An organic compound contains Carbon, Hydrogen and Sulfur. Asample of it with a mass of 2.107 g was burned in oxygen to give gaseous CO2 SO2 and H2O . These gases were passed through 503.8 mL of an acidified 0.0200 MKMnO4 solution, which caused the SO2 tobe oxidized to SO42-. Only part of the available KMnO4 was reduced to Mn2+. Next,50.38 mL of 0.0300 M SnCl2 was added to 50.38 a mL portion of this solution, which still contained unreduced KMnO4. There was more than enough added SnCl2to cause all the remaining MnO4- in the 50.38mL portion to be reduced to Mn2+. The excess Sn2+ that still remained after the reaction was then titrated with 0.0100 M KMnO4, requiring 0.02562 L of the KMnO4 solution to reach the end point. Based upon allthis data, what is the percentage of Sulfur in the original sample of the organic compound that had been burned is?