# A 2.00 L container holds .700 mol of oxygen gas at 285 K. What is the pressure in atm inside the container?

Jun 9, 2016

The pressure inside the container is $8.19 a t m .$

#### Explanation:

For this type of question we would use the ideal gas law equation
$P \times V = n \times R \times T$.

• P represents pressure (must have units of atm)
• V represents volume (must have units of liters)
• n represents the number of moles
• R is the proportionality constant (has a value of 0.0821 with units of $\frac{L \times a t m}{m o l \times K}$)
• T represents the temperature, which must be in Kelvins.

Now what you want to do is list your known and unknown variables. Our only unknown is the pressure of ${O}_{2}$. Our known variables are V,n,R, and T.

Now all we have to do is rearrange the equation and solve for P like so:
$P = \frac{n \times R \times T}{V}$
$P = \frac{0.700 m o l \times 0.0821 \frac{L \times a t m}{m o l \times K} \times \left(285 K\right)}{2.00 L}$
$P = 8.19 a t m$