Elemental sulfur occurs as octatomic molecules, S8. How many moles of fluorine gas, F2, are needed for complete reaction with 50.5 g sulfur to form sulfur hexafluoride?
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To find out how many moles of fluorine gas (F2) are required to react with 50.5 g of sulfur (S), we need to use the balanced chemical equation for the reaction between sulfur and fluorine gas to form sulfur hexafluoride (SF6):
S8 + 24 F2 → 8 SF6
From the equation, we can see that it takes 24 moles of fluorine gas to react with 1 mole of sulfur (S8) to produce 8 moles of sulfur hexafluoride (SF6).
Now, let's calculate the number of moles of sulfur:
First, we need to determine the molar mass of sulfur (S). The atomic mass of sulfur (S) is approximately 32.06 g/mol.
Molar mass of sulfur (S) = 32.06 g/mol
Next, we can calculate the number of moles of sulfur using the given mass:
Number of moles of sulfur = Mass of sulfur / Molar mass of sulfur
Number of moles of sulfur = 50.5 g / 32.06 g/mol
Number of moles of sulfur = 1.574 mol
Now that we know we have 1.574 moles of sulfur, we can calculate the number of moles of fluorine gas needed using the mole ratio from the balanced equation:
Number of moles of F2 = Number of moles of S8 × (24 mol F2 / 1 mol S8)
Number of moles of F2 = 1.574 mol × (24 mol F2 / 1 mol S8)
Number of moles of F2 = 37.776 mol
Therefore, you would need 37.776 moles of fluorine gas (F2) to completely react with 50.5 g of sulfur (S) to form sulfur hexafluoride (SF6).