Question

xenon tetrafluoride gas is placed in a 3 liter container at 80°c. the pressure of the gas is found to be 0.117 atm. how many moles of the gas are in the container?
0.0121 mol
0.0534 mol
18.700 mol
82.517 mol

Explanation:

Step1: Convert temperature to Kelvin

$T = 80 + 273.15=353.15\ K$

Step2: Recall ideal - gas law

The ideal - gas law is $PV = nRT$, where $P$ is pressure, $V$ is volume, $n$ is the number of moles, $R$ is the ideal - gas constant ($R = 0.0821\ L\cdot atm/(mol\cdot K)$), and $T$ is temperature. We need to solve for $n$.

Step3: Rearrange the ideal - gas law for $n$

$n=\frac{PV}{RT}$

Step4: Substitute the given values

$P = 0.117\ atm$, $V = 3\ L$, $R = 0.0821\ L\cdot atm/(mol\cdot K)$, $T = 353.15\ K$
$n=\frac{0.117\ atm\times3\ L}{0.0821\ L\cdot atm/(mol\cdot K)\times353.15\ K}$
$n=\frac{0.351}{29.093615}\ mol\approx0.0121\ mol$

Answer:

0.0121 mol