How many grams of methane gas (CH4) are in a 15.8 liter sample at 1.2 atmospheres and 27°C? Show all
work used to solve this problem.
V= 15.8 liter = 0.0158 m3
P= 1.2 atm = 121590 Pa
T = 27°C = 300 K
R = 8.31 J · K-1 · mol-1
n= ? mole
PV=nRT
121590*0.0158 =n*8.31*300
n= PV/RT
n= (121590*0.0158)/ (8.31*300)
n= 0.770 moles of CH4
Mole= mass/Mr
Mass = Mr*mole
so mass = 16 x 0.770
= 12.32g