The rate of the following reaction has been found to be first-order with respect to hydroxyl ions and ethyl acetate: OH + CH3COCH₂CH3 CH3CO + CH3CH₂OH In a stirred-flow reactor of volume V = 0.602 L, the following data have been obtained at 298 K [Denbigh et al., Disc. Faraday Soc., 2 (1977) 263]: flow rate of barium hydroxide solution: flow rate of ethyl acetate solution: 1.16 L/h 1.20 L/h inlet concentration of OH: inlet concentration of ethyl acetate: outlet concentration of OH: Calculate the rate constant. Changes in volume accompanying the reaction are negligible. 0.00587 mol/L 0.0389 mol/L 0.001094 mol/L
The rate of the following reaction has been found to be first-order with respect to hydroxyl ions and ethyl acetate: OH + CH3COCH₂CH3 CH3CO + CH3CH₂OH In a stirred-flow reactor of volume V = 0.602 L, the following data have been obtained at 298 K [Denbigh et al., Disc. Faraday Soc., 2 (1977) 263]: flow rate of barium hydroxide solution: flow rate of ethyl acetate solution: 1.16 L/h 1.20 L/h inlet concentration of OH: inlet concentration of ethyl acetate: outlet concentration of OH: Calculate the rate constant. Changes in volume accompanying the reaction are negligible. 0.00587 mol/L 0.0389 mol/L 0.001094 mol/L
Introduction to Chemical Engineering Thermodynamics
8th Edition
ISBN:9781259696527
Author:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Publisher:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Chapter1: Introduction
Section: Chapter Questions
Problem 1.1P
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![The rate of the following reaction has been found to be first-order with respect to hydroxyl ions and ethyl acetate:
\[
\text{OH}^- + \text{CH}_3\text{COCH}_2\text{CH}_3 \rightarrow \text{CH}_3\text{CO}^- + \text{CH}_3\text{CH}_2\text{OH}
\]
In a stirred-flow reactor of volume \( V = 0.602 \, \text{L} \), the following data have been obtained at 298 K [Denbigh et al., Disc. Faraday Soc., 2 (1977) 263]:
- Flow rate of barium hydroxide solution: 1.16 L/h
- Flow rate of ethyl acetate solution: 1.20 L/h
- Inlet concentration of \(\text{OH}^-\): 0.00587 mol/L
- Inlet concentration of ethyl acetate: 0.0389 mol/L
- Outlet concentration of \(\text{OH}^-\): 0.001094 mol/L
Calculate the rate constant. Changes in volume accompanying the reaction are negligible.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fa44690e9-30d8-418e-a506-c4a735505b35%2F5aecaf4b-f8e7-4db4-abab-27bf18fab5cf%2Frzmfurr_processed.jpeg&w=3840&q=75)
Transcribed Image Text:The rate of the following reaction has been found to be first-order with respect to hydroxyl ions and ethyl acetate:
\[
\text{OH}^- + \text{CH}_3\text{COCH}_2\text{CH}_3 \rightarrow \text{CH}_3\text{CO}^- + \text{CH}_3\text{CH}_2\text{OH}
\]
In a stirred-flow reactor of volume \( V = 0.602 \, \text{L} \), the following data have been obtained at 298 K [Denbigh et al., Disc. Faraday Soc., 2 (1977) 263]:
- Flow rate of barium hydroxide solution: 1.16 L/h
- Flow rate of ethyl acetate solution: 1.20 L/h
- Inlet concentration of \(\text{OH}^-\): 0.00587 mol/L
- Inlet concentration of ethyl acetate: 0.0389 mol/L
- Outlet concentration of \(\text{OH}^-\): 0.001094 mol/L
Calculate the rate constant. Changes in volume accompanying the reaction are negligible.
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