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Problem: Sulfur and fluorine react to form sulfur hexafluoride:S(s) + 3 F2(g) → SF6(g)If 50.0 g S is allowed to react as completely as possible with 105.0 g F2(g), what mass of the excess reactant is left?

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We first need to determine the moles of SF6 formed by each reactant. The reactant that forms the lower amount of product is the limiting reactant and will dictate the amount of product formed.

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Problem Details

Sulfur and fluorine react to form sulfur hexafluoride:

S(s) + 3 F2(g) → SF6(g)

If 50.0 g S is allowed to react as completely as possible with 105.0 g F2(g), what mass of the excess reactant is left?

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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 Limiting Reagent concept. If you need more Limiting Reagent practice, you can also practice Limiting Reagent practice problems.

What professor is this problem relevant for?

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