Reaction:

**N _{2}O_{3}(g) → NO_{2}(g) + NO(g)**

P_{1} = 0.018 atm

initial temperature = T_{1}

final temperature = 2 T_{1}

initial amount = 1 mole of gas

final amount = 2 moles of gas

**Ideal Gas Law:**

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

**Isolate pressure:**

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

A sample of N_{2}O_{3}(g) has a pressure of 0.018 atm . The temperature (in K) is then doubled and the N_{2}O_{3} undergoes complete decomposition to NO_{2}(g) and NO(g).

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

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 The Ideal Gas Law concept. You can view video lessons to learn The Ideal Gas Law. Or if you need more The Ideal Gas Law practice, you can also practice The Ideal Gas Law practice problems.