Consider this reaction: CICH₂CH₂Cl (g) → CH₂CHCI (g) + HC1 (g) At a certain temperature it obeys this rate law. rate - (2.00 s¹) [CICH₂CH₂CI] S Suppose a vessel contains CICH₂CH₂Cl at a concentration of 1.22M. Calculate how long it takes for the concentration of CICH₂CH₂Cl to decrease to 21.0% of its initial value. You may assume no other reaction is important. Round your answer to 2 significant digits. 11. X G

Consider this reaction: CICH₂CH₂Cl (g) → CH₂CHCI (g) + HC1 (g) At a certain temperature it obeys this rate law. rate - (2.00 s¹) [CICH₂CH₂CI] S Suppose a vessel contains CICH₂CH₂Cl at a concentration of 1.22M. Calculate how long it takes for the concentration of CICH₂CH₂Cl to decrease to 21.0% of its initial value. You may assume no other reaction is important. Round your answer to 2 significant digits. 11. X G

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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Consider this reaction: 2H₂PO4 (aq) → P₂O5 (aq) + 3H₂O (aq) At a certain temperature it obeys this rate law. rate = (0.069 M¹.¹) [H₂PO4] Suppose a vessel contains H₂PO4 at a concentration of 0.380 M. Calculate how long it takes for the concentration of H3PO4 to decrease to 5.0% of its initial value. You may assume no other reaction is important. Round your answer to 2 significant digits. ? Submit A Continue 2 X
Consider this reaction: NH,OH (аq) — NH, (ад)+ н,о (ад) At a certain temperature it obeys this rate law. rate = (0.619 s)[NH,OH] S Suppose a vessel contains NH,OH at a concentration of 0.340M. Calculate the concentration of NH,OH in the vessel 2.60 seconds later. You may assume no 4 other reaction is important. Round your answer to 2 significant digits. ) M x10
Consider the reaction: (CH3)3CBr + OH– → (CH3)3COH + Br– with the rate law: Rate = (0.034 hour–1)[(CH3)3CBr] Calculate the time (in hours) at which 33.3% of the initial (CH3)3CBr concentration remains.
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Consider this reaction: 2N₂O5 (g) → 2N₂O4 (8) + 0₂ (8) At a certain temperature it obeys this rate law. -1 rate = (0.799 M¹-s¯¹) [N₂0₂]² S Suppose a vessel contains N₂O5 at a concentration of 0.960M. Calculate the concentration of N₂O5 in the vessel 15.0 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. M x10 X G
Consider the two chemical reactions with their overall stoichiometries and corresponding rate laws shown. Rxn1: 2 N205 (g) 4 NO2 (g) * 02 (g) Rxn2: NO2 (g) + CO (g) → NO (g) CO2 (g) Rate = k [N205)2 Rate = k [NO2]0 By how much will the rate of each reaction be affected if the concentration of each reactant is doubled? Assume all other conditions are held constant. Use equations to justify your answer. a. By how much will the half-life of each reaction be affected if the concentration of each reactant is doubled? Assume all other conditions are held constant. Use equations to justify your answer. b.
Consider this reaction: 2N₂O5 (g) → 2N₂O4 (g) + O₂(g) At a certain temperature it obeys this rate law. = (0.291 M¹s¹) [N₂0₂] rate Suppose a vessel contains N₂O, at a concentration of 0.230 M. Calculate how long it takes for the concentration of N₂O to decrease to 23.0% of its initial value. You may assume no other reaction is important. Round your answer to 2 significant digits. ? Subm Continue Ⓒ2022 McGraw Hill LLC. All Rights Reserved. Terms of Use Privacy Cente 80°F Partly sunny ^ pe here to search B X G
Consider this reaction: 2N₂O, (e)- 2N₂O₂(g) + O₂(g) At a certain temperature it obeys this rate law. rate - (0.0664 M¹¹)[N₂05] Suppose a vessel contains N₂O, at a concentration of 0.870M. Calculate how long it takes for the concentration of N₂O, to decrease to 16.0% of its initial value. You may assume no other reaction is important. Round your answer to 2 significant digits. 0.P
26. Hydrogen reacts with nitrogen monoxide to form dinitrogen monoxide (laughing gas) according to the equation: H2(g)+2NO(g)⟶N2O(g)+H2O(g) Determine the rate law, the rate constant, and the orders with respect to each reactant from the following data: [NO] (M) 0.30 0.60 0.60 [H2] (M) 0.35 0.35 0.70 Rate (mol L−1 s−1) 2.835 × 10−3 1.134 × 10−2 2.268 × 10−2
Consider this reaction: H,CO, (ag) → H,0 (aq)+CO, (aq) At a certain temperature it obeys this rate law. rate = (0.0261 s')[H,Co,] [H,Co.] Suppose a vessel contains H,CO, at a concentration of 0.390M. Calculate the concentration of H,CO, in the vessel 40.0 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. M x10 Continue Submit Assign 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center Acces MacBook Air 80 DII DD F1 F3 F4 F5 F6 F7 F8 F9 F10