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At a certain temperature this reaction follows first-order kinetics with a rate constant of 4.6 s 2H;PO, (aq) → P,O5 (aq) +3H,0 (aq) Suppose a vessel contains H,PO, at a concentration of 1.39M. Calculate how long it takes for the concentration of H,PO, to decrease by 93.%. You may assume no other reaction is important. Round your answer to 2 significant digits.

At a certain temperature this reaction follows first-order kinetics with a rate constant of 4.6 s 2H;PO, (aq) → P,O5 (aq) +3H,0 (aq) Suppose a vessel contains H,PO, at a concentration of 1.39M. Calculate how long it takes for the concentration of H,PO, to decrease by 93.%. You may assume no other reaction is important. Round your answer to 2 significant digits.

Chemistry: The Molecular Science
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter11: Chemical Kinetics: Rates Of Reactions
Section: Chapter Questions
Problem 39QRT
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At a certain temperature this reaction follows first-order kinetics with a rate constant of 4.6 s 2H,РО, (ад) — Р,0, (аg) +зн,о (аq) Suppose a vessel contains H,PO, at a concentration of 1.39M. Calculate how long it takes for the concentration of H,PO, to decrease by 93.%. You may 4 assume no other reaction is important. Round your answer to 2 significant digits. S х10
Transcribed Image Text:At a certain temperature this reaction follows first-order kinetics with a rate constant of 4.6 s 2H,РО, (ад) — Р,0, (аg) +зн,о (аq) Suppose a vessel contains H,PO, at a concentration of 1.39M. Calculate how long it takes for the concentration of H,PO, to decrease by 93.%. You may 4 assume no other reaction is important. Round your answer to 2 significant digits. S х10
Expert Solution
Step 1

Given reaction: 2H3PO4 (aq) → P2O5 (aq) + 3H2O (aq)

Given, the initial concentration of H3PO4 = 1.39 M

The rate constant = 4.6 s-1

We have to calculate the time required for the concentration of H3PO4 to decrease by 93%.

 

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