# What is the volume, in liters, of 5.0 mol of Ne gas at STP?

##### 1 Answer
Mar 24, 2018

${V}_{N e}$ $=$ $22.41$ $L$

#### Explanation:

$\text{We use the ideal gas law,}$

$\textcolor{\mathmr{and} a n \ge}{P V = n R T}$

$\text{We know the conditions for STP are the following,}$

$P = 101.325$ $k P a$

V=?

$n = 1.0$ $m o l$

$R = 8.314$

$T = 273.15$ $K$

Plug in your values.

color(orange)(V_(Ne)=(nRT)/(P)

$= \frac{\left(1.0 m o l\right) \left(8.314\right) \left(273.15\right)}{101.325}$

$= \frac{\left(1.0 m o l\right) \left(8.314\right) \left(273.15\right)}{101.325}$

$= \frac{2270.9691}{101.325}$

${V}_{N e}$ $=$ $22.41$ $L$

$\text{This is true because the volume of an ideal gas is 22.41 L/mol at STP.}$