Donna was studying the following reaction for a stoichiometry project: s(s) + 3 f2(g) → sf6(s) she wondered how much she could obtain if she used 3.5 g of fluorine. what mass of sf6(s) would she obtain from the calculation using this amount of fluorine?

             4.48 g of SF₆

Solution:

The reaction is as follow,

                                           S  +  3 F₂     →     SF₆

According to equation,

           113.94 g (3 mole) F₂ produced  =  146.06 g (1 mole) SF₆
So,
                           3.5 g F₂ will produce  =  X g of SF₆

Solving for X,
                      X  =  (3.5 g × 146.06 g) ÷ 113.94 g

                      X  =  4.48 g of SF₆