10.19. A chemical reaction with stoichiometry A → products is said to follow an nh-order rate law if A is consumed at a rate proportional to the nth power of its concentration in the reaction mixture. If ra is the rate of consumption of A per unit reactor volume, then ra[mol/(L-s)] = kC, where CA(mol/L) is the reactant concentration, and the constant of proportionality k is the reaction rate constant. A reaction that follows this law is referred to as an nh order reaction. The rate constant is a strong function of temperature but is independent of the reactant concentration. (a) Suppose a first-order reaction (n = 1) is carried out in an isothermal batch reactor of constant volume V. Write a material balance on A and integrate it to derive the expression CA = CA0 exp(-kt) where CA0 is the concentration of A in the reactor at t = 0. (b) The gas-phase decomposition of sulfuryl chloride SO2CI2 → SO2 + Cl2 is thought to follow a first-order rate law. The reaction is carried out in a constant-volume isothermal batch reactor and the concentration of SO,Cl, is measured at several reaction times, with the following results: 1(min) 4.0 21.3 39.5 63.4 120.0 175.6 CA(mol/L) | 0.0279 | 0.0262 | 0.0246 0.0226 | 0.0185 | 0.0152 Verify the proposed rate law graphically [i.e., demonstrate that the expression given in Part (a) fits the data for CA(t)] and determine the rate constant k, giving both its value and its units.
10.19. A chemical reaction with stoichiometry A → products is said to follow an nh-order rate law if A is consumed at a rate proportional to the nth power of its concentration in the reaction mixture. If ra is the rate of consumption of A per unit reactor volume, then ra[mol/(L-s)] = kC, where CA(mol/L) is the reactant concentration, and the constant of proportionality k is the reaction rate constant. A reaction that follows this law is referred to as an nh order reaction. The rate constant is a strong function of temperature but is independent of the reactant concentration. (a) Suppose a first-order reaction (n = 1) is carried out in an isothermal batch reactor of constant volume V. Write a material balance on A and integrate it to derive the expression CA = CA0 exp(-kt) where CA0 is the concentration of A in the reactor at t = 0. (b) The gas-phase decomposition of sulfuryl chloride SO2CI2 → SO2 + Cl2 is thought to follow a first-order rate law. The reaction is carried out in a constant-volume isothermal batch reactor and the concentration of SO,Cl, is measured at several reaction times, with the following results: 1(min) 4.0 21.3 39.5 63.4 120.0 175.6 CA(mol/L) | 0.0279 | 0.0262 | 0.0246 0.0226 | 0.0185 | 0.0152 Verify the proposed rate law graphically [i.e., demonstrate that the expression given in Part (a) fits the data for CA(t)] and determine the rate constant k, giving both its value and its units.
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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![10.19. A chemical reaction with stoichiometry A → products is said to follow an nh-order rate law if A is
consumed at a rate proportional to the nth power of its concentration in the reaction mixture. If ra is
the rate of consumption of A per unit reactor volume, then
ra[mol/(L-s)] = kC,
where CA(mol/L) is the reactant concentration, and the constant of proportionality k is the reaction
rate constant. A reaction that follows this law is referred to as an nh order reaction. The rate constant
is a strong function of temperature but is independent of the reactant concentration.
(a) Suppose a first-order reaction (n = 1) is carried out in an isothermal batch reactor of constant
volume V. Write a material balance on A and integrate it to derive the expression
CA = CA0 exp(-kt)
where CA0 is the concentration of A in the reactor at t = 0.
(b) The gas-phase decomposition of sulfuryl chloride
SO2CI2 → SO2 + Cl2
is thought to follow a first-order rate law. The reaction is carried out in a constant-volume
isothermal batch reactor and the concentration of SO,Cl, is measured at several reaction times,
with the following results:
1(min)
4.0
21.3
39.5
63.4
120.0
175.6
CA(mol/L) | 0.0279 | 0.0262 | 0.0246 0.0226 | 0.0185 | 0.0152
Verify the proposed rate law graphically [i.e., demonstrate that the expression given in Part (a) fits
the data for CA(t)] and determine the rate constant k, giving both its value and its units.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fc12ab97c-f8f1-4017-b9a2-ab223869998c%2F0d35b7b2-5f59-4a97-8b33-9279788d7dbb%2F4n3hnc_processed.png&w=3840&q=75)
Transcribed Image Text:10.19. A chemical reaction with stoichiometry A → products is said to follow an nh-order rate law if A is
consumed at a rate proportional to the nth power of its concentration in the reaction mixture. If ra is
the rate of consumption of A per unit reactor volume, then
ra[mol/(L-s)] = kC,
where CA(mol/L) is the reactant concentration, and the constant of proportionality k is the reaction
rate constant. A reaction that follows this law is referred to as an nh order reaction. The rate constant
is a strong function of temperature but is independent of the reactant concentration.
(a) Suppose a first-order reaction (n = 1) is carried out in an isothermal batch reactor of constant
volume V. Write a material balance on A and integrate it to derive the expression
CA = CA0 exp(-kt)
where CA0 is the concentration of A in the reactor at t = 0.
(b) The gas-phase decomposition of sulfuryl chloride
SO2CI2 → SO2 + Cl2
is thought to follow a first-order rate law. The reaction is carried out in a constant-volume
isothermal batch reactor and the concentration of SO,Cl, is measured at several reaction times,
with the following results:
1(min)
4.0
21.3
39.5
63.4
120.0
175.6
CA(mol/L) | 0.0279 | 0.0262 | 0.0246 0.0226 | 0.0185 | 0.0152
Verify the proposed rate law graphically [i.e., demonstrate that the expression given in Part (a) fits
the data for CA(t)] and determine the rate constant k, giving both its value and its units.
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