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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

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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
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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
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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