Answered: H2Olag) + CaCl2 • 2H2O(ag) → CaC204 •…

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter4: Stoichiometry

Section: Chapter Questions

Problem 4.106PAE: 4.106 An ore sample with a mass of 670 kg contains 27.7% magnesium carbonate, MgCO3. If all of the...

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K2C204 • H2Otag) + CaCl2 • 2H20(ag) → CaC204 • H2O(s) + 2KCl(ag) + 2H2O)
A 0.422 g sample of CaCl2 • 2H20 (molar mass = 147 g/mol) was reacted with 0.644 g of K2C204 • H20
(molar mass = 184 g/mol).
%3D
a. Calculate the moles of CaCl2 • 2H2O added.
b. Calculate the moles of K2C204 • H2O added.
Determine the limiting reactant and theoretical yield of CaC204 • H2O (molar mass = 146
g/mol).
с.
d. Calculate the mass of excess reactant that did not react.

Transcribed Image Text:K2C204 • H2Olag) + CaCl2 • 2H2O(ag) → CaC204 • H2O(s) + 2KCI(ag) + 2H2O) Unspecified amounts of CaCl2 • 2H2O and K2C2O4 • H2O were reacted and the calcium oxalate precipitate was allowed to settle to the bottom of the beaker. Two samples of clear supernatant were tested for the presence of unreacted ions by adding calcium chloride to one sample and potassium oxalate to the other. The sample in which calcium chloride was added showed the formation of a white precipitate whereas the sample in which potassium oxalate was added remained a clear solution. From this profile, identify the limiting reactant. Justify your answer.

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