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?

Do not enter units.

Here is a worked example. Just follow the steps.

http://www.jiskha.com/science/chemistry/stoichiometry.html

To determine the number of moles of fluorine gas (F2) needed for the reaction, we need to follow these steps:

1. Write down the balanced chemical equation for the reaction between sulfur (S8) and fluorine (F2) to form sulfur hexafluoride (SF6).

The balanced chemical equation is:
S8 + 24F2 → 8SF6

2. Calculate the molar mass of sulfur (S) and fluorine (F).

The molar mass of sulfur (S) is 32.07 g/mol (the atomic mass of sulfur). The molar mass of fluorine (F) is 18.99 g/mol (the atomic mass of fluorine).

3. Convert the given mass of sulfur into moles.

Using the formula:
moles = mass (g) / molar mass (g/mol)

moles of sulfur = 50.5 g sulfur / 32.07 g/mol = 1.576 mol sulfur

4. Use the stoichiometry of the balanced chemical equation to determine the mole ratio between sulfur and fluorine.

From the balanced chemical equation, we can see that 1 mole of sulfur reacts with 24 moles of fluorine.

5. Calculate the moles of fluorine needed.

moles of fluorine = moles of sulfur × mole ratio

moles of fluorine = 1.576 mol sulfur × 24 mol fluorine/1 mol sulfur
moles of fluorine = 37.824 mol fluorine

Therefore, 37.824 moles of fluorine gas (F2) are needed for complete reaction with 50.5 g of sulfur to form sulfur hexafluoride.