Answer: There are 6.9 mol of [tex]F_{2}[/tex] are required to react completely with 2.30 mol of S.
Explanation:
The given reaction equation is as follows.
[tex]S(s) + 3F_{2}(g) \rightarrow SF_{6}(g)[/tex]
Here, 1 mole of S is reaction with 3 moles of [tex]F_{2}[/tex] which means 1 mole of S requires 3 moles of [tex]F_{2}[/tex].
Therefore, moles of [tex]F_{2}[/tex] required to react completely with 2.30 moles S are calculated as follows.
[tex]1 mol S = 3 mol F_{2}\\2.30 mol S = 3 mol F_{2} \times 2.30 \\= 6.9 mol F_{2}[/tex]
Thus, we can conclude that there are 6.9 mol of [tex]F_{2}[/tex] are required to react completely with 2.30 mol of S.
