if 11.80 g of iron reacts with 5.06 g of oxygen . Determine the empirical formula of the resulting oxide ?

To determine the empirical formula of the resulting oxide, you need to find the ratio of the number of atoms of each element in the compound.

Since we have the masses of iron (Fe) and oxygen (O), we can use these values to calculate the number of moles of each element.

Step 1: Convert the masses of iron and oxygen to moles:
- Moles of iron (Fe):
- Mass of Fe = 11.80 g
- Molar mass of Fe = 55.845 g/mol (you can find this in the periodic table)
- Moles of Fe = Mass of Fe / Molar mass of Fe

- Moles of oxygen (O):
- Mass of O = 5.06 g
- Molar mass of O = 16.00 g/mol (you can find this in the periodic table)
- Moles of O = Mass of O / Molar mass of O

Step 2: Find the mole ratio of Fe to O:
- Divide the moles of Fe and O by the smallest value you obtained in Step 1 to get a whole-number ratio.

Step 3: Write the empirical formula:
- Use the mole ratio obtained in Step 2 to write the empirical formula of the resulting oxide. The empirical formula represents the simplest whole-number ratio of atoms in the compound.

Now, let's calculate the moles of Fe and O:
- Moles of Fe = 11.80 g / 55.845 g/mol ≈ 0.2110 mol
- Moles of O = 5.06 g / 16.00 g/mol ≈ 0.3160 mol

Next, we divide the moles of Fe and O by the smallest value, which is approximately 0.2110 mol:
- Fe: 0.2110 mol / 0.2110 mol ≈ 1.000
- O: 0.3160 mol / 0.2110 mol ≈ 1.500

The mole ratio between Fe and O is approximately 1:1.5. To obtain whole numbers, we can multiply the ratio by 2:
- Fe: 1 × 2 = 2
- O: 1.5 × 2 = 3

Therefore, the empirical formula of the resulting oxide is Fe2O3.

figure the moles of each element.

divide both moles by the lower of the two.

The result, is the ratio of the elements. Convert that ratio to small whole numbers. For instance:

X 1.5 Y 1 X3Y2
X 7 Y 5.1 X7Y5
X1 Y 1.333 X3Y4