CaCO3 + HCl →CO2 + CaCl2 + H2O Suppose you collect a 5.00 g sample of impure limestone and want to know how pure it is. You add the sample to an excess of HCl and collect 1.91 g of CO2. Assuming that the reaction went to completion, what percent of the sample was CaCO3?
CaCO3 + HCl →CO2 + CaCl2 + H2O Suppose you collect a 5.00 g sample of impure limestone and want to know how pure it is. You add the sample to an excess of HCl and collect 1.91 g of CO2. Assuming that the reaction went to completion, what percent of the sample was CaCO3?
Introductory Chemistry: A Foundation
9th Edition
ISBN:9781337399425
Author:Steven S. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Donald J. DeCoste
Chapter6: Chemical Reactions: An Introduction
Section: Chapter Questions
Problem 20QAP: Many over-the-counter antacid tablets are now formulated using calcium carbonate as the active...
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The DePauw Nature Park is a former quarry site where limestone, CaCO3, was mined until the 1970s. Limestone can be converted to carbon dioxide, CO2, by reacting it with hydrochloric acid, HCl, as shown by the following unbalanced
CaCO3 + HCl →CO2 + CaCl2 + H2O
Suppose you collect a 5.00 g sample of impure limestone and want to know how pure it is. You add the sample to an excess of HCl and collect 1.91 g of CO2. Assuming that the reaction went to completion, what percent of the sample was CaCO3?
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