Question

Use the balanced chemical equation below. How many grams of the product are formed when 2.34 g of sulfur is completely reacted with fluorine? S8 + 16F2(g) → 8SF4

Answer 1

Answer:

7.89 g

Explanation:

Step 1: Write the balanced equation

S₈ + 16 F₂(g) → 8 SF₄

Step 2: Calculate the moles corresponding to 2.34 g of S₈

The molar mass of S₈ is 256.52 g/mol.

$2.34g \times \frac{1mol}{256.52g} = 9.12 \times 10^{-3} mol$

Step 3: Calculate the moles of SF₄ produced from 9.12 × 10⁻³ mol of S₈

The molar ratio of S₈ to SF₄ is 1:8. The moles of SF₄ produced are 8/1 × 9.12 × 10⁻³ mol = 0.0730 mol

Step 4: Calculate the mass corresponding to 0.0730 moles of SF₄

The molar mass of SF₄ is 108.07 g/mol.

$0.0730 mol \times \frac{108.07 g}{mol} = 7.89 g$