# What is the volume of 6.23 moles of carbon dioxide at STP?

Apr 12, 2017

Of course this depends on how your syllabus defines STP. We might be given the molar volume at $\text{STP} .$

#### Explanation:

The current definition prescribes a temperature of $273.15 \cdot K$, and a pressure of $1 \cdot \text{bar}$, $100 \cdot k P a$.

And we then use the Ideal Gas Equation to get our $\text{volume}$ .

V=(nRT)/P=(6.23*cancel(mol)xx8.314xx10^-2cancel((L*"bar")/(K^-1*mol^-1))xx273.15*cancelK)/(1*cancel"bar") $= 141 \cdot L$

Note that I chose the $R$ constant appropriately.

Alternatively, sometimes the supplementary material in an exam gives the $\text{molar volume at STP}$, whatever standard they have used.