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In the lab, students decomposed a sample of calcium carbonate by heating it over a Bunsen burner and collected carbon dioxide according to the following equation: CaCO3(s) CaO(s) + CO2g) (a) How many mL of carbon dioxide gas were generated by the decomposition of 5.38 g of calcium carbonate at STP? _mL (b) How many moles of calcium carbonate would be required to generate 57.9 L of carbon dioxide at STP? _mol CaCO3

In the lab, students decomposed a sample of calcium carbonate by heating it over a Bunsen burner and collected carbon dioxide according to the following equation: CaCO3(s) CaO(s) + CO2g) (a) How many mL of carbon dioxide gas were generated by the decomposition of 5.38 g of calcium carbonate at STP? _mL (b) How many moles of calcium carbonate would be required to generate 57.9 L of carbon dioxide at STP? _mol CaCO3

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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In the lab, students decomposed a sample of calcium carbonate by heating it over a Bunsen burner and collected carbon dioxide according to the following equation: CaCO3(s) CaO(s) + CO2g) (a) How many mL of carbon dioxide gas were generated by the decomposition of 5.38 g of calcium carbonate at STP? _mL (b) How many moles of calcium carbonate would be required to generate 57.9 L of carbon dioxide at STP? _mol CaCO3
Transcribed Image Text:In the lab, students decomposed a sample of calcium carbonate by heating it over a Bunsen burner and collected carbon dioxide according to the following equation: CaCO3(s) CaO(s) + CO2g) (a) How many mL of carbon dioxide gas were generated by the decomposition of 5.38 g of calcium carbonate at STP? _mL (b) How many moles of calcium carbonate would be required to generate 57.9 L of carbon dioxide at STP? _mol CaCO3
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