**Transcription for Educational Website**---**51. Lead(II) Carbonate:**Lead(II) carbonate, also known as "white lead," was historically used as a pigment in white paints. Due to its toxicity, lead is no longer permitted in paints intended for residential homes. Lead(II) carbonate is produced industrially via the reaction of aqueous lead(II) acetate with carbon dioxide gas. The unbalanced chemical equation for this process is:\[ \text{Pb(C}_2\text{H}_3\text{O}_2\text{)}_2\text{(aq) + H}_2\text{O(l) + CO}_2\text{(g) } \rightarrow \text{ PbCO}_3\text{(s) + HC}_2\text{H}_3\text{O}_2\text{(aq)} \]**Problem Statement:**Suppose an aqueous solution containing 1.25 g of lead(II) acetate is treated with 5.95 g of carbon dioxide. Calculate the theoretical yield of lead carbonate.--- This transcription includes the chemical equation and problem context for understanding the reaction and performing yield calculations in a chemistry course.

The reaction taking place is given as, => Pb(C2H3O2)2 (aq) + H2O (l) + CO2 (g) → PbCO3 (s) + HC2H3O2 (aq) Given: Mass of Pb(C2H3O2)2 taken = 1.25 g. And the mass of CO2 taken = 5.95 g. Molar mass of CO2 = Atomic mass of C + Atomic mas O × 2 = 12 + 16 × 2 = 44 g/mol.And molar mass of Pb(C2H3O2)2 = Atomic mass of Pb + Atomic mass of C ×4 + Atomic mass of O × 4 + Atomic mass of H × 6 => molar mass of Pb(C2H3O2)2 = 207.2 + 12 × 4 + 1 × 6 + 16 × 4 = 325.2 g/mol.Since moles = MassMolar massHence moles of CO2 taken = 5.9544 = 0.13523 mol approx.And moles of Pb(C2H3O2)2 taken = 1.25325.2= 0.0038438 mol approx. Balancing: Since we have 2 C2H3O2 in the LHS. Hence making it 2 in RHS also. => Pb(C2H3O2)2 (aq) + H2O (l) + CO2 (g) → PbCO3 (s) + 2 HC2H3O2 (aq) Since all the elements are in equal number on both sides of the reaction now. Hence the reaction is now balanced.From the above-balanced reaction, we can see that 1 mole of CO2 is reacting with 1 mole of Pb(C2H3O2)2. Hence moles of Pb(C2H3O2)2 required = moles of CO2 taken = 0.13523 mol approx. Since moles of Pb(C2H3O2)2 taken is much less than required. Hence Pb(C2H3O2)2 is the limiting reagent and will react completely. Hence moles of PbCO3 produced theoretically = moles of Pb(C2H3O2)2 taken = 0.0038438 mol approx. Molar mass of PbCO3 = Atomic mass of Pb + Atomic mass of C + Atomic mass of O × 3=> Molar mass of PbCO3 = 207.2 + 12 + 16 × 3 = 267.2 g/mol.Hence the theoretical yield of PbCO3 = Moles × molar mass = 0.0038438 × 267.2 = 1.03 g approx. Hence the answer is 1.03 g approx.

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Lead(II) carbonate, also called "white lead, was formerly used as a pigment in white paints. However, because of its toxicity, lead can no longer be used in paints intended for residential homes. Lead(II) carbonate is prepared industrially by reaction of aqueous lead(II) acetate with carbon dioxide gas. The unbalanced equation is Pb(C2H3 O2), (aq) + H2O(1) + CO2 (9) → PBCO3(s) + HC,H3 O2 (aq) Suppose an aqueous solution containing 1.25 g of lead(II) acetate is treated with 5.95 g of carbon dioxide. Calculate the theoretical yield of lead carbonate.

Lead(II) carbonate, also called "white lead, was formerly used as a pigment in white paints. However, because of its toxicity, lead can no longer be used in paints intended for residential homes. Lead(II) carbonate is prepared industrially by reaction of aqueous lead(II) acetate with carbon dioxide gas. The unbalanced equation is Pb(C2H3 O2), (aq) + H2O(1) + CO2 (9) → PBCO3(s) + HC,H3 O2 (aq) Suppose an aqueous solution containing 1.25 g of lead(II) acetate is treated with 5.95 g of carbon dioxide. Calculate the theoretical yield of lead carbonate.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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