Respuesta :
Molecular formula of the compound will be [tex]Si_{2} Fe_{6}[/tex].
Molar mass of silicon fluoride ,
P=1.Satm = 1.5 x 101000 = 151500Pa
V=0.25L=0.25x103[tex]m^{3}[/tex]
T= 27 +273 = 300K
Now, use ideal gas equation.
PV=nRT
Where, P is pressure, n is number of ,moles and T is temperature.
Now, put the value the given data in above equation.
151500x0.25x103=nx8.31x300
n=0.015mol .
Molar mass can be determined by using the formula:
Molar mass = mass/moles
Molar mass = 2.60.015 = 171g/mol
The relation between empirical formula and molecular formula can be written as:
Molecular formula = n ×Empirical formula
Moles of Si= mass of Si / molar mass of Si
=33.01/28
= 1.17mol
Moles of F= 67/19 = 3.52mol
Simple ratio Si= 1.17/1.17=1
Simple ratio F = 3.52/1.17=3
Emp formula =[tex]SiF_{3}[/tex]
Emp formula mass = 28 + (19 x3)= 85
Molecular formula = molecular mass/emp formula mass x emp formula
Molecular formula of the compound = 171/85 x [tex]SiF_{3}[/tex]=[tex]Si_{2} Fe_{6}[/tex]
To know more about gaseous compounds here
brainly.com/question/15710581
#SPJ4
