From the combination of boyel's Charle's and Avogadro's law show that PM=dRTwhere P=pressure of gas M equals to molecular mass of gas equals to density of gas equals to temperature are equals to molar gas constant?
1 Answer
Boyle's law was
From this we find:
V prop T V prop n
Thus,
PV = nRT
is the ideal gas law, where:
P is the pressure in"atm" ifR = "0.082057 L"cdot"atm/mol"cdot"K" .V is the volume in"L" .n is the mols of ideal gas.T is the temperature in"K" .
Now, the units of molar mass are
overbrace("g"/cancel"mol")^(M) xx (overbrace(cancel("mol"))^(n))/underbrace("L")_(V) = overbrace("g"/"L")^(d)
and it follows that
As a result, by multiplying by molar mass on both sides,
PVM = nMRT
=> color(blue)(PM) = (nMRT)/V = color(blue)(dRT)
So if a gas has a density of
M = (dRT)/P
= ("0.08988 g/"cancel"L" cdot 0.082057 cancel"L"cdotcancel"atm""/mol"cdotcancel"K" cdot 273.15 cancel"K")/cancel"1 atm"
= "2.0145 g/mol"
Given that this gas is a homonuclear diatomic molecule, what is it?