2. The reaction H2 (g) + 2 NO (g) → N,O (g) + H,O (g) is studied at a certain tempera- ture by determining the rate of reaction at reactant concentrations. The results are as follows. Concentration (M) Rate [NO] [H2] (M/s) (i) 0.25 0.10 0.126 (ii) 0.50 0.10 0.504 (iii) 0.50 0.20 1.03 The rate law is written as Rate = order with respect to NO and H2, respectively. Calculate the value of x and y from the data provided. k [NO]* [H2]v. The exponents x and y represent the %3D 3. The decomposition of N2O5 in carbon tetrachloride has been studied: 2 N,O5 (g) 2 N,O4 (g) + O2 (g) The concentration of N,O5 is measured every 400 seconds. The data are tabulated below. [N2O5] (M) A[N¿O5] (M) Rate = -A[N2O5]/At (M/s) At %3D time (s) (s) 0.0 1.40 400.0 1.10 800.0 0.87 1200.0 0.68 a) Fill the blanks in the table. Note that the last column is the average rate of reaction. b) Briefly explain why the rates are decreasing.
2. The reaction H2 (g) + 2 NO (g) → N,O (g) + H,O (g) is studied at a certain tempera- ture by determining the rate of reaction at reactant concentrations. The results are as follows. Concentration (M) Rate [NO] [H2] (M/s) (i) 0.25 0.10 0.126 (ii) 0.50 0.10 0.504 (iii) 0.50 0.20 1.03 The rate law is written as Rate = order with respect to NO and H2, respectively. Calculate the value of x and y from the data provided. k [NO]* [H2]v. The exponents x and y represent the %3D 3. The decomposition of N2O5 in carbon tetrachloride has been studied: 2 N,O5 (g) 2 N,O4 (g) + O2 (g) The concentration of N,O5 is measured every 400 seconds. The data are tabulated below. [N2O5] (M) A[N¿O5] (M) Rate = -A[N2O5]/At (M/s) At %3D time (s) (s) 0.0 1.40 400.0 1.10 800.0 0.87 1200.0 0.68 a) Fill the blanks in the table. Note that the last column is the average rate of reaction. b) Briefly explain why the rates are decreasing.
Chemistry & Chemical Reactivity
9th Edition
ISBN:9781133949640
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter14: Chemical Kinetics: The Rates Of Chemical Reactions
Section: Chapter Questions
Problem 12PS: The reaction 2 NO(g) + 2 H2(g) N2(g) + 2 H2O(g) was studied at 904 C, and the data in the table...
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Question
3a
![2. The reaction H2 (g) + 2 NO (g) → N,O (g) + H,O (g) is studied at a certain tempera-
ture by determining the rate of reaction at reactant concentrations. The results are as
follows.
Concentration (M)
Rate
[NO]
[H2]
(M/s)
(i)
0.25
0.10
0.126
(ii)
0.50
0.10
0.504
(iii)
0.50
0.20
1.03
The rate law is written as Rate =
order with respect to NO and H2, respectively. Calculate the value of x and y from the
data provided.
k [NO]* [H2]v. The exponents x and y represent the
%3D
3. The decomposition of N2O5 in carbon tetrachloride has been studied:
2 N,O5 (g)
2 N,O4 (g) + O2 (g)
The concentration of N,O5 is measured every 400 seconds. The data are tabulated below.
[N2O5]
(M)
A[N¿O5]
(M)
Rate = -A[N2O5]/At
(M/s)
At
%3D
time
(s)
(s)
0.0
1.40
400.0
1.10
800.0
0.87
1200.0
0.68
a) Fill the blanks in the table. Note that the last column is the average rate of reaction.
b) Briefly explain why the rates are decreasing.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fdce7689d-4520-4a5f-90cf-3f573cfd3075%2F428f48f1-22ed-4bfe-b751-14fdaa29c744%2Fvd37qtu.jpeg&w=3840&q=75)
Transcribed Image Text:2. The reaction H2 (g) + 2 NO (g) → N,O (g) + H,O (g) is studied at a certain tempera-
ture by determining the rate of reaction at reactant concentrations. The results are as
follows.
Concentration (M)
Rate
[NO]
[H2]
(M/s)
(i)
0.25
0.10
0.126
(ii)
0.50
0.10
0.504
(iii)
0.50
0.20
1.03
The rate law is written as Rate =
order with respect to NO and H2, respectively. Calculate the value of x and y from the
data provided.
k [NO]* [H2]v. The exponents x and y represent the
%3D
3. The decomposition of N2O5 in carbon tetrachloride has been studied:
2 N,O5 (g)
2 N,O4 (g) + O2 (g)
The concentration of N,O5 is measured every 400 seconds. The data are tabulated below.
[N2O5]
(M)
A[N¿O5]
(M)
Rate = -A[N2O5]/At
(M/s)
At
%3D
time
(s)
(s)
0.0
1.40
400.0
1.10
800.0
0.87
1200.0
0.68
a) Fill the blanks in the table. Note that the last column is the average rate of reaction.
b) Briefly explain why the rates are decreasing.
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