What Is the Pressure of Methyl Cyanide After 520 Seconds?

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SUMMARY

The discussion centers on the isomerization of methyl isocyanide (CH3NC) to methyl cyanide (CH3CN) in a first-order reaction at 500K, with a rate constant of 7.70x10^-4 s^-1. The initial pressure of methyl isocyanide is 25.0 torr in a 23.2L container. After 520 seconds, the calculated pressure of methyl cyanide is incorrectly determined as 16.75 torr, while the correct value is 8.25 torr. The error arises from a misunderstanding of the reaction dynamics and the application of the first-order kinetics equation.

PREREQUISITES
  • Understanding of first-order reaction kinetics
  • Familiarity with the natural logarithm function
  • Knowledge of gas laws and pressure calculations
  • Ability to manipulate and solve equations involving rates and concentrations
NEXT STEPS
  • Review first-order reaction kinetics and the integrated rate law
  • Study the derivation and application of the equation ln(P)t/(P)0 = -kt
  • Explore the concepts of isomerization in organic chemistry
  • Practice problems involving gas phase reactions and pressure changes over time
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Chemistry students, particularly those studying reaction kinetics, organic chemistry enthusiasts, and educators looking to clarify concepts related to gas phase reactions.

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Homework Statement


In the gas phase methyl isocyanide (CH3NC) isomerizes to methyl cyanide (CH3CN) in a first order reaction with a rate constant of 7.70x10^-4s^-1 at 500K. An experiment is performed, where 25.0 torr of methyl isocyanide is placed in 23.2L container at 500K.

After 520 seconds, what is the pressure of methyl cyanide?


Homework Equations


ln (P)t/(P)0 = -kt


The Attempt at a Solution


I used the equation above to solve for (P)t, and I got 16.75, but the answer in my book is 8.25 torr, what am I doing wrong here? Please help...
 
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