What is the molecular mass of a gas if 0.0866g sample in 60ml bulb has a pressure of 400mm at 20°c
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Answer:
Whenever you see molar masses in gas law questions, more often than not density will be involved. This question is no different. To solve this, however, we will first need to play with the combined ideal gas equation
P
V
=
n
R
T
to make it work for density and molar mass. The derivation is simple but for the sake of time and space, I will skip it. Hence, just take my word for it that you will end up with the equation:
M
=
d
R
T
P
M = molar mass (g/mol)
d = density (g/L)
R = Ideal Gas Constant (
≈
0.0821
a
t
m
⋅
L
m
o
l
⋅
K
)
T = Temperature (In Kelvin)
P = Pressure (atm)
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