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Consider the following reaction between sulfur trioxide and water: SO3(g)+H2O(l)=H2SO4(aq) A chemist allows 61.5 g fo SO3 and...

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Chemistry

Consider the following reaction between sulfur trioxide andwater:

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

A chemist allows 61.5 g fo SO3 and 11.2 g of H2O to react. Whenthe reaction is finished, the chemist collects 51.0g of H2SO4.

1) Determine the theoretical yield for the reaction.

2) Determine the percent yield for the reaction.

Answer & Explanation Solved by verified expert
3.5 Ratings (351 Votes)

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

Moles       61.5/80                   11.2/18

              = 0.76875               = 0.622     

Water is limiting reagnet so all caluclations should be according to water

expected moles of H2SO4(aq) formed = 0.622 moles

Mass of   H2SO4(aq) formed    = 0.622x98 = 60.9 75 gram ( theoretical yield)

% yield = (actual mass formed/expected mass )x100 = ( 51.0g/60.9 75)x100 = 83.64 %
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