Answer:
15.95 g
Explanation:
Calculation of the moles of sulfur as:-
Mass = 3.5 g
Molar mass of sulfur = 32.065 g/mol
The formula for the calculation of moles is shown below:
[tex]moles = \frac{Mass\ taken}{Molar\ mass}[/tex]
Thus,
[tex]Moles= \frac{3.5\ g}{32.065\ g/mol}[/tex]
[tex]Moles= 0.1092\ mol[/tex]
From the reaction,
[tex]S+3F_2\rightarrow SF_6[/tex]
1 mole of sulfur on reaction forms 1 mole of sulfur hexafluoride
0.1092 mole of sulfur on reaction forms 0.1092 mole of sulfur hexafluoride
Molar mass of sulfur hexafluoride = 146.06 g/mol
Mass= Moles*Molar mass = 0.1092*146.06 g = 15.95 g
15.95 g is the maximum amount of [tex]SF_6[/tex] that can be produced from the reaction of 3.5 g of sulfur with of fluorine.
