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) + CO2(3) (a) How many mL of carbon dioxide gas were generated by the decomposition of 3.33 g of calcium carbonate at STP? mL (b) How many moles of calcium carbonate would be required to generate 55.5 L of carbon dioxide at STP? i 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) + CO2(3) (a) How many mL of carbon dioxide gas were generated by the decomposition of 3.33 g of calcium carbonate at STP? mL (b) How many moles of calcium carbonate would be required to generate 55.5 L of carbon dioxide at STP? i mol CaCO3

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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