In: Chemistry
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.
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 %