Limestone stalactites and stalagmites are formed in caves by the following reaction: Ca2+(aq) + 2HCO3 (aq) → CaCO3(s) + CO2(g) + H2O(l) -> If 1 mol of CaCO3 forms at 298 K under 1 atm pressure, the reaction performs 2.45 kJ of P-V work, pushing back the atmosphere as the gaseous CO2 forms. At the same time, 38.80 kJ of heat is absorbed from the environment.

Limestone stalactites and stalagmites are formed in caves by the following reaction: Ca2+(aq) + 2HCO3 (aq) → CaCO3(s) + CO2(g) + H2O(l) -> If 1 mol of CaCO3 forms at 298 K under 1 atm pressure, the reaction performs 2.45 kJ of P-V work, pushing back the atmosphere as the gaseous CO2 forms. At the same time, 38.80 kJ of heat is absorbed from the environment.

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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