A sample of limestone and other soil materials was heated, and the limestone decomposed to give calcium oxide and carbon dioxide. CACO3(s) → CaO(s) + CO2(g) A 2.631 g sample of limestone-containing material gave 1.08 g of CO2, in addition to CaO, after being heated at a high temperature. What was the mass percent of CaCO3 in the origînal sample?

Chemistry & Chemical Reactivity
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Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
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Chapter4: Stoichiometry: Quantitative Information About Chemical Reactions
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A sample of limestone and other soil materials was heated, and the limestone decomposed to give calcium oxide and carbon dioxide.
CACO3 (s) → CaO(s) + CO2(g)
A 2.631 g sample of limestone-containing material gave 1.08 g of
CO2, in addition to
CaO, after being heated at a high temperature. What was the mass percent of
CaCO3 in the original sample?
Transcribed Image Text:A sample of limestone and other soil materials was heated, and the limestone decomposed to give calcium oxide and carbon dioxide. CACO3 (s) → CaO(s) + CO2(g) A 2.631 g sample of limestone-containing material gave 1.08 g of CO2, in addition to CaO, after being heated at a high temperature. What was the mass percent of CaCO3 in the original sample?
An unknown compound has the formula
C,H,0z. You burn 0.1258 g of the compound and isolate 0.3071 g of
CO2 and 0.1257 g of
H2O. What is the empirical formula of the compound? If the molar mass is 72.1 g/mol, what is the molecular formula?
(Enter the elements in the order: C, H, O.)
Empirical formula:
Molecular formula:
Transcribed Image Text:An unknown compound has the formula C,H,0z. You burn 0.1258 g of the compound and isolate 0.3071 g of CO2 and 0.1257 g of H2O. What is the empirical formula of the compound? If the molar mass is 72.1 g/mol, what is the molecular formula? (Enter the elements in the order: C, H, O.) Empirical formula: Molecular formula:
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