What was the initial concentration of A if k = 8.75 × 10 2 s 1? For - ProProfs Discuss
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What was the initial concentration of A if k = 8.75 × 10-2 s-1? For the first-order reaction below, the concentration of product B after 24.2 seconds is 0.322 M. A → 2B rate = k[



A. 0.0341 M
B. 0.183 M
C. 1.34 M
D. 2.68 M
E. 29.3 M

This question is part of CHEM 2425
Asked by Ochiengj, Last updated: Feb 15, 2020

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1 Answer

John Smith

John Smith

Answered Dec 10, 2016

0.183 M

Solving: Initial Final A X X -x B 0 2x = 0.322 x= 0.166 lnX/X-0.166 = kt= 8.75 10?-2 24.2 = 2.1175 X/X-0.166 = e2.1175 =8.31 X = 8.31X 1.38 7.31X = 1.38 X = 0.188M 24. For the first-order reaction below, the concentration of product B after 24.2 seconds is 0.322 M. If k = 8.75 10-2 s-1, what was the initial concentration of A? A 2B rate = k[A] a. 0.0341 M b. 0.183 M c. 1.34 M d. 2.68 M e. 29.3 M ln 0.322 M/ [A]0 = 8.75 10-2 s-1 24.2 s = 2.12 e2.12 = 0.322 M/ [A]0 8.33 = 0.322 M/ [A]0 [A]0 = 0.322 /8.33 = 0.0386 M
 

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