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.

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

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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.