# What molar quantity of dinitrogen gas is present in a 300*mL volume under standard conditions of temperature and pressure?

Jul 23, 2017

Volume is a state function, of number of gaseous molecules......I gets approx. $0.01 \cdot m o l$.

#### Explanation:

....and the pressure of those molecules, .......and the temperature of those molecules.........I will use $\text{STP}$ as $105 \cdot k P a$ and a temperature of $0$ ""^@C, i.e. $273.15 \cdot K$.

We use of course employ the Ideal Gas equation.........and the only difficulty is in finding the appropriate gas constant, $R$. This site lists the various gas constants, including the one I use here.

$R = 8.3144598 \left(48\right) \times {10}^{-} 2 \cdot L \cdot \text{bar} \cdot {K}^{-} 1 \cdot m o {l}^{-} 1$

n=(PV)/(RT)=(1*"bar"xx300*mLxx10^-3*L*mL^-1)/(8.31xx10^-2*(L*"bar")/(K*mol)xx273.15*K)

$= 0.0132 \cdot m o l$ of $\text{dinitrogen gas}$. What is the mass of this gas?