An organic compound contains carbon, hydrogen, and sulfur. A sample of it with a mass of 1.548 g was burned in oxygen to give gaseous CO2, H2O, and SO2. These gases were passed through 574.8 mL of an acidified 0.0200 M KMnO4 solution, which caused the SO2 to be oxidized to SO42-. Only part of the available KMnO4 was reduced to Mn2+. Next, 57.48 mL of 0.0300 M SnCl2 was added to 57.48 a mL portion of this solution, which still contained unreduced KMnO4. There was more than enough added SnCl2 to cause all of the remaining MnO4- in the 57.48 mL portion to be reduced to Mn2+. The excess Sn2+ that still remained after the reaction was then titrated with 0.0100 M KMnO4, requiring 0.02844 L of the KMnO4 solution to reach the end point. Based upon all this data, the percentage of sulfur in the original sample of the organic compound that had been burned is_______________.