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**Problem**: A chemist vaporized a liquid compound to determine its molar mass. If the density of the vaporized liquid (collected in a 120 mL flask) at 97°C is 3.24 g/L, and the pressure exerted by the vaporized liquid is 0.958 atm, what is its molar mass?(a) 103 g/mol (b) 121 g/mol (c) 187 g/mol (d) 31.6 g/mol(e) Insufficient information was given to calculate molar mass.

###### FREE Expert Solution

We’re being asked to calculate for the molar mass at 97°C and 0.958 atm.

To calculate for the molar mass, we’re going to use the **ideal gas equation**.

$\overline{){\mathbf{P}}{\mathbf{V}}{\mathbf{=}}{\mathbf{n}}{\mathbf{R}}{\mathbf{T}}}\phantom{\rule{0ex}{0ex}}\frac{\mathbf{P}\overline{)\mathbf{V}}}{\overline{)\mathbf{V}}}\mathbf{=}\frac{\mathbf{n}\mathbf{R}\mathbf{T}}{\mathbf{V}}\phantom{\rule{0ex}{0ex}}\mathit{P}\mathbf{=}\frac{{\mathbf{n}}\mathbf{R}\mathbf{T}}{\mathbf{V}}$

${\mathit{n}}{\mathbf{=}}\frac{\mathbf{m}\mathbf{a}\mathbf{s}\mathbf{s}\mathbf{}\left(\mathbf{m}\right)}{\mathbf{m}\mathbf{o}\mathbf{l}\mathbf{a}\mathbf{r}\mathbf{}\mathbf{m}\mathbf{a}\mathbf{s}\mathbf{s}\mathbf{}\left(\mathbf{M}\right)}$

###### Problem Details

A chemist vaporized a liquid compound to determine its molar mass. If the density of the vaporized liquid (collected in a 120 mL flask) at 97°C is 3.24 g/L, and the pressure exerted by the vaporized liquid is 0.958 atm, what is its molar mass?

(a) 103 g/mol

(b) 121 g/mol

(c) 187 g/mol

(d) 31.6 g/mol

(e) Insufficient information was given to calculate molar mass.

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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 .