Chapter 14, Problem 42E

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 2.47 kJ of P-V work, pushing back the atmosphere as the gaseous CO₂ forms. At the same time, 38.95 kJ of heat is absorbed from the environment. What are the values of $\Delta H$ and of $\Delta E$ or this reaction?