The chemical reaction is:
H2SO4(aq) + Pb(C2H3O2)2(aq) → PbSO4(s) + HC2H3O2(aq)
Balancing this gives us:
H2SO4(aq) + Pb(C2H3O2)2(aq) → PbSO4(s) + 2 HC2H3O2(aq)
We're being asked to determine the mass of H2SO4 present in the mixture after the reaction is complete. This means that H2SO4 is the excess reactant while Pb(C2H3O2)2 is the limiting reactant.
The molar mass of H2SO4 is 2(1.01 g/mol H) + 32.06 g/mol S + 4(16.00 g/mol O) = 98.08 g/mol. The molar mass of Pb(C2H3O2)2 is 207.20 g/mol Pb + 4(12.01 g/mol C) + 6(1.01 g/mol H) + 4(16.00 g/mol O) = 325.30 g/mol. From the balanced chemical equation, 1 mole of Pb(C2H3O2)2 reacts with 1 mole of H2SO4.
Calculate the number of grams of sulfuric acid present in the mixture after the reaction is complete.
Frequently Asked Questions
What scientific concept do you need to know in order to solve this problem?
Our tutors have indicated that to solve this problem you will need to apply the Limiting Reagent concept. If you need more Limiting Reagent practice, you can also practice Limiting Reagent practice problems.
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Based on our data, we think this problem is relevant for Professor Kizilkaya's class at LSU.