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Problems oe.o of the of the rate constant k. 13.4 Activation Dependen Review Question 13.25 ) What is the half-life of a compound if 75 percent of a given sample of the compound decomposes in 60 min? Assume first-order kinetics. 13.26 ) The thermal decomposition of phosphine (PH3) into 13.31 Define ac energy pl 13.32 Write the phosphorus and molecular hydrogen is a first-order reaction: 13.33 Use the constant activation 4PH3(g) → P4(g) + 6H2(g) temperat 13.34 The burni 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. mic react gas can change. 13.35 Sketch a 13.27 / The rate constant for the second-order reaction plot for (a) S(s) 2NOBR(g) 2NO(g) + Br2(g) (b) Cl is 0.80/M s at 10°C. (a) Starting with a concentra- tion of 0.086 M, calcuiate the concentration of NOBR after 22 s. (B) Calculate the half-lives when [NOBr]o = 0.072 M and [NOBro= 0.054 M. 13.36 The rea for man 0 action p 13.28 The rate constant for the second-order reaction Problems 2NO2(8) 2NO(g) + O2(g) is 0.54/M s at 300°C. How long (in seconds) would it take for the concentration of NO, to decrease from 13.37 (1) The 1/T for constar 0.62 M to 0.28 M? reaction 13.29 Consider the first-order reaction A B shown here. (a) What is the rate constant of the reaction? (b) How many A (yellow) and B (blue) molecules agram tion at corresp are present at t= 20 s and 30 s? Jom t = 10 s t 0 s un hore follows first-order In k

Problems oe.o of the of the rate constant k. 13.4 Activation Dependen Review Question 13.25 ) What is the half-life of a compound if 75 percent of a given sample of the compound decomposes in 60 min? Assume first-order kinetics. 13.26 ) The thermal decomposition of phosphine (PH3) into 13.31 Define ac energy pl 13.32 Write the phosphorus and molecular hydrogen is a first-order reaction: 13.33 Use the constant activation 4PH3(g) → P4(g) + 6H2(g) temperat 13.34 The burni 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. mic react gas can change. 13.35 Sketch a 13.27 / The rate constant for the second-order reaction plot for (a) S(s) 2NOBR(g) 2NO(g) + Br2(g) (b) Cl is 0.80/M s at 10°C. (a) Starting with a concentra- tion of 0.086 M, calcuiate the concentration of NOBR after 22 s. (B) Calculate the half-lives when [NOBr]o = 0.072 M and [NOBro= 0.054 M. 13.36 The rea for man 0 action p 13.28 The rate constant for the second-order reaction Problems 2NO2(8) 2NO(g) + O2(g) is 0.54/M s at 300°C. How long (in seconds) would it take for the concentration of NO, to decrease from 13.37 (1) The 1/T for constar 0.62 M to 0.28 M? reaction 13.29 Consider the first-order reaction A B shown here. (a) What is the rate constant of the reaction? (b) How many A (yellow) and B (blue) molecules agram tion at corresp are present at t= 20 s and 30 s? Jom t = 10 s t 0 s un hore follows first-order In k

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Problems oe.o of the of the rate constant k. 13.4 Activation Dependen Review Question 13.25 ) What is the half-life of a compound if 75 percent of a given sample of the compound decomposes in 60 min? Assume first-order kinetics. 13.26 ) The thermal decomposition of phosphine (PH3) into 13.31 Define ac energy pl 13.32 Write the phosphorus and molecular hydrogen is a first-order reaction: 13.33 Use the constant activation 4PH3(g) → P4(g) + 6H2(g) temperat 13.34 The burni 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. mic react gas can change. 13.35 Sketch a 13.27 / The rate constant for the second-order reaction plot for (a) S(s) 2NOBR(g) 2NO(g) + Br2(g) (b) Cl is 0.80/M s at 10°C. (a) Starting with a concentra- tion of 0.086 M, calcuiate the concentration of NOBR after 22 s. (B) Calculate the half-lives when [NOBr]o = 0.072 M and [NOBro= 0.054 M. 13.36 The rea for man 0 action p 13.28 The rate constant for the second-order reaction Problems 2NO2(8) 2NO(g) + O2(g) is 0.54/M s at 300°C. How long (in seconds) would it take for the concentration of NO, to decrease from 13.37 (1) The 1/T for constar 0.62 M to 0.28 M? reaction 13.29 Consider the first-order reaction A B shown here. (a) What is the rate constant of the reaction? (b) How many A (yellow) and B (blue) molecules agram tion at corresp are present at t= 20 s and 30 s? Jom t = 10 s t 0 s un hore follows first-order In k
Transcribed Image Text:Problems oe.o of the of the rate constant k. 13.4 Activation Dependen Review Question 13.25 ) What is the half-life of a compound if 75 percent of a given sample of the compound decomposes in 60 min? Assume first-order kinetics. 13.26 ) The thermal decomposition of phosphine (PH3) into 13.31 Define ac energy pl 13.32 Write the phosphorus and molecular hydrogen is a first-order reaction: 13.33 Use the constant activation 4PH3(g) → P4(g) + 6H2(g) temperat 13.34 The burni 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. mic react gas can change. 13.35 Sketch a 13.27 / The rate constant for the second-order reaction plot for (a) S(s) 2NOBR(g) 2NO(g) + Br2(g) (b) Cl is 0.80/M s at 10°C. (a) Starting with a concentra- tion of 0.086 M, calcuiate the concentration of NOBR after 22 s. (B) Calculate the half-lives when [NOBr]o = 0.072 M and [NOBro= 0.054 M. 13.36 The rea for man 0 action p 13.28 The rate constant for the second-order reaction Problems 2NO2(8) 2NO(g) + O2(g) is 0.54/M s at 300°C. How long (in seconds) would it take for the concentration of NO, to decrease from 13.37 (1) The 1/T for constar 0.62 M to 0.28 M? reaction 13.29 Consider the first-order reaction A B shown here. (a) What is the rate constant of the reaction? (b) How many A (yellow) and B (blue) molecules agram tion at corresp are present at t= 20 s and 30 s? Jom t = 10 s t 0 s un hore follows first-order In k
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