Question

Sulfur burns in air to form sulfur dioxide in the following reaction s O₂ – sO₂. What mass of sO₂ forms from 64 g of sulfur?

Answer 1

The mass of sulfur dioxide (SO2) that forms from 64 g of sulfur, when burned in air, is 128.14 g. This is calculated using stoichiometry with a 1:1 mole ratio between sulfur and sulfur dioxide.

Step-by-step explanation:

The question involves calculating the mass of sulfur dioxide (SO2) that forms from burning sulfur in air. To find this, we'll have to use stoichiometry from the balanced chemical reaction. The balanced equation for the combustion of sulfur to produce sulfur dioxide is:

S(s) + O2(g) → SO2(g)

First, we need to convert the mass of sulfur (S) to moles using the molar mass of sulfur (approximately 32.07 g/mol). Then, by using the stoichiometry of the balanced equation, we'll determine the moles of sulfur dioxide formed. Since the stoichiometry shows a 1:1 mole ratio between sulfur and sulfur dioxide, the moles of sulfur burnt will equal the moles of sulfur dioxide formed. Finally, we convert the moles of SO2 back to grams using its molar mass (approximately 64.07 g/mol).

Step-by-step:

1. Convert 64 g of sulfur to moles: 64 g S * (1 mol S / 32.07 g S) = 2 moles S.
2. Using the 1:1 mole ratio, 2 moles of S produce 2 moles of SO2.
3. Convert 2 moles of SO2 back to grams: 2 moles SO2 * (64.07 g SO2 / 1 mol SO2) = 128.14 g SO2.

Therefore, the mass of SO2 that forms from 64 g of sulfur is 128.14 g.