if .500 mol of copper combines with .250 mol of sulfur what is the empirical formula of copper sulfide?

0.500 mol Cu + 0.250 mol S. Let's make those whole numbers.

4*0.500 = 2.00 Cu
4*0.250 = 1.00 S
Cu2S?

To determine the empirical formula of copper sulfide, you need to find the simplest whole number ratio between copper and sulfur atoms. To do so, follow these steps:

Step 1: Determine the moles of copper and sulfur individually.
- Moles of copper = 0.500 mol
- Moles of sulfur = 0.250 mol

Step 2: Divide the number of moles of each element by the smallest number of moles to obtain the mole ratio.
- Moles of copper / Moles of sulfur = 0.500 mol / 0.250 mol = 2 mol / 1 mol

Step 3: Simplify the mole ratio to the smallest whole number ratio.
In this case, the ratio is already simplified to 2:1.

Step 4: Determine the empirical formula using the mole ratio.
The empirical formula of copper sulfide is Cu2S.

To determine the empirical formula of copper sulfide, follow these steps:

Step 1: Determine the number of moles of copper and sulfur:
- Number of moles of copper = 0.500 mol
- Number of moles of sulfur = 0.250 mol

Step 2: Find the ratio of moles between copper and sulfur:
- Divide the number of moles of copper and sulfur by the smaller value to get the simplest whole number ratio:
0.500 mol / 0.250 mol = 2 mol of copper / 1 mol of sulfur

Step 3: Write the empirical formula:
- Convert the ratio of moles to the simplest whole number ratio, if necessary:
2 mol of copper / 1 mol of sulfur
- The empirical formula will have the subscripts of "2" for copper and "1" for sulfur:
Cu2S

Therefore, the empirical formula of copper sulfide is Cu2S.