measurements show that unknown compound x has the following composition:\nwrite the empirical chemical…

Explanation:

Step1: Assume 100g of the compound

If we assume we have 100g of compound (X), then the mass of iron ((Fe)) is (m_{Fe}=69.9g) and the mass of oxygen ((O)) is (m_{O} = 30.0g).

Step2: Calculate the number of moles of each element

The molar mass of (Fe) is (M_{Fe}=55.85g/mol), and the molar mass of (O) is (M_{O}=16.00g/mol). The number of moles of (Fe), (n_{Fe}=\frac{m_{Fe}}{M_{Fe}}=\frac{69.9g}{55.85g/mol}\approx1.25mol) The number of moles of (O), (n_{O}=\frac{m_{O}}{M_{O}}=\frac{30.0g}{16.00g/mol}=1.875mol)

Step3: Find the mole - ratio

Divide each number of moles by the smaller number of moles. Here, (n = 1.25mol) (for (Fe)) For (Fe): (\frac{n_{Fe}}{n}=\frac{1.25mol}{1.25mol}=1) For (O): (\frac{n_{O}}{n}=\frac{1.875mol}{1.25mol}=1.5) Multiply each ratio by 2 to get whole - numbers. For (Fe): (1\times2 = 2) For (O): (1.5\times2=3)

Answer:

(Fe_2O_3)