Chapter 15, Problem 1SEPP

Lime $\left(\text{CaO}\right)$ is used to prevent ${\text{SO}}_{\text{2}}$ from escaping from the smokestacks of coal-burning power plants via the formation of solid ${\text{CaSO}}_{\text{4}}\cdot {\text{ 2H}}_{\text{2}}\text{O}$ (gypsum). One of the important reactions in the overall process is the decomposition of ${\text{CaCO}}_{\text{3}}$:

${\text{CaCO}}_{\text{3}}\left(s\right)\underset{}{\rightleftarrows }\text{ CaO}\left(s\right){\text{ + CO}}_{\text{2}}\left(g\right)$

which has an equilibrium constant $\left(K_{\text{c}}\right)\text{ of 3}\text{.0 }\times {\text{ 10}}^{\text{-6}}\text{ at 725°C}\text{.}$

Calculate the value of $K_{\text{p}}$ for the decomposition of ${\text{CaCO}}_{\text{3}}\text{ at 725°C}$

$\begin{array}{l}\text{a)}\hfill \\ \text{3}\text{.0 }\times {\text{ 10}}^{\text{-6}}\hfill \\ \text{b)}\hfill \\ \text{2}\text{.5}\times {\text{10}}^{\text{-4}}\hfill \\ \text{c)}\hfill \\ \text{2}\text{.0 }\times {\text{ 10}}^{\text{-2}}\hfill \\ \text{d)}\hfill \\ \text{37 }\times {\text{ 10}}^{\text{-8}}\hfill \end{array}$