Final answer:
The molecular formula of the compound is Sr2O2Cl2.
Step-by-step explanation:
The molecular formula of a compound can be determined based on the given information. In this case, we have 0.500 mol of the compound that contains 0.500 mol of Sr, 1.81 x 10^24 atoms of O, and 35.5g of Cl. To determine the molecular formula, we need to compare the given amounts of each element to the molar masses of the elements.
We can start by calculating the moles of each element:
moles of Sr: 0.500 mol
moles of O: (1.81 x 10^24 atoms / 6.02 x 10^23 atoms/mol) = 3.00 mol
moles of Cl: (35.5g / 35.45 g/mol) = 1.00 mol
Based on these calculations, the empirical formula of the compound is SrOCl3. However, the molecular formula can be determined by comparing the empirical formula mass to the molar mass of the compound. If we divide the molar mass by the empirical formula mass, we get:
molar mass / empirical formula mass = (molar mass / 167.78 g/mol)
To get a value of 1, we can multiply the subscripts in the empirical formula by 2. Therefore, the molecular formula of the compound is Sr2O2Cl2.