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 balf-life (t) and in terms of the rate constant k. 13.4 Activ Depe Review Qu 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. 13.31 Det ene 13.32 Wr 13.26 The thermal decomposition of phosphine (PH3) into 13.33 Us phosphorus and molecular hydrogen is a first-order reaction: CO act ter 4PH3(g) P4(8) + 6H2(8) 13.34 TH 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. ga ch 13.35 S 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. 13.36 %3D %3D a 13.28 The rate constant for the second-order reaction Problem 2NO,(g) 2NO(g) + O2(g) 13.37 ( is 0.54/M s at 300°C. How long (in seconds) would it take for the concentration of NO, to decrease from 0.62 M to 0.28 M? 1. CO re 13.29 Consider the first-order reaction A B shown ag tic here. (a) What is the rate constant of the reaction? (b) How many A (yellow) and B (blue) molecules are prese co ent at
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 balf-life (t) and in terms of the rate constant k. 13.4 Activ Depe Review Qu 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. 13.31 Det ene 13.32 Wr 13.26 The thermal decomposition of phosphine (PH3) into 13.33 Us phosphorus and molecular hydrogen is a first-order reaction: CO act ter 4PH3(g) P4(8) + 6H2(8) 13.34 TH 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. ga ch 13.35 S 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. 13.36 %3D %3D a 13.28 The rate constant for the second-order reaction Problem 2NO,(g) 2NO(g) + O2(g) 13.37 ( is 0.54/M s at 300°C. How long (in seconds) would it take for the concentration of NO, to decrease from 0.62 M to 0.28 M? 1. CO re 13.29 Consider the first-order reaction A B shown ag tic here. (a) What is the rate constant of the reaction? (b) How many A (yellow) and B (blue) molecules are prese co ent at
Chemistry by OpenStax (2015-05-04)
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ISBN:9781938168390
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Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Chapter12: Kinetics
Section: Chapter Questions
Problem 50E: For the past 10 years, the unsaturated hydrocarbon 1, 3-butadiene (CH2 = CH - CH = CH2) has ranked...
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Question
13.26
![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
balf-life (t) and in terms of the rate constant k.
13.4 Activ
Depe
Review Qu
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.
13.31 Det
ene
13.32 Wr
13.26 The thermal decomposition of phosphine (PH3) into
13.33 Us
phosphorus and molecular hydrogen is a first-order
reaction:
CO
act
ter
4PH3(g) P4(8) + 6H2(8)
13.34 TH
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.
ga
ch
13.35 S
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.
13.36
%3D
%3D
a
13.28 The rate constant for the second-order reaction
Problem
2NO,(g) 2NO(g) + O2(g)
13.37 (
is 0.54/M s at 300°C. How long (in seconds) would
it take for the concentration of NO, to decrease from
0.62 M to 0.28 M?
1.
CO
re
13.29 Consider the first-order reaction A B shown
ag
tic
here. (a) What is the rate constant of the reaction?
(b) How many A (yellow) and B (blue) molecules
are prese
co
ent at](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fdce7689d-4520-4a5f-90cf-3f573cfd3075%2F6a0fd313-1e3c-4a8f-9bef-9a3b6e880f83%2Fh4wygu6.jpeg&w=3840&q=75)
Transcribed Image Text: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
balf-life (t) and in terms of the rate constant k.
13.4 Activ
Depe
Review Qu
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.
13.31 Det
ene
13.32 Wr
13.26 The thermal decomposition of phosphine (PH3) into
13.33 Us
phosphorus and molecular hydrogen is a first-order
reaction:
CO
act
ter
4PH3(g) P4(8) + 6H2(8)
13.34 TH
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.
ga
ch
13.35 S
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.
13.36
%3D
%3D
a
13.28 The rate constant for the second-order reaction
Problem
2NO,(g) 2NO(g) + O2(g)
13.37 (
is 0.54/M s at 300°C. How long (in seconds) would
it take for the concentration of NO, to decrease from
0.62 M to 0.28 M?
1.
CO
re
13.29 Consider the first-order reaction A B shown
ag
tic
here. (a) What is the rate constant of the reaction?
(b) How many A (yellow) and B (blue) molecules
are prese
co
ent at
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