For the following reaction,CaCl2(aq) + 2NaHCO3(aq) → CaCO3(s) + H2O(l) + CO2(g) + 2NaCl(aq)Molar mass of CaCl2 = 110.98 g/molMolar mass of NaHCO3 = 84.007 g/molMolar mass of CaCO3 = 100.09 g/molThe CaCl2 used in this experiment exist as a dihydrate, CaCl2 ⋅⋅ 2H2O. If 1.00 g of CaCl2 ⋅⋅ 2H2O reacted with an excess amount of NaHCO3, how many grams of solid CaCO3 should precipitate out?

The given reaction is: CaCl2(aq) + 2NaHCO3(aq) → CaCO3(s) + H2O(l) + CO2(g) + 2NaCl(aq) Let, the…

Answered: For the following reaction, CaCl2(aq)…

Introduction to Chemical Engineering Thermodynamics

8th Edition

ISBN:9781259696527

Author:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart

Publisher:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart

Chapter1: Introduction

Section: Chapter Questions

Problem 1.1P

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For the following reaction,

CaCl₂(aq) + 2NaHCO₃(aq) → CaCO₃(s) + H₂O(l) + CO₂(g) + 2NaCl(aq)

Molar mass of CaCl₂ = 110.98 g/mol
Molar mass of NaHCO₃ = 84.007 g/mol
Molar mass of CaCO₃ = 100.09 g/mol

The CaCl₂ used in this experiment exist as a dihydrate, CaCl₂ ⋅⋅ 2H₂O. If 1.00 g of CaCl₂ ⋅⋅ 2H₂O reacted with an excess amount of NaHCO₃, how many grams of solid CaCO₃ should precipitate out?

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