109% of carbon,18,2% of hydrogen and 73% of oxygen how do i calculate emperical formular?
First you need to correct the typos and make sue you have the correct numbers. They can't be right because they don't add to 100%
To calculate the empirical formula, you need to find the simplest whole number ratio between the elements in the given compound.
First, convert the percentages to grams by assuming you have 100g of the compound.
Therefore, you have:
- Carbon: 109g (109% of 100g)
- Hydrogen: 18.2g (18.2% of 100g)
- Oxygen: 73g (73% of 100g)
Next, calculate the number of moles of each element:
- Carbon: Use the atomic mass of carbon (12.01 g/mol) to calculate the number of moles:
Number of moles of carbon = Mass of carbon / Atomic mass of carbon = 109g / 12.01 g/mol
- Hydrogen: Use the atomic mass of hydrogen (1.01 g/mol):
Number of moles of hydrogen = Mass of hydrogen / Atomic mass of hydrogen = 18.2g / 1.01 g/mol
- Oxygen: Use the atomic mass of oxygen (16.00 g/mol):
Number of moles of oxygen = Mass of oxygen / Atomic mass of oxygen = 73g / 16.00 g/mol
Next, divide the number of moles of each element by the smallest number of moles calculated to obtain the simplest whole number ratio.
In this case, the number of moles of carbon is the smallest value.
Dividing the number of moles of each element by the smallest value:
Number of moles of carbon (C) = 109g / 12.01 g/mol = 9.08 mol
Number of moles of hydrogen (H) = 18.2g / 1.01 g/mol = 18.02 mol
Number of moles of oxygen (O) = 73g / 16.00 g/mol = 4.57 mol
Rounding to the nearest whole number, the empirical formula is:
C9H18O4