chemistry

Consider the following reaction.
SO3(g) + H2O(l) → H2SO4(aq)

A chemist allows 60.9 g of SO3 and 11.1 g of H2O to react. When the reaction is finished, the chemist collects 54.4 g of H2SO4. Determine the limiting reactant, theoretical yield, and percent yield for the reaction

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  1. mols SO3 = grams/molar mass = ?
    mols H2O = grams/molar mass = ?

    Using the coefficients in the balanced equation, convert mols SO3 to mols H2SO4.
    Do the same and convert mols H2O to mols H2SO4.
    In limiting reagent problems the SMALLER amount of product formed is ALWAYS the right correct answer and the reagent responsible for that is the limiting reagent.
    Then grams H2SO4 = mols H2SO4 x molar mass H2SO4. The is the theoretical yield(TY). The actual yield (AY) in the problem is 54.4 g.
    % yield = (AY/TY)*100 = ?

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