**Ideal Gas Law:**

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

$\mathbf{moles}\mathbf{}\mathbf{\text{(n)}}\mathbf{=}\frac{\mathbf{mass}\mathbf{}\mathbf{\left(}\mathbf{m}\mathbf{\right)}}{\mathbf{molar}\mathbf{}\mathbf{mass}\mathbf{}\mathbf{\left(}\mathbf{M}\mathbf{\right)}}$

$\mathbf{PV}\mathbf{=}\frac{\mathbf{mRT}}{\mathbf{M}}\phantom{\rule{0ex}{0ex}}\frac{\overline{)\mathbf{P}}\mathbf{V}}{\overline{)\mathbf{P}}}\mathbf{=}\frac{\mathbf{mRT}}{\mathbf{MP}}\phantom{\rule{0ex}{0ex}}\overline{)\mathbf{V}\mathbf{=}\frac{\mathbf{mRT}}{\mathbf{MP}}}$

**Calculate the volume of the balloon:**

molar mass carbon dioxide (CO_{2}) = 44.01 g/mol

T = 23°C + 273.15 = 296.15 K

A piece of dry ice (solid carbon dioxide) with a mass of 28.5 g sublimes (converts from solid to gas) into a large balloon.

Assuming that all of the carbon dioxide ends up in the balloon, what is the volume of the balloon at 23 ^{o}C and a pressure of 746 mmHg ?

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