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 SO₄^2-. 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 Mn^2+. 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?