64 g of sulfur is burnt to SO2 with 90% yield. The SO2 is then oxidised, 2SO2 + O2 -> 2SO3, with 75% yield. The mass of SO3 finally obtained is (S = 32, O = 16)

JEE Advanced levelSingle correct optionDifficulty 3 of 3mc195

$64 g$ of sulfur is burnt to $SO X_{2}$ with $90%$ yield. The $SO X_{2}$ is then oxidised, $2 SO X_{2} + O X_{2} 2 SO X_{3}$ , with $75%$ yield. The mass of $SO X_{3}$ finally obtained is (S = 32, O = 16)

n(S) = 2.00 mol gives 2 x 0.90 = 1.80 mol SO2. This gives 1.350 mol SO3 (1 : 1 mole ratio, 75% yield). Mass = 1.35 x 80 = 108 g.