with the second-order differential rate law and derive the second-order integrated rate law. 116. The rate constant for the first-order decomposition of N2O;(g) to at a given temperature. NO2(g) and O2(g) is 7.48 × 10-3 s-1 a. Find the length of time required for the total pressure in a system containing N,O5 at an initial pressure of 0.100 atm to rise to 0.145 atm. b. Find the length of time required for the total pressure in a system containing N,O5 at an initial pressure of 0.100 atm to rise to 0.200 atm. c. Find the total pressure after 100 s of reaction. 117. Phosgene (Cl,CO), a poison gas used in World War I, is formed by the reaction of Cl2 and CO. The proposed mechanism for the reaction is: Cl2 2 Cl Fast, equilibrium Cl + CO CICO Fast, equilibrium CICO + Cl2 C12CO + Cl Slow What rate law is consistent with this mechanism? 118. The rate of decomposition of N,O3(g) to NO2(g) and NO(g) is monitored by measuring [NO2] at different times. The following tabulated data are obtained. [NO2](mol/L) 0.193 0.316 0.427 0.784 t(s) 884 1610 2460 50,000 The reaction follows a first-order rate law. Calculate the rate constant. Assume that after 50,000 s all the N,O3(g) had decomposed. k1 119. At 473 K, for the elementary reaction 2 NOCI(g) 2 NO(g) + Cl,(g) k-1 k1 : = 7.8 × 10-2 L/mol s and k-1 = 4.7 × 10² L²/mol? s A sample of NOCI is placed in a container and heated to 473 K. •1:1
with the second-order differential rate law and derive the second-order integrated rate law. 116. The rate constant for the first-order decomposition of N2O;(g) to at a given temperature. NO2(g) and O2(g) is 7.48 × 10-3 s-1 a. Find the length of time required for the total pressure in a system containing N,O5 at an initial pressure of 0.100 atm to rise to 0.145 atm. b. Find the length of time required for the total pressure in a system containing N,O5 at an initial pressure of 0.100 atm to rise to 0.200 atm. c. Find the total pressure after 100 s of reaction. 117. Phosgene (Cl,CO), a poison gas used in World War I, is formed by the reaction of Cl2 and CO. The proposed mechanism for the reaction is: Cl2 2 Cl Fast, equilibrium Cl + CO CICO Fast, equilibrium CICO + Cl2 C12CO + Cl Slow What rate law is consistent with this mechanism? 118. The rate of decomposition of N,O3(g) to NO2(g) and NO(g) is monitored by measuring [NO2] at different times. The following tabulated data are obtained. [NO2](mol/L) 0.193 0.316 0.427 0.784 t(s) 884 1610 2460 50,000 The reaction follows a first-order rate law. Calculate the rate constant. Assume that after 50,000 s all the N,O3(g) had decomposed. k1 119. At 473 K, for the elementary reaction 2 NOCI(g) 2 NO(g) + Cl,(g) k-1 k1 : = 7.8 × 10-2 L/mol s and k-1 = 4.7 × 10² L²/mol? s A sample of NOCI is placed in a container and heated to 473 K. •1:1
Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter13: Chemical Kinetics
Section: Chapter Questions
Problem 13.99QE
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I'm not sure how to do question 118
![with the second-order differential rate law and derive the
second-order integrated rate law.
116. The rate constant for the first-order decomposition of N2O;(g) to
at a given temperature.
NO2(g) and O2(g) is 7.48 × 10-3 s-1
a. Find the length of time required for the total pressure in a
system containing N,O5 at an initial pressure of 0.100 atm to
rise to 0.145 atm.
b. Find the length of time required for the total pressure in a
system containing N,O5 at an initial pressure of 0.100 atm to
rise to 0.200 atm.
c. Find the total pressure after 100 s of reaction.
117. Phosgene (Cl,CO), a poison gas used in World War I, is formed
by the reaction of Cl2 and CO. The proposed mechanism for the
reaction is:
Cl2
2 Cl
Fast, equilibrium
Cl + CO
CICO
Fast, equilibrium
CICO + Cl2
C12CO + Cl Slow
What rate law is consistent with this mechanism?
118. The rate of decomposition of N,O3(g) to NO2(g) and NO(g) is
monitored by measuring [NO2] at different times. The following
tabulated data are obtained.
[NO2](mol/L)
0.193
0.316
0.427
0.784
t(s)
884
1610
2460
50,000
The reaction follows a first-order rate law. Calculate the rate
constant. Assume that after 50,000 s all the N,O3(g) had
decomposed.
k1
119. At 473 K, for the elementary reaction 2 NOCI(g)
2 NO(g) + Cl,(g)
k-1
k1 :
= 7.8 × 10-2 L/mol s and
k-1
= 4.7 × 10² L²/mol? s
A sample of NOCI is placed in a container and heated to 473 K.
•1:1](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F37c49ffc-d941-453a-b990-121f54a1645c%2Fb27da170-f086-402b-8001-055005976760%2Fpr3pznn.png&w=3840&q=75)
Transcribed Image Text:with the second-order differential rate law and derive the
second-order integrated rate law.
116. The rate constant for the first-order decomposition of N2O;(g) to
at a given temperature.
NO2(g) and O2(g) is 7.48 × 10-3 s-1
a. Find the length of time required for the total pressure in a
system containing N,O5 at an initial pressure of 0.100 atm to
rise to 0.145 atm.
b. Find the length of time required for the total pressure in a
system containing N,O5 at an initial pressure of 0.100 atm to
rise to 0.200 atm.
c. Find the total pressure after 100 s of reaction.
117. Phosgene (Cl,CO), a poison gas used in World War I, is formed
by the reaction of Cl2 and CO. The proposed mechanism for the
reaction is:
Cl2
2 Cl
Fast, equilibrium
Cl + CO
CICO
Fast, equilibrium
CICO + Cl2
C12CO + Cl Slow
What rate law is consistent with this mechanism?
118. The rate of decomposition of N,O3(g) to NO2(g) and NO(g) is
monitored by measuring [NO2] at different times. The following
tabulated data are obtained.
[NO2](mol/L)
0.193
0.316
0.427
0.784
t(s)
884
1610
2460
50,000
The reaction follows a first-order rate law. Calculate the rate
constant. Assume that after 50,000 s all the N,O3(g) had
decomposed.
k1
119. At 473 K, for the elementary reaction 2 NOCI(g)
2 NO(g) + Cl,(g)
k-1
k1 :
= 7.8 × 10-2 L/mol s and
k-1
= 4.7 × 10² L²/mol? s
A sample of NOCI is placed in a container and heated to 473 K.
•1:1
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