The chemical reaction A → C + D is known to be second order with respect to the concentration of reactant [A] and second order overall. The rate constant for the disappearance of A is 0.0525 L/mol·min at 100°C, with an activation energy of 95.0 kJ/mol. Substance A is placed in a container at an initial concentration of 7.50 M. How long will it take for the concentration of A to fall to 0.500 M?
The chemical reaction A → C + D is known to be second order with respect to the concentration of reactant [A] and second order overall. The rate constant for the disappearance of A is 0.0525 L/mol·min at 100°C, with an activation energy of 95.0 kJ/mol. Substance A is placed in a container at an initial concentration of 7.50 M. How long will it take for the concentration of A to fall to 0.500 M?
Introduction to Chemical Engineering Thermodynamics
8th Edition
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Author:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
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Chapter1: Introduction
Section: Chapter Questions
Problem 1.1P
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![The chemical reaction A → C + D is known to be second order with respect to the
concentration of reactant [A] and second order overall. The rate constant for the disappearance
of A is 0.0525 L/mol·min at 100°C, with an activation energy of 95.0 kJ/mol.
ii. Substance A is placed in a container at an initial concentration of 7.50 M. How long will it take
for the concentration of A to fall to 0.500 M?
iii. The reaction is run again with the same initial concentration of A but at a temperature of 125°C.
How long will it take to reach the same final concentration?](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F2e2aebe5-d113-466b-915f-65981f2c201e%2F2a84521b-9a70-403f-afc7-dc5dec10b169%2F81yrxmg_processed.png&w=3840&q=75)
Transcribed Image Text:The chemical reaction A → C + D is known to be second order with respect to the
concentration of reactant [A] and second order overall. The rate constant for the disappearance
of A is 0.0525 L/mol·min at 100°C, with an activation energy of 95.0 kJ/mol.
ii. Substance A is placed in a container at an initial concentration of 7.50 M. How long will it take
for the concentration of A to fall to 0.500 M?
iii. The reaction is run again with the same initial concentration of A but at a temperature of 125°C.
How long will it take to reach the same final concentration?
Expert Solution
Introduction
This problem is based on Chemical reaction Engineering.
Data given :
Reaction :
A ---> C + D
Overall reaction order = 2
Activation energy = 98 kJ/ mol
Rate constant , k1 at 100 degree C (= 100 + 273 K = 373 K) = 0.0525 L/ mol.min
For part (i):
Initial Concentration of A = 7.50 M= 7.50 mol / L
Final Concentration of A = 0.500 M = 0.500 mol /L
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