The reaction of sulfur trioxide with atmospheric water droplets results in sulfuric acid, a contributor to acid rain.According to the equation below, how many moles of sulfuric acid can you predict will be formed from 58.0 g of SO3 and an excess of water?

Question

SO3(g) + H2O(l) H2SO4(aq)

    A.  0.592 mol
    B.  0.724 mol
    C.  0.242 mol
    D.  1.45 mol

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Answer 1 · 2017-11-05T18:43:25

#"Option B"#

We gots the stoichiometric equation...

#SO_3(g) + H_2O(l) rarr H_2SO_4(g)#

#"Moles of sulfur trioxide"=(58.0*g)/(80.07*g*mol^-1)=0.724*mol#.

And given the stoichiometry, an equimolar quantity of sulfuric acid will be formed....what mass?

SO3(g) + H2O(l) H2SO4(aq)

`A. 0.592 mol B. 0.724 mol C. 0.242 mol D. 1.45 mol`