Consider this reaction: 2Cl,0, (g) - 2C1, (g) + 50, (3) At a certain temperature it obeys this rate law. rate = (12.5 M-1. Suppose a vessel contains Cl,0, at a concentration of 0.880 M. Calculate how long it takes for the concentration of Cl,0, to decrease to 0.114 M. You may assume no other reaction is important. Round your answer to 2 significant digits.

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Using first- and second-order integrated rate laws
Stella v
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Consider this reaction:
2Cl,0, (g) → 2C1, (g) + 50, (g)
At a certain temperature it obeys this rate law.
= (125 M-1.)[C1,0,
團
Suppose a vessel contains Cl,0, at a concentration of 0.880 M. Calculate how long it takes for the concentration of Cl,0, to decrease to 0.114 M. You may
assume no other reaction is important.
Round your answer to 2 significant digits.
Explanation
Recheck
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Transcribed Image Text:https://www-awn.aleks.com/alekscgi/x/Isl.exe/1o_u-lgNslkr7j8P3jH-IBInzn17HUz2IYCcR4NM7yr_lpMriNwxOI *** O KINETICS AND EQUILIBRIUM Try again. Using first- and second-order integrated rate laws Stella v Try Again Consider this reaction: 2Cl,0, (g) → 2C1, (g) + 50, (g) At a certain temperature it obeys this rate law. = (125 M-1.)[C1,0, 團 Suppose a vessel contains Cl,0, at a concentration of 0.880 M. Calculate how long it takes for the concentration of Cl,0, to decrease to 0.114 M. You may assume no other reaction is important. Round your answer to 2 significant digits. Explanation Recheck O 2021 McGraw-Hil Education. All Rights Rserved. Terms of Use Privacy Accessibility P Type here to search 11:02 AM 2/4/2021
Expert Solution
Step 1 :- Given Details

Rate = (12.5 M-1 s-1) [Cl2O5]2

Rate contant, K = 12.5 M-1 s-1

This implies;

Given reaction is second order.

Initial concentration of [Cl2O5] , [A]o = 0.880 M

Final concentration of [Cl2O5] , [A] = 0.114 M

 

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