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### Consider the systems shown in Figure 5.10. In one…

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Oklahoma State University

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Problem 103

Limestone stalactites and stalagmites are formed in caves by
the following reaction:
$$\mathrm{Ca}^{2+}(a q)+2 \mathrm{HCO}_{3}^{-}(a q) \longrightarrow \mathrm{CaCO}_{3}(s)+\mathrm{CO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(l)$$
If 1 $\mathrm{mol}$ of $\mathrm{CaCO}_{3}$ forms at 298 $\mathrm{K}$ under 1 atm pressure, the
reaction performs 2.47 $\mathrm{kJ}$ of $P-V$ work, pushing back the atmo-
sphere as the gaseous $\mathrm{CO}_{2}$ forms. At the same time, 3.95 $\mathrm{kJ}$
of heat is absorbed from the environment. What are the
values of $\Delta H$ and of $\Delta E$ for this reaction?

\begin{aligned} \Delta H &=+38.95 \mathrm{kJ} \\ \Delta E &=+36.48 \mathrm{kJ} \end{aligned}

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## Video Transcript

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