3 3 0.40 0.050 9.6x10-3 Trial 1 2 What is the rate law for this reaction? Express the rate law symbolically in terms of k, [A], and [B]. ► View Available Hint(s) rate = Submit VE ΑΣΦ ?
The data below were collected for the following reaction: CH3CI(g) + 3 Cl2(g) CCI4(g) + 3 HCI(g) Trial [CH3CI] / mol L-1 [Cl2] / mol L-1 Initial Rate / mol L-1 s-1 1 0.050 0.050 0.0142 2 0.100 0.050 0.0290 3 0.200 0.200 0.115 What is the rate constant?
Pre-lab question #10-3: A reaction between substances A and B has been found to give the following data: 3 A + 2 B → 2 C + D Rate of Appearance of C, M/hr [A], M [В], М 1.0 x 10-2 1.0 0.300 x 10-6 1.0 x 10-2 3.0 8.10 x 10-6 2.0 x 10-2 3.0 3.24 x 10-5 2.0 x 10-2 1.0 1.20 x 10-6 3.0 x 10-2 3.0 7.30 x 10-5 Using the data above, determine the following: Pre-lab question #10-3: c) Calculate the value of the rate constant, k. 0.00300 O 0.0120 0.00900 0.00600
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Given the following results: Run Rate of Reaction (M/s) [I-] [H2O2] 1 1.99 0.516 0.561 2 3.15 0.516 0.643 3 5.22 0.817 0.561 Calculate the rate constant(k) for each run. Assuming the Rate Law = k[I-]2[H2O2] calculate the average rate constant,k, for this reaction. Give your answer to 2 places after the decimal.
16. The reaction between A and B is as follows: * A + 2B → 2C The rate of reaction with variation of concentration of A and B at the same temperature is shown in Table 2. Table 2 Rate of reaction /mol dm³s' 1.20 × 10² 9.00 × 103 1.35 × 102 Experiment [A]/mol dm³³ | [B]/mol dm³³ I 1.00 2.00 II 1.00 1.50 III 1.50 1.00 IV 2.00 0.50 What is the value of x ? A. 3.00 × 103 В. 6.00 х 103 C. 1.20 × 10² D. 2.40 × 102
Use the following data to determine the rate law and rate constant for the reaction: NH4+ NO₂¹ → N₂ + 2H₂O. Trial 1 2 3 4 [NH4*] (M) [NO₂] (M) 0.0184 0.098 0.0184 0.047 0.0249 0.196 0.0114 0.196 p Rate M S 6.98 x 10-6 3.32 x 10-6 1.68 x 10-5 7.80 x 10-6 amse och sill binowe erw sill to buissopust
For this reaction occurring at 20 °C, the following data was obtained. C6H12O + Br2 → C6H11OBr + HBr What is the rate law of the reaction? Run C6H12O (M) Br2 (M) Initial Rate, M/min 1 0.20 0.15 2.55 x 10-4 2 0.40 0.15 2.52 x 10-4 3 0.40 0.30 5.09 x 10-4
The rate constant of a certain reaction is known to obey the Arrhenius equation, and to have an activation energy E=52.0 kJ/mol. If the rate constant of this -1 -1 reaction is 1.7 × 10+ M's at 197.0 °C, what will the rate constant be at 168.0 °C? Round your answer to 2 significant digits. k = □M -1 5 ? 0 xno 圖□ □ □

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