The decomposition of N2O5 can be described by the equation2N₂O₂(soln)-4 NO2 (soln) + O2(g)Consider the data in the table for the reaction at 45 °C in carbon tetrachloride solution.(s)0[N2O5] (M)1.8491451.6884161.4237451.157Given the data, calculate the average rate of reaction for each successive time interval.What is the average rate of reaction for the time interval from 0s to 145 s?1.11 ×10¯³-3average rate of reaction:Question Source: McQuarrie, Rock, And Gallogly 4e - General Chemistry | Publisher: University Science BooksM/s of 19>average rate of reaction:1.11 ×10−3IncorrectWhat is the average rate of reaction for the time interval from 145 s to 416 s?9.78 ×10-8average rate of reaction:IncorrectWhat is the average rate of reaction for the time interval from 416 s to 745 s?average rate of reaction:8.09 ×10-4Incorrect> Attempt 1M/sM/s123Question Source: McQuarrie, Rock, And Gallogly 4e - General Chemistry | Publisher: University Science Books::

The balanced chemical equation is:2N2O5→4NO2+O2The rate of chemical equation will…

Answered: The decomposition of N2O5 can be…

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: 2N₂O5 (g) → 2N₂O4 (g) + O₂(g) At a certain temperature it obeys this rate law. rate = (0.0317 M¹-s¯¹) [₂0₂] S Suppose a vessel contains N₂O5 at a concentration of 0.440 M. Calculate the concentration of N₂O5 in the vessel 480. seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. M x10 ? X S
Consider this reaction: H₂CO3(aq) → H₂O (aq) + CO₂ (aq) At a certain temperature it obeys this rate law. =(0.0152 s¹)[H₂CO3] rate = Suppose a vessel contains H₂CO3 at a concentration of 0.250M. Calculate the concentration of H₂CO3 in the vessel 56.0 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. M X
Consider this reaction: 2N₂O5 (g) → 2N₂O4 (g) +O₂ (g) At a certain temperature it obeys this rate law. rate = (0.0328 s−¹)[N₂05] S Suppose a vessel contains N₂O5 at a concentration of 0.860M. Calculate the concentration of N₂O5 in the vessel 22.0 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. M x10 X Ś
A chemistry graduate student is studying the rate of this reaction: 250, (g)2SO₂ (g) + O₂ (g) She fills a reaction vessel with SO, and measures its concentration as the reaction proceeds: time (minutes) 0 10. 20. [So, 0.400M 0.118 M 0.0693 M 30. 0.0490M 40. 0.0379 M 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. rate = 0 of 0 D+D X 09
Consider following reaction: 2 A2B5(g) → 4AB2(g) + B2(g) The rate constant is 0.129 s-1 at 298 K for this reaction. What is the percent of A2B5 left after the first 19.091 s? Report your answer with three decimals. Enter numbers only;
The following mechanism has been suggested for a reaction: NO(g) + Br2(g) → NOBR2(g) fast NOBR2(g) + NO(g) 2 NOBr(g) slow (a) What is the overall reaction? (b) What are the intermediates in the mechanism? (c) What is the rate law for the reaction? Edit View Insert Format Tools Table 12pt v Paragraph B IUA IMG F4 F5 F6 E10
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2. Fill in the following chart. pH [OH] рон A/B/N 6.55 -8 10 3.05 -6 3.34 X 10

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