# Problem: A sample of N2O3(g) has a pressure of 0.018 atm . The temperature (in K) is then doubled and the N2O3 undergoes complete decomposition to NO2(g) and NO(g).Find the total pressure of the mixture of gases assuming constant volume and no additional temperature change.

###### FREE Expert Solution

Reaction:

N2O3(g) → NO2(g) + NO(g)

P1 = 0.018 atm

initial temperature = T1

final temperature = 2 T1

initial amount = 1 mole of gas

final amount = 2 moles of gas

Ideal Gas Law:

$\overline{)\mathbf{PV}\mathbf{=}\mathbf{nRT}}$

Isolate pressure:

$\overline{)\mathbf{P}\mathbf{=}\frac{\mathbf{nRT}}{\mathbf{V}}}$

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###### Problem Details

A sample of N2O3(g) has a pressure of 0.018 atm . The temperature (in K) is then doubled and the N2O3 undergoes complete decomposition to NO2(g) and NO(g).

Find the total pressure of the mixture of gases assuming constant volume and no additional temperature change.