A 0.02847 g sample of gas occupies 10.0-mL at 292.0 K and 1.10 atm. Upon further analysis, the compound is found to be 38.734% C and 61.266% F.
What is the molecular formula of the compound?
__________________?
To determine the molecular formula of the compound, we first need to calculate the number of moles of carbon (C) and fluorine (F) in the given sample of gas.
1. Calculate the moles of carbon (C):
- Convert the mass of carbon to moles using the molar mass of carbon (12.01 g/mol):
moles of C = (mass of C / molar mass of C)
= (38.734% / 100) x (0.02847 g / 12.01 g/mol)
2. Calculate the moles of fluorine (F):
- Convert the mass of fluorine to moles using the molar mass of fluorine (19.00 g/mol):
moles of F = (mass of F / molar mass of F)
= (61.266% / 100) x (0.02847 g / 19.00 g/mol)
3. Determine the ratio of moles of C to moles of F:
- Divide the moles of C by the smallest number of moles (either C or F) to get a whole number ratio. Round to the nearest whole number to obtain the subscripts for the molecular formula.
Ratio = (moles of C / smallest number of moles)
Ratio ≈ (moles of C / moles of F)
4. Write the molecular formula:
- Use the determined ratio to write the molecular formula, including the subscripts for the atoms.
Let's calculate the moles of carbon (C) and fluorine (F) to continue with the steps.