Problem: Elemental sulfur occurs as octatomic molecules, S8. What mass (g) of fluorine gas is needed to react completely with 17.8 g of sulfur to form sulfur hexafluoride?

🤓 Based on our data, we think this question is relevant for Professor Bush's class at PVAMU.

FREE Expert Solution

The reaction is:

24 F2 + S8 → 8 SF6



We’re given the following:

Moles of S8 = 17.8 g

Mole-to-mole comparison = 1 mole of S8 reacts with 24 moles of F2

Molar Mass of F2 = 38.00 g/mol F2

Molar Mass of S8 = 256.56 g/mol S8

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Problem Details

Elemental sulfur occurs as octatomic molecules, S8. What mass (g) of fluorine gas is needed to react completely with 17.8 g of sulfur to form sulfur hexafluoride?

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What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Stoichiometry concept. You can view video lessons to learn Stoichiometry. Or if you need more Stoichiometry practice, you can also practice Stoichiometry practice problems.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Bush's class at PVAMU.

What textbook is this problem found in?

Our data indicates that this problem or a close variation was asked in Chemistry: The Molecular Nature of Matter and Change - Silberberg 8th Edition. You can also practice Chemistry: The Molecular Nature of Matter and Change - Silberberg 8th Edition practice problems.