The molecular formula of the compound of sulfur and fluorine is .
Further Explanation:
Empirical formula:
It is atom’s simplest positive integer ratio in compound. It may or may not be the same as that of molecular formula. For example, empirical formula of disulfur dioxide is .
Molecular formula:
It is chemical formula that indicates the total number and kinds of atoms in molecule. For example, molecular formula of disulfur dioxide is
Step 1: Mass of sulfur (S) and fluorine (F) is to be calculated. This is done by using equation (1).
Since the given compound contains only sulfur and fluorine. So the mass of sulfur is calculated as follows:
......(1)
The mass of the compound is 102.13 g/mol.
The percentage of sulfur is 62.79 %.
Substitute the values in equation (1).
The mass offluorine (F) is calculated as follows:
......(2)
Substitute 102.13 g/mol for mass of the compound and 64.13 g/mol for mass of sulfur in equation (2).
Step 2: The number of sulfur (S) and fluorine (F) in the compound is to be calculated.
The formula to calculate the number of sulfur (S)atoms in the molecule is as follows:
......(3)
The given mass of S is 64.13 g/mol.
The molar mass of S is 32 g/mol.
Substitute these values in equation (3).
The formula to calculate the number of fluorine (F) atoms in the molecule is as follows:
......(4)
The given mass of F is 38 g/mol.
The molar mass of F is 19 g/mol.
Substitute these values in equation (4).
Hence the molecular formula of the given compound is .
Learn more:
1. Calculate the moles of ions in the solution: brainly.com/question/5950133
2. Calculate the moles of chlorine in 8 moles of carbon tetrachloride: brainly.com/question/3064603
Answer details:
Grade: Senior School
Subject: Chemistry
Chapter: Stoichiometry of formulas and equations
Keywords: empirical formula, S, F, SF, S2F2, subscript, moles of F, moles of S, mass of S, mass of F and molecular formula.