Question

In: Chemistry

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

Consider the following reaction between sulfur trioxide and water:

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

A chemist allows 61.5 g fo SO3 and 11.2 g of H2O to react. When the 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.

Solutions

Expert Solution

                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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