At a certain temperature the rate of this reaction is first order in H₂CO, with a rate constant of 0.0158 s H_CO, (aq) —+ H,O(aq)+CO, (aq) Suppose a vessel contains H₂CO, at a concentration of 0.330M. Calculate how long it takes for the concentration of H₂CO, to decrease to 0.0363 M. You may assume no other reaction is important. Round your answer to 2 significant digits.
At a certain temperature the rate of this reaction is first order in H₂CO, with a rate constant of 0.0158 s H_CO, (aq) —+ H,O(aq)+CO, (aq) Suppose a vessel contains H₂CO, at a concentration of 0.330M. Calculate how long it takes for the concentration of H₂CO, to decrease to 0.0363 M. You may assume no other reaction is important. Round your answer to 2 significant digits.
Chemistry for Engineering Students
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Author:Lawrence S. Brown, Tom Holme
Publisher:Lawrence S. Brown, Tom Holme
Chapter11: Chemical Kinetics
Section: Chapter Questions
Problem 11.99PAE: Substances that poison a catalyst pose a major concern for many engineering designs, including those...
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![**Kinetics and Equilibrium: Using First- and Second-Order Integrated Rate Laws**
At a certain temperature, the rate of this reaction is first order in \( \text{H}_2\text{CO}_3 \), with a rate constant of \( 0.0158 \, \text{s}^{-1} \):
\[ \text{H}_2\text{CO}_3 (aq) \rightarrow \text{H}_2\text{O} (aq) + \text{CO}_2 (aq) \]
Suppose a vessel contains \( \text{H}_2\text{CO}_3 \) at a concentration of \( 0.330 \, \text{M} \). Calculate how long it takes for the concentration of \( \text{H}_2\text{CO}_3 \) to decrease to \( 0.0363 \, \text{M} \). You may assume no other reaction is important.
Round your answer to 2 significant digits.
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Transcribed Image Text:**Kinetics and Equilibrium: Using First- and Second-Order Integrated Rate Laws**
At a certain temperature, the rate of this reaction is first order in \( \text{H}_2\text{CO}_3 \), with a rate constant of \( 0.0158 \, \text{s}^{-1} \):
\[ \text{H}_2\text{CO}_3 (aq) \rightarrow \text{H}_2\text{O} (aq) + \text{CO}_2 (aq) \]
Suppose a vessel contains \( \text{H}_2\text{CO}_3 \) at a concentration of \( 0.330 \, \text{M} \). Calculate how long it takes for the concentration of \( \text{H}_2\text{CO}_3 \) to decrease to \( 0.0363 \, \text{M} \). You may assume no other reaction is important.
Round your answer to 2 significant digits.
**Input Box:**
An interactive section where users can enter their calculated result.
**Explanation and Check Buttons:**
- "Explanation" button provides detailed steps and solutions.
- "Check" button verifies if the entered answer is correct.
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Given : rate constant= 0.0158 s-1
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