Problem: Dinitrogen pentoxide decomposes in the gas phase to form nitrogen dioxide and oxygen gas. The reaction is first order in dinitrogen pentoxide and has a half-life of 2.81 h at 25oC. If a 1.6-L reaction vessel initially contains 750 torr of N2O5 at 25 oC, what partial pressure of O2 will be present in the vessel after 220 minutes?

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FREE Expert Solution

We’re being asked to calculate partial pressure of O2 will be present in the vessel after 220 minutes.

The given equation is: N2O5(g) → NO2(g) + O2(g)

Balancing the equation is: N2O5(g) → 4 NO2(g) + O2(g)


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


ln [A]t=-kt+ln [A]0

where:

[A]t = concentration at time, t
k = decay constant
t = time
[A]0 = initial concentration


Also, recall that half-life is the time needed for the amount of a reactant to decrease by 50% or one-half

The half-life of a first-order reaction is given by:

t12=ln 2k


We first need to calculate for the decay constant using the given half-life, 2.81 hr:

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Problem Details

Dinitrogen pentoxide decomposes in the gas phase to form nitrogen dioxide and oxygen gas. The reaction is first order in dinitrogen pentoxide and has a half-life of 2.81 h at 25oC. If a 1.6-L reaction vessel initially contains 750 torr of N2O5 at 25 oC, what partial pressure of O2 will be present in the vessel after 220 minutes?

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