Final answer:
To find the molecular formula of the compound, determine the empirical formula first. The empirical formula represents the simplest whole number ratio of the atoms in a compound. In this case, the compound contains 30% nitrogen and 70% sulfur. The empirical formula of the compound is N100S102, and the molecular formula is N700S714.
Step-by-step explanation:
To find the molecular formula of the compound, we need to determine the empirical formula first. The empirical formula represents the simplest whole number ratio of the atoms in a compound. In this case, the compound contains 30% nitrogen and 70% sulfur. We can assume 100 g of the compound to make calculations easier. So, we have 30 g of nitrogen and 70 g of sulfur.
To find the empirical formula, we need to convert the masses to moles. The molar mass of nitrogen is approximately 14 g/mol, so we have 30 g / 14 g/mol = 2.14 mol of nitrogen.
The molar mass of sulfur is approximately 32 g/mol, so we have 70 g / 32 g/mol = 2.19 mol of sulfur.
Next, we need to find the lowest whole number ratio between nitrogen and sulfur. Dividing both moles by the smaller value (2.14 mol in this case), we get approximately 1 mol of nitrogen and 1.02 mol of sulfur.
To get whole numbers, we can multiply both by 100, which gives us approximately 100 mol of nitrogen and 102 mol of sulfur. Therefore, the empirical formula of the compound is N100S102.
To find the molecular formula, we need to know the molar mass of the compound.
The molar mass is given as 92 g/mol. Dividing the molar mass by the empirical formula mass (14 g/mol for nitrogen and 32 g/mol for sulfur), we get approximately 6.57. We round this value to the nearest whole number, which gives us 7. So, the molecular formula of the compound is N700S714.