# What is the volume of "0.220 mols" of carbon monoxide gas found at STP?

Jun 3, 2016

If we assume that carbon monoxide ($\text{CO}$) is an ideal gas, then we can use the ideal gas law:

$\setminus m a t h b f \left(P V = n R T\right)$

where:

• $P$ is the pressure of the gas. We can use $\text{bars}$ as our units.
• $V$ is the volume of the gas in $\text{L}$.
• $n$ is the $\setminus m a t h b f \left(\text{mol}\right)$s of gas.
• $R$ is the universal gas constant, $\text{0.083145 L"cdot"bar/mol"cdot"K}$.
• $T$ is the temperature of the gas in $\text{K}$.

At STP, $T = {0}^{\circ} \text{C" = "273.15 K}$, and $P = \text{1 bar}$. So, to get the volume, just solve for $V$.

$\textcolor{b l u e}{{V}_{\text{CO}}} = \frac{n R T}{P}$

= ((0.220 cancel("mol CO"))("0.083145 L"cdotcancel("bar")"/"cancel("mol")cdotcancel("K"))(273.15 cancel("K")))/(1 cancel"bar")

$=$ $\textcolor{b l u e}{\text{5.00 L}}$ to 3 sig figs.