A sulfur-containing compound is decomposed and the products are collected over water according to this equation:

SxOy -> SO2(g) + O2(g)

The mole fractions for the products are as follows:

SO2 (.8) and O2 (.2)

What is the empirical formula for the original compound?

To find the empirical formula for the original sulfur-containing compound, we need to determine the molar ratios of the elements present in the compound.

First, let's start by calculating the mole ratios of sulfur and oxygen in the products.

From the equation provided, we can see that for every 1 mole of SO2 produced, 1 mole of sulfur atoms (S) is required.
Similarly, for every 1 mole of O2 produced, 2 moles of oxygen atoms (O) are required.

Mole ratio of Sulfur (S) to Sulfur Dioxide (SO2) = 1:1
Mole ratio of Oxygen (O) to Oxygen (O2) = 2:1

Now, let's use the mole fractions of the products to determine the mole ratios of sulfur and oxygen.

Given:
Mole fraction of SO2 = 0.8
Mole fraction of O2 = 0.2

The mole ratio of Sulfur Dioxide (SO2) can be calculated as:
Mole ratio of SO2 = (Mole fraction of SO2) / (Mole fraction of O2)
= 0.8 / 0.2
= 4

The mole ratio of Oxygen (O) can be calculated as:
Mole ratio of O = (2 * Mole ratio of SO2)
= (2 * 4)
= 8

Therefore, the empirical formula for the original sulfur-containing compound can be determined based on these mole ratios.

Empirical formula = S4O8