# Question b9b46

Sep 27, 2016

$\text{9.69 mL}$

#### Explanation:

The problem provides you with the density of the helium sample, which essentially means that it is providing you with the mass of one unit of volume of helium at a certain temperature.

A density of $\text{0.17847 g/L}$ means that at a specific temperature, $\text{1 L}$ of helium has a mass of $\text{0.17847 g}$.

In your case, the sample is said to have a mass of $1.73 \cdot {10}^{- 3} \text{g}$. Use the given density to find the volume of the sample in liters

1.73 * 10^(-3)color(red)(cancel(color(black)("g"))) * "1 L"/(0.17847 color(red)(cancel(color(black)("g")))) = 9.694 * 10^(-3)"L"

Now all you have to do is convert the volume from liters to milliliters

9.694 * color(blue)(cancel(color(black)(10^(-3)))) color(red)(cancel(color(black)("L")))* (color(blue)(cancel(color(black)(10^(3))))"mL")/(1color(red)(cancel(color(black)("L")))) = color(green)(bar(ul(|color(white)(a/a)color(black)("9.69 mL")color(white)(a/a)|)))#

The answer is rounded to three sig figs, the number of sig figs you have for the mass of the sample.