# Problem: The density of a gas of unknown molar mass was measured as a function of pressure at 0 oC, as in the table below. Pressure (atm)1.000.6660.5000.3330.250 Density  (g/L) 2.30741.52631.14010.75710.5660Determine a precise molar mass for the gas. Hint: Graph d / P versus P.

###### FREE Expert Solution

We’re being asked to calculate for the molar mass of a gas using the plot of density and pressure

Recall that to calculate using density, we can use the ideal gas equation.

$\overline{){\mathbf{P}}{\mathbf{V}}{\mathbf{=}}{\mathbf{n}}{\mathbf{R}}{\mathbf{T}}}$

$\frac{\mathbf{P}\overline{)\mathbf{V}}}{\overline{)\mathbf{V}}}\mathbf{=}\frac{\mathbf{n}\mathbf{R}\mathbf{T}}{\mathbf{V}}$

$\mathbit{P}\mathbf{=}\frac{{\mathbf{n}}\mathbf{RT}}{\mathbf{V}}$

###### Problem Details
The density of a gas of unknown molar mass was measured as a function of pressure at 0 oC, as in the table below.

 Pressure (atm) 1.00 0.666 0.500 0.333 0.250 Density (g/L) 2.3074 1.5263 1.1401 0.7571 0.5660

Determine a precise molar mass for the gas. Hint: Graph d / P versus P.