Using a second-order integrated rate law to find concentration change-1 -1At a certain temperature this reaction follows second-order kinetics with a rate constant of 0.0107 M .S2NH3 (g) → N2 (g) + 3H2(g):Suppose a vessel contains NH3 at a concentration of 0.610M. Calculate the concentration of NH3 in the vessel 870. seconds later. You mayassume no other reaction is important.Round your answer to 2 significant digits.Шм☐ x10☑00.Ar

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Answered: Using a second-order integrated rate…

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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= 5 = 6 = 7 = 8 9 = 10 = 11 12 13 = 14 At a certain temperature this reaction follows second-order kinetics with a rate constant of 0.0162 M.s: NH,OH (ag) → NH, (aq) +H,0 (aq) Suppose a vessel contains NH,OH at a concentration of 0.700 M. Calculate the concentration of NH,OH in the vessel 590. seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. OM Continue Submit Assignment O 2021 McGraw-Hill Education. All Rights Reserved. Terms of Use I Privacy Accessibility
-1. Under certain conditions the rate of this reaction is zero order in dinitrogen monoxide with a rate constant of 0.0058 M-s: 2N₂O(g) → 2N₂ (g) +0₂ (8) Suppose a 2.0 L flask is charged under these conditions with 450. mmol of dinitrogen monoxide. After how much time is there only 225. mmol left? You may assume no other reaction is important. Be sure your answer has a unit symbol, if necessary, and round it to 2 significant digits. 0 S Ala X 2. ?
1
Consider the following reaction: 12 (g) + H2 (g) --> 2 HI (g). Given the mechanism below, determine the rate law for the equation. Note: input the rate law following the format rate-k[A]2[B2] with no spaces don't worry about formatting upper or lower case. 1₂ (g) 21 (g) (fast) H₂ (9)+21 (g) → 2HI (g) (slow)
Consider the gas-phase reaction: H2(g) + 12(g) → 2 HI(g) The reaction was experimentally determined to be first order in H₂ and first order in 12. Consider the proposed mechanisms. Mechanism 1: H2(g) + 2(g) 2 HI(g) single step k₁ Mechanism 2: 12(g) k_1 21(g) fast H2 212 HI(g) slow K2 *Draw energy diagrams for the mechanisms shown: Show that both of the proposed mechanisms are valid.
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
F8 =9 =10 = 11 = 12 = 13 14 = 15 16 18 19 At a certain temperature this reaction follows second-order kinetics with a rate constant of 0.0618M-¹.s-¹: 2NH3 (g) → N₂ (g) + 3H₂ (g) Suppose a vessel contains NH3 at a concentration of 1.25 M. Calculate the concentration of NH3 in the vessel 68.0 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. OM ? Su ontinue 0 10 X S hp
The decomposition of N2O5 in solution in carbon tetrachloride is a first-order reaction. 2N2O5 → 4NO2 + O2 The rate constant at a given temperature is found to be 5.25 x 10-4 s-1. If the initial concentration of N2O5 is 0.11 M, what is its concentration after exactly 11 minutes have passed? Round your answer to 2 decimal places.
Consider the mechanism. O3 + NO, – NO, + O, NO, + NO, – N,O5 slow fast O, + 2 NO, – 0, + N,O5 Identify the rate law for the overall reaction based on the mechanism. rate = k[O,||NO,? rate = k[O3] rate = k[O3][NO,1 rate = k[NO,? k[NO, ][NO3] rate =
Consider the hypothetical reaction A(g) + B(g) C(g) The four containers below represent this reaction being run with different initial amounts of A and B. Assume that the volume of each container is 1.0L. The reaction is second order with respect to A and first order in respect to B. Which of the containers, W,X,Y or Z, would have the greatest reaction rate? Justify your answer.
At a certain temperature the rate of this reaction is second order in CICH₂CH₂Cl with a rate constant of 0.00455 M S -1 CICH₂CH₂Cl (g) → CH₂CHC1 (g) + HC1 (g) Suppose a vessel contains CICH₂CH₂Cl at a concentration of 1.11 M. Calculate the concentration of CICH₂CH₂Cl in the vessel 900. seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits.
Using an integrated rate law for a first-order reaction At a certain temperature this reaction follows first-order kinetics with a rate constant of 0.141 s¯¹: H₂CO3(aq) → H₂O (aq) + CO₂ (aq) Suppose a vessel contains H₂CO3 at a concentration of 0.290M. Calculate the concentration of H₂CO3 in the vessel 4.40 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. M x10 X Ś

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