a chemist discovered an ore and analyzed its composition to contain 2% iron, 5% phosphor, and 93% sodium. What is the correct formula?
To determine the correct formula of the ore, we need to analyze the composition and determine the elements present in the ore. Given that the ore contains 2% iron, 5% phosphorus, and 93% sodium, we can calculate the number of moles of each element present in 100 grams of the ore.
First, we need to determine the atomic masses of the elements. The atomic mass of iron is about 55.845 g/mol, the atomic mass of phosphorus is about 30.974 g/mol, and the atomic mass of sodium is about 22.990 g/mol.
Next, let's calculate the composition in moles:
- Iron: (2 g / 55.845 g/mol) ≈ 0.036 moles
- Phosphorus: (5 g / 30.974 g/mol) ≈ 0.161 moles
- Sodium: (93 g / 22.990 g/mol) ≈ 4.048 moles
Now, we want to determine the empirical formula of the ore, which is the simplest whole number ratio of the elements present. To do this, we divide each number of moles by the smallest number of moles (in this case, 0.036 moles of iron).
Dividing the number of moles by 0.036:
- Iron: ~0.036 moles / 0.036 moles ≈ 1
- Phosphorus: ~0.161 moles / 0.036 moles ≈ 4.5
- Sodium: ~4.048 moles / 0.036 moles ≈ 112.444
Since we need to have whole number ratios, we can round the numbers:
- Iron: 1
- Phosphorus: 5
- Sodium: 112
Now we have the empirical formula of the ore: FePO5Na112. However, this formula seems unbalanced and unlikely. It is possible that there was an error in the analysis or thought process. It would be advisable to double-check the calculations and reanalyze the composition of the ore to ensure accuracy.