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?

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)#

1 Answer
Jun 22, 2017

Answer:

Approx.....#2*L#

Explanation:

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#