# Question efd49

May 11, 2017

See below

#### Explanation:

At STP, we know the following:

Temperature = $\text{273.15 K}$ (0^@ "C")#
Pressure = $1$ $\text{atm}$

Plugging this into the ideal gas law yields:

$P V = n R T$

$\implies \left(\text{1 atm")V = n("0.0821 L"cdot"atm/mol"cdot"K")("273.15 K}\right)$

$\implies V = \text{22.414 L/mol} \cdot \left(n\right)$

Note that all units except $L$ will cancel out, due to the dimensions of the $R$ value

Therefore, for 1 mol of gas:

$V = \text{22.414 L}$

There you have it.

Hope that helps :)