relating the half-life of a second- order reaction to the rate constant. How does it differ from the equation for a first-order reaction? 13.24 For a first-order reaction, how long will it take for the concentration of reactant to fall to one-eighth its original value? Express your answer in terms of the half-life (t) and in terms of the rate constant k. 1. Problems 13.25 ) What is the half-life of a compound if 75 percent of a given sample of the compound decomposes in 60min? Assume first-order kinetics. 13 13 13.26 The thermal decomposition of phosphine (PH3) into 13 phosphorus and molecular hydrogen is a first-order reaction: 4PH3(g) → P4(g) + 6H2(g) 13 The half-life of the reaction is 35.0 s at 680°C. Cal- culate (a) the first-order rate constant for the reac- tion and (b) the time required for 95 percent of the phosphine to decompose. 13 13.27/ The rate constant for the second-order reaction 2NOBr(g) 2NO(g) + Br2(g) -> is 0.80/M s at 10°C. (a) Starting with a concentra- tion of 0.086 M, calculate the concentration of NOBr after 22 s. (b) Calculate the half-lives when [NOBR]o =0.072 M and [NOBR]o = 0.054 M. 13 %3D %3D 13.28 The rate constant for the second-order reaction Pr 2NO2(g) 2NO(g) + O2(8) is 0 54/AA
relating the half-life of a second- order reaction to the rate constant. How does it differ from the equation for a first-order reaction? 13.24 For a first-order reaction, how long will it take for the concentration of reactant to fall to one-eighth its original value? Express your answer in terms of the half-life (t) and in terms of the rate constant k. 1. Problems 13.25 ) What is the half-life of a compound if 75 percent of a given sample of the compound decomposes in 60min? Assume first-order kinetics. 13 13 13.26 The thermal decomposition of phosphine (PH3) into 13 phosphorus and molecular hydrogen is a first-order reaction: 4PH3(g) → P4(g) + 6H2(g) 13 The half-life of the reaction is 35.0 s at 680°C. Cal- culate (a) the first-order rate constant for the reac- tion and (b) the time required for 95 percent of the phosphine to decompose. 13 13.27/ The rate constant for the second-order reaction 2NOBr(g) 2NO(g) + Br2(g) -> is 0.80/M s at 10°C. (a) Starting with a concentra- tion of 0.086 M, calculate the concentration of NOBr after 22 s. (b) Calculate the half-lives when [NOBR]o =0.072 M and [NOBR]o = 0.054 M. 13 %3D %3D 13.28 The rate constant for the second-order reaction Pr 2NO2(g) 2NO(g) + O2(8) is 0 54/AA
Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
Related questions
Question
13.25
![relating the half-life of a second-
order reaction to the rate constant. How does it differ
from the equation for a first-order reaction?
13.24 For a first-order reaction, how long will it take for
the concentration of reactant to fall to one-eighth its
original value? Express your answer in terms of the
half-life (t) and in terms of the rate constant k.
1.
Problems
13.25 ) What is the half-life of a compound if 75 percent of
a given sample of the compound decomposes in
60min? Assume first-order kinetics.
13
13
13.26 The thermal decomposition of phosphine (PH3) into
13
phosphorus and molecular hydrogen is a first-order
reaction:
4PH3(g) → P4(g) + 6H2(g)
13
The half-life of the reaction is 35.0 s at 680°C. Cal-
culate (a) the first-order rate constant for the reac-
tion and (b) the time required for 95 percent of the
phosphine to decompose.
13
13.27/ The rate constant for the second-order reaction
2NOBr(g) 2NO(g) + Br2(g)
->
is 0.80/M s at 10°C. (a) Starting with a concentra-
tion of 0.086 M, calculate the concentration of
NOBr after 22 s. (b) Calculate the half-lives when
[NOBR]o =0.072 M and [NOBR]o = 0.054 M.
13
%3D
%3D
13.28 The rate constant for the second-order reaction
Pr
2NO2(g) 2NO(g) + O2(8)
is 0 54/AA](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fdce7689d-4520-4a5f-90cf-3f573cfd3075%2F7f6ac66f-e38b-441f-ab48-d21474966eb9%2Fv2zfgj.jpeg&w=3840&q=75)
Transcribed Image Text:relating the half-life of a second-
order reaction to the rate constant. How does it differ
from the equation for a first-order reaction?
13.24 For a first-order reaction, how long will it take for
the concentration of reactant to fall to one-eighth its
original value? Express your answer in terms of the
half-life (t) and in terms of the rate constant k.
1.
Problems
13.25 ) What is the half-life of a compound if 75 percent of
a given sample of the compound decomposes in
60min? Assume first-order kinetics.
13
13
13.26 The thermal decomposition of phosphine (PH3) into
13
phosphorus and molecular hydrogen is a first-order
reaction:
4PH3(g) → P4(g) + 6H2(g)
13
The half-life of the reaction is 35.0 s at 680°C. Cal-
culate (a) the first-order rate constant for the reac-
tion and (b) the time required for 95 percent of the
phosphine to decompose.
13
13.27/ The rate constant for the second-order reaction
2NOBr(g) 2NO(g) + Br2(g)
->
is 0.80/M s at 10°C. (a) Starting with a concentra-
tion of 0.086 M, calculate the concentration of
NOBr after 22 s. (b) Calculate the half-lives when
[NOBR]o =0.072 M and [NOBR]o = 0.054 M.
13
%3D
%3D
13.28 The rate constant for the second-order reaction
Pr
2NO2(g) 2NO(g) + O2(8)
is 0 54/AA
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