To find the percentage of oxygen composition in the organic compound, we will follow these steps:
### Step 1: Calculate the moles of carbon from CO₂ produced
The mass of CO₂ produced is 0.793 g. The molar mass of CO₂ is 44 g/mol (12 g/mol for C and 32 g/mol for O).
\[
\text{Moles of } CO_2 = \frac{\text{mass of } CO_2}{\text{molar mass of } CO_2} = \frac{0.793 \, \text{g}}{44 \, \text{g/mol}} \approx 0.0180 \, \text{mol}
\]
### Step 2: Calculate the mass of carbon in the organic compound
From the moles of CO₂, we can find the moles of carbon (C) since each mole of CO₂ contains one mole of carbon.
\[
\text{Moles of C} = \text{Moles of } CO_2 = 0.0180 \, \text{mol}
\]
Now, calculate the mass of carbon:
\[
\text{Mass of C} = \text{Moles of C} \times \text{molar mass of C} = 0.0180 \, \text{mol} \times 12 \, \text{g/mol} \approx 0.216 \, \text{g}
\]
### Step 3: Calculate the moles of hydrogen from H₂O produced
The mass of H₂O produced is 0.442 g. The molar mass of H₂O is 18 g/mol (2 g/mol for H and 16 g/mol for O).
\[
\text{Moles of } H_2O = \frac{\text{mass of } H_2O}{\text{molar mass of } H_2O} = \frac{0.442 \, \text{g}}{18 \, \text{g/mol}} \approx 0.0246 \, \text{mol}
\]
### Step 4: Calculate the mass of hydrogen in the organic compound
From the moles of H₂O, we can find the moles of hydrogen (H) since each mole of H₂O contains two moles of hydrogen.
\[
\text{Moles of H} = 2 \times \text{Moles of } H_2O = 2 \times 0.0246 \, \text{mol} \approx 0.0492 \, \text{mol}
\]
Now, calculate the mass of hydrogen:
\[
\text{Mass of H} = \text{Moles of H} \times \text{molar mass of H} = 0.0492 \, \text{mol} \times 1 \, \text{g/mol} \approx 0.0492 \, \text{g}
\]
### Step 5: Calculate the mass of oxygen in the organic compound
Now we can find the mass of oxygen (O) in the organic compound. The total mass of the organic compound is given as 0.492 g.
\[
\text{Mass of O} = \text{Total mass} - (\text{Mass of C} + \text{Mass of H})
\]
Substituting the values we calculated:
\[
\text{Mass of O} = 0.492 \, \text{g} - (0.216 \, \text{g} + 0.0492 \, \text{g}) \approx 0.2268 \, \text{g}
\]
### Step 6: Calculate the percentage of oxygen in the organic compound
Finally, we can calculate the percentage of oxygen in the organic compound:
\[
\text{Percentage of O} = \left( \frac{\text{Mass of O}}{\text{Total mass}} \right) \times 100 = \left( \frac{0.2268 \, \text{g}}{0.492 \, \text{g}} \right) \times 100 \approx 46.1\%
\]
Rounding to the nearest integer, the percentage of oxygen composition in the organic compound is **46%**.
