How many grams of ethane gas (C2H6) are in a 12.7 liter sample at 1.6 atmospheres and 24C? Show all work used to solve this problem.

Question

thomaster · Answer

$\Huge\bf \color{black}{Welcome~to~OpenStudy!!}\hspace{-310pt}\color{black}{Welcome~to~OpenStudy!!}\hspace{-307.1pt}\color{#ff7100}{Welcome~to~\color{#00B4ff}{Open}}\color{#7cc517}{Study!!}$

Do you know the ideal gas law?

$\large PV=nRT$

anonymous · Answer

Not really.

thomaster · Answer

P= pressure in atm
V= volume inliter
n= moles of gas
R= gas constant (0.0820574614L  atm K−1 mol−1
T= temperature in kelvin

thomaster · Answer

You know the pressure, the volume, the gas constant and the temperature. You only need to calculate n

To do that you need to convert the fomula to 

$\Large n=\dfrac{PV}{RT}$

24°C = 297,15 Kelvin

$\Large n=\dfrac{1.6*12.7}{0.0820574614*297.15}$

Then you have the moles of ethane gas.
Use the attached diagram to convert to gram.