201₂05 (8)→201₂ (8) ¹0₂ (8) a certain temperature it obeys this rate law. rate = (1.30 s¯¹)[C1₂05] ppose a vessel contains Cl₂O, at a concentration of 0.120M. Calculate the concentration of Cl₂O5 in the vessel 0.890 seconds later. You may assume no her reaction is important. und your answer to 2 significant digits. M

201₂05 (8)→201₂ (8) ¹0₂ (8) a certain temperature it obeys this rate law. rate = (1.30 s¯¹)[C1₂05] ppose a vessel contains Cl₂O, at a concentration of 0.120M. Calculate the concentration of Cl₂O5 in the vessel 0.890 seconds later. You may assume no her reaction is important. und your answer to 2 significant digits. M

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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At a certain temperature the rate of this reaction is second order in HI with a rate constant of 1.96 M 2HI (g) → H₂(g) + 1₂ (8) Suppose a vessel contains HI at a concentration of 1.18M. Calculate the concentration of HI in the vessel 3.50 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. M X S ? Submit As Continue Ⓒ2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center 80°F Partly sunny ere to search 81 (=
At a certain temperature the rate of this reaction is second order in NH,OH with a rate constant of 25.4 M s: NH,OH (aq)NH;(aq)+H,0(aq) Suppose a vessel contains NH,OH at a concentration of 1.33 M. Calculate the concentration of NH, OH in the vessel 0.240 seconds later. You may assum other reaction is important. Round your answer to 2 significant digits. M x10
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Smail ||| YouTube O KINETICS AND EQUILIBRIUM Using an integrated rate law for a first-order reaction At a certain temperature the rate of this reaction is first order in NH4OH with a rate constant of 0.0108 s NH,OH(aq). } → NH, (aq) +H,O(aq) Translate M Suppose a vessel contains NH4OH at a concentration of 1.24 M. Calculate the concentration of NH OH in the vessel 63.0 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. Explanation 82°F Mostly cloudy Check 0/5 Q Search © 2023 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | 1
A certain reaction is first order in H, and first order in I,. Use this information to complete the table below. Round each of your answers to 3 significant digits. [4.] [+] initial rate of reaction Calculator 圖 х10 0.429 M 0.563 M 0.0218 M/s olo 0.429 M 1.36 M |M/s 18 Ar I M/s 0.0981 M 2.46 M
Hi I need help with the last 2 questions
The following data were collected for the reaction: 2A > 4B + C Time Concentration of A Concentration of B (minutes) (moles/L) (moles/L) 1.000 0.000 10 0.800 0.400 20 0.667 0.677 30 0.571 0.858 40 0.500 1.000 50 0.444 1.112 1. Make a graph of the concentrations of A and B versus time. Estimate the rate of disappearance of A and the rate of formation of B at t= 25 min and at t= 40 min. Compare the rates of disappearance of A and formation of B. What would you expect the rate of formation of C to be at t= 25 min and t=40 min? 2. Determine graphically whether the reaction in #1 above is a first order or a second order reaction. Calculate the rate constant for the reaction.
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8 OKONETICS AND EQUILIBRIUM Deducing a rate law from the change in concentration over time A chemistry graduate student is studying the rate of this reaction: 2N₂O, (g) → 2N₂O, (g) + O₂(g) He fills a reaction vessel with N₂O, and measures its concentration as the reaction proceeds: time (minutes) 0 10. [N₂O,] Explanation 0.300M 0.121 M 20. 0.0762 M 30. 0.0555 M 40. 0.0436M Use this data to answer the following questions. Write the rate law for this reaction. Calculate the value of the rate constant k Round your answer to 2 significant digits. Also be sure your answer has the correct unit symbol. Check rate & D www-awa.aleks.com k= D.D X
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Consider the reaction described by the equation C,H,Br, (aq) + 3 I (aq) C,H, (g) + 2 Br¯(aq) + I5 (aq) The rate law is rate = k[C,H¸Br,][I¯] where k = 0.00504 M-1. s-1. What are the missing entries in the table? Run [C,H,Br,h (M). [I¯], (M) Initial rate of formation of C,H, (M-s) 1 0.162 0.000529 0.162 y 0.000265 3 0.162 0.162 M X = M y = z = M-s-1