To find the molecular formula of the compound with 25.2% sulfur and a molar mass of 254, we calculate the mass of sulfur and fluorine in one mole of the compound. It contains 2 moles of sulfur and 10 moles of fluorine, giving us the molecular formula SF10.
To determine the molecular formula of the compound formed by the reaction of fluorine with sulfur, which has 25.2% sulfur by mass and a relative molecular mass of 254, we should follow a step-by-step approach.
Firstly, calculate the mass of sulfur in one mole of the compound:
254 g/mol × 0.252 (25.2%) = 64.008 g/mol of sulfur
Since the atomic mass of sulfur (S) is approximately 32.07 amu, the number of moles of sulfur in the compound is:
64.008 g / 32.07 g/mol = 2 moles of sulfur
This means the compound contains two sulfur atoms. With this information, we can subtract the mass of sulfur from the total mass to find the mass of fluorine in the compound:
254 g/mol - 64.008 g/mol = 189.992 g/mol of fluorine
Given that the atomic mass of fluorine (F) is approximately 19 amu, we can find the number of moles of fluorine:
189.992 g / 19 g/mol = 10 moles of fluorine
Therefore, the molecular formula for the compound is SF10.