Problem: At 25°C the decomposition of N2O5 (g) into NO2 (g) and O2(g) follows first-order kinetics with k = 3.4 10-5 s-1. How long will it take for a sample originally containing 2.0 atm of N2O5 to reach a partial pressure of 380 torr?

FREE Expert Solution

The integrated rate law for a first-order reaction is as follows:


ln[A]t = -kt + ln[A]o


where: 

[A]t = concentration at time t

k = rate constant

t = time

[A]0 = initial concentration


The moles are proportional to pressure so we can use the pressure in the equation. 


93% (451 ratings)
View Complete Written Solution
Problem Details

At 25°C the decomposition of N2O5 (g) into NO2 (g) and O2(g) follows first-order kinetics with k = 3.4 10-5 s-1. How long will it take for a sample originally containing 2.0 atm of N2O5 to reach a partial pressure of 380 torr?

Frequently Asked Questions

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Integrated Rate Law concept. You can view video lessons to learn Integrated Rate Law. Or if you need more Integrated Rate Law practice, you can also practice Integrated Rate Law practice problems.