Final answer:
The empirical formula of Vitamin C can be found by converting the masses of CO₂ and H₂O from combustion into moles, finding the molar ratios, and using these to derive the simplest whole-number ratio of elements. The actual empirical formula of Vitamin C is C3H4O3.
Step-by-step explanation:
The empirical formula of a compound gives the simplest whole-number ratio of the elements within it. To determine the empirical formula of Vitamin C from the given data, we first need to convert the masses of CO₂ and H₂O produced upon combustion into moles. These moles will then be used to find the molar ratio of carbon and hydrogen in Vitamin C. Oxygen's contribution can be calculated by difference because Vitamin C contains only carbon, hydrogen, and oxygen. Here's how you do it:
- Determine moles of carbon by dividing the mass of CO₂ by its molar mass (44.01 g/mol) since each CO₂ molecule contains one carbon atom.
- Determine moles of hydrogen by dividing the mass of H₂O by its molar mass (18.02 g/mol) and then multiplying by 2, since each H₂O molecule contains two hydrogen atoms.
- The mass of oxygen in Vitamin C can be found by subtracting the mass of carbon and hydrogen (as their components in CO₂ and H₂O) from the total mass of Vitamin C combusted.
- Divide the moles of each element by the smallest number of moles to get the simplest whole-number ratio.
By applying the above steps to the given masses, we can calculate the empirical formula. Please note that, in reality, the empirical formula of Vitamin C, or ascorbic acid, is actually C3H4O3 based on its composition percentages and experimentally determined molecular mass (176 amu).
To provide a full understanding, it might be helpful for you to perform these calculations step by step as practice, using the combustion data provided above; this exercise will reinforce your understanding of stoichiometry and empirical formulas.