Using a second-order integrated rate law to find concentration changeAt a certain temperature the rate of this reaction is second order in Cl2O5 with a rate constant of 0.0752M2C1205 (g) →2Cl2(g) +502 (g)1-1.S:Suppose a vessel contains C₁₂05 at a concentration of 0.280 M. Calculate the concentration of C1205 in the vessel 190. seconds later. Youmay assume no other reaction is important.Round your answer to 2 significant digits.M☐ x10☑

Step 1: Write the Rate Law for a Second-Order ReactionThe rate law for a second-order reaction…

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
At a certain temperature the rate of this reaction is first order in N₂O5 with a rate constant of 0.0125 s¯¹: 2N₂O5 (g) → 2N₂O4 (8) + 0₂ (8) Suppose a vessel contains N₂O5 at a concentration of 1.14M. Calculate the concentration of N₂O5 in the vessel 88.0 seconds later. You may assume no of reaction is important. Round your answer to 2 significant digits.
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 nitrous oxide at 565 °C N,0(g)N2(g) +½ O2(g) is second order in N2O with a rate constant of 1.10x10-3 M's. If the initial concentration of N20 is 2.08 M, the concentration of N,0 will be |M after 3.30x103 seconds have passed.
Nitrification is a biological process for removing NH3 from wastewater as NH4+: NH, +20, → NO3 + 2H + H2O The first-order rate constant is given as k₁ = 0.47e0.095(T-15°C) where k₁ is in day¹ and T is in °C. If the initial concentration of NH3 is 3.0 mol/m³, how long will it take to reduce the concentration to 0.66 mol/m³: (a) in the spring (T = 20°C)? days (b) in the winter (T = 10°C)? days
5
At a certain temperature the rate of this reaction is second order in NH OH with a rate constant of 0.0123 M¹s¹: NH,OH (aq) → NH, (aq)+H,O(aq) Suppose a vessel contains NH OH at a concentration of 0.690 M. Calculate the concentration of NH OH in the vessel 790. seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. X
At a certain temperature the rate of this reaction is second order in H₂CO3 with a rate constant of 2.75Ms H₂CO3(aq) → H₂O (aq) + CO₂ (aq) Suppose a vessel contains H₂CO3 at a concentration of 0.130M. Calculate how long it takes for the concentration of H₂CO3 to decrease to 0.0286 M. You may assume no other reaction is important. Round your answer to 2 significant digits. X ? S
The gas phase decomposition of sulfuryl chloride at 600 K SO₂ Cl₂ (g) → SO₂ (g)+ Cl₂ (g) is first order in SO₂ Cl2 with a rate constant of 2.80 × 10-³ min-¹. If the initial concentration of SO₂ Cl2 is 0.00164 M, the concentration of SO₂ Cl2 will be 0.000364 M after min have passed.
Q2) Consider the following third order reaction: A➜ product The following is the integrated rate law for the third order reaction: 2[A];² 11/2 = kt + 1.5 K[A]0² 2[A]o² If the concentration of the reactant after 26.5 second of the experiment was found to 0.348 M and the rate constant for this reaction was found to be 1.5x10¹² M².S¹. a) Determine the initial concentration of the reactant. b) What is the half-life of this reaction? c) What is the concentration of the reactants after 1.00 min of the experiment?
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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