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Step-by-Step Solution
Step 1: Determine the mass of Carbon in the compound
From the given data, the complete combustion of the compound yields 2.64 g of CO2. The ratio of carbon’s mass to the mass of CO2 can be found as follows:
The molar mass of CO2 is $44 \text{ g/mol}$, where carbon’s mass in each mole of CO2 is $12 \text{ g}$. Thus, for every $44 \text{ g}$ of CO2, carbon contributes $12 \text{ g}$.
Therefore, the mass of carbon in $2.64 \text{ g}$ of CO2 is:
$ \text{Mass of C} = 2.64 \times \frac{12}{44} \text{ g} = 0.72 \text{ g}$
Step 2: Determine the mass of Hydrogen in the compound
The complete combustion of the compound also yields 1.08 g of H2O. The ratio of hydrogen’s mass to the mass of H2O is as follows:
The molar mass of H2O is $18 \text{ g/mol}$, where hydrogen’s mass in each mole of H2O is $2 \text{ g}$. Thus, for every $18 \text{ g}$ of H2O, hydrogen contributes $2 \text{ g}$.
Therefore, the mass of hydrogen in $1.08 \text{ g}$ of H2O is:
$ \text{Mass of H} = 1.08 \times \frac{2}{18} \text{ g} = 0.12 \text{ g}$
Step 3: Calculate the mass of Oxygen in the compound
We know the total mass of the compound taken for combustion is 1.80 g. The mass of oxygen in the compound can be found by subtracting the masses of carbon and hydrogen from the total mass:
$ \text{Mass of O} = 1.80 \text{ g} - (0.72 \text{ g} + 0.12 \text{ g}) = 0.96 \text{ g}$
Step 4: Calculate the percentage of Oxygen in the compound
The percentage of oxygen in the compound is given by the ratio of the mass of oxygen to the total mass of the compound, multiplied by 100:
$ \% \text{ of O} = \frac{0.96}{1.80} \times 100 = 53.33\%$
Hence, the percentage of oxygen in the compound is 53.33%.
