To determine the molecular formula of the hydrocarbon, we need to use the information provided about the masses of
CO2 and
H2O produced during combustion. Here's a step-by-step solution:
Step 1: Determine the moles of
CO2 produced.
The molar mass of
CO2 is
44g∕mol.
Therefore, the number of moles of
CO2 is:
‌=4‌moles Step 2: Determine the moles of
H2O produced.
The molar mass of
H2O is
18g∕mol.
Therefore, the number of moles of
H2O is:
‌=5‌ moles ‌ Step 3: Find the moles of carbon and hydrogen atoms in the hydrocarbon.
Each mole of
CO2 contains one mole of carbon atoms. Therefore, the number of moles of carbon is:
4 moles of C
Each mole of
H2O contains two moles of hydrogen atoms. Therefore, the number of moles of hydrogen is:
5×2=10‌ moles of ‌H Step 4: Determine the empirical formula.
The empirical formula is based on the simplest whole-number ratio of carbon to hydrogen. Here, the ratio is:
C4H10 Step 5: Verify the molecular formula.
Since the mass of the hydrocarbon produced the mentioned amounts of
CO2 and
H2O, the empirical formula is also the molecular formula for the given options. Therefore, the molecular formula of the compound is:
Option C:
C4H10