Complete combustion of 1.80 g of an oxygen containing compound ($$C_xH_yO_z$$) gave 2.64 g of $$CO_2$$ and 1.08 g of $$H_2O$$. The percentage of oxygen in the organic compound is:

The compound has the formula $$C_xH_yO_z$$ and weighs 1.80 g. On complete combustion, it produces 2.64 g of $$CO_2$$ and 1.08 g of $$H_2O$$.

Moles of $$CO_2 = \frac{2.64}{44} = 0.06\,\text{mol}$$. Since each mole of $$CO_2$$ contains one mole of carbon, moles of C $$= 0.06$$. Mass of C $$= 0.06 \times 12 = 0.72\,\text{g}$$.

Moles of $$H_2O = \frac{1.08}{18} = 0.06\,\text{mol}$$. Since each mole of $$H_2O$$ contains 2 moles of hydrogen, moles of H $$= 0.12$$. Mass of H $$= 0.12 \times 1 = 0.12\,\text{g}$$.

Mass of oxygen in the compound $$= 1.80 - 0.72 - 0.12 = 0.96\,\text{g}$$.

Percentage of oxygen $$= \frac{0.96}{1.80} \times 100 = 53.33\%$$.

Therefore, the percentage of oxygen in the organic compound is $$53.33\%$$, which corresponds to option (1).