How many oxygen molecules are required to oxidize a #4.42*g# mass of sulfur?

1 Answer
anor277
Dec 23, 2017

We address the stoichiometric equation...

#S(s) + O_2(g) rarr SO_2(g)#

Explanation:

Sulfur COULD be oxidized further, but we will stick with this formula for this calculation.

#"Moles of sulfur"=(4.42*g)/(32.06*g*mol^-1)=0.138*mol#

Given the stoichiometry of the reaction we need #0.138*mol# dioxygen molecules for equivalence, i.e. #0.138*molxx6.022xx10^23*mol^-1=??# #O_2# #"molecules?"#

What mass of dioxygen does this represent?

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