[References] 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 3.043 g sanmple of limestone-containing material gave 1.25 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?
[References] 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 3.043 g sanmple of limestone-containing material gave 1.25 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?
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![[References]
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 3.043 g sanmple of limestone-containing material gave 1.25 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?](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F4ab01804-9df7-476f-99db-b22132fa7e75%2F3a6c7724-c2f5-463f-bab1-c998a08a2769%2Fahbn3dq.jpeg&w=3840&q=75)
Transcribed Image Text:[References]
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 3.043 g sanmple of limestone-containing material gave 1.25 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?
Expert Solution
Step 1
Calcium carbonate decomposes into calcium oxide and carbon dioxide. The equation for the balanced chemical reaction is as follows:
Mass of the limestone sample is = 3.043 g
Mass of CO2 = 1.25 g
The mass percent of CaCO3 in the sample =?
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