What volume of $O_2$ (g) at $350^oC$ and a pressure of 5.25 atm is needed to completely convert 5.00 g of sulfur to sulfur trioxide?

Question

Sulfur trioxide, $SO_3$ , is produced in enormous quantities each year for use in the synthesis of sulfuric acid.
$S (s) + O_2 (g) -> SO_2 (g)$
$2SO_2 (g) + O2 (g) -> 2SO_3 (g)$

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Answer 1 · 2017-06-22T05:17:22

Approx..... $2*L$

We can combine the given equations........

$S(s) + 3/2O_2(g) rarr SO_3(g)$

And this clearly gives us the mass transfer; 1 equiv of sulfur is oxidized by 3/2 equiv dioxygen gas.....

$"Moles of sulfur"=(5.00*g)/(32.06*g*mol^-1)=0.156*mol$

And so we need $0.156*molxx3/2xx32.00*g*mol^-1=7.49*g$ with respect to dioxygen gas......

And we use the Ideal Gas Equation.......

$V=(nRT)/P=((7.49*g)/(32.00*g*mol^-1)xx0.0821*(L*atm)/(K*mol)xx623.2*K)/(5.25*atm)$

$=??L$