Solved: Determining the Half-Life of a First-Order

Chapter , Problem 1PE

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We noted in an earlier Practice Exercise that at \(25^{\circ} \mathrm{C}\) the decomposition of \(\mathrm{N}_{2} \mathrm{O}_{5}(\mathrm{~g})\) into \(\mathrm{NO}_{2}(\mathrm{~g}) \text { and } \mathrm{O}_{2}(\mathrm{~g})\)  follows first-order kinetics with \(k=3.4 \times 10^{-5} \mathrm{~s}^{-1}\). How long will it take for a sample originally containing \(2.0 \mathrm{~atm} \text { of } \mathrm{N}_{2} \mathrm{O}_{5}\) to reach a partial pressure of \(380 \text { torr }\)?

(a)  \(5.7 \mathrm{~h}\)

(b)  \(8.2 \mathrm{~h}\)         

(c)  \(11 \mathrm{~h}\)         

(d)  \(16 \mathrm{~h}\)         

(e)  \(32 \mathrm{~h}\)

 

Equation Transcription:

   

   

   

     

 

 

Text Transcription:

25°C

N2O5(g)  

NO2(g) and O2(g)  

k=3.4 x 10-5s-1    

2.0 atm of N2O5    

380 torr

5.7 h

8.2 h

11 h

16 h  

32 h