We are asked to calculate the density of laughing gas, dinitrogen monoxide, N_{2}O, at a temperature of 325 K and a pressure of 113.0 kPa.

Use the modified ideal gas law to solve for density:

$\overline{){\mathbf{d}}{\mathbf{=}}\frac{\mathbf{PM}}{\mathbf{RT}}}$

**We can now calculate the ****density :**

$\mathbf{P}\mathbf{}\mathbf{=}\mathbf{}\mathbf{}\mathbf{113}\mathbf{.}\mathbf{0}\mathbf{}\overline{)\mathbf{kPa}\mathbf{}}\mathbf{\times}\frac{\mathbf{1}\mathbf{}\mathbf{atm}}{\mathbf{101}\mathbf{.}\mathbf{325}\mathbf{}\mathbf{}\overline{)\mathbf{kPa}\mathbf{}}}\mathbf{}\mathbf{=}\mathbf{}\mathbf{1}\mathbf{.}\mathbf{115}\mathbf{}\mathbf{atm}$**R** = universal gas constant = 0.08206 (L∙atm)/(mol∙K)**T **= 325 K**M** = 44.02 g/mol

What is the density of laughing gas, dinitrogen monoxide, N_{2}O, at a temperature of 325 K and a pressure of 113.0 kPa?

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

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Based on our data, we think this problem is relevant for Professor Clymer's class at Capital University.

What textbook is this problem found in?

Our data indicates that this problem or a close variation was asked in Chemistry - OpenStax 2015th Edition. You can also practice Chemistry - OpenStax 2015th Edition practice problems.