(Solved): Consider the decomposition of calcium carbonate: CaCO3(s)CaO(s)+CO2(g)H=177.8molkJ ...

Consider the decomposition of calcium carbonate: $\begin{array}{l}{\mathrm{CaCO}}_3(s)?\mathrm{CaO}(s)+{\mathrm{CO}}_2(\mathrm{g})\\ ?H^{?}=177.8\frac{\mathrm{kJ}}{\mathrm{mol}}\\ ?S^{?}=160.5\frac{\mathrm{J}}{\mathrm{mol}?\mathrm{K}}\end{array}$ Assume the $?H^{?}$ and $?S^{?}$ remain constant over the temperature range. Note: Reference the Fundamental constants table for additional information. Part 1 of 2 Calculate the equilibrium pressure, in atm, of ${\mathrm{CO}}_2$ at $25^{?}\mathrm{C}$. Be sure your answer has the correct number of significa $P_{{\mathrm{CO}}_2}=\mathrm{atm}$ Part 2 of 2 Calculate the equilibrium pressure, in atm, of ${\mathrm{CO}}_2$ at $766^{?}\mathrm{C}$. Be sure your answer has the correct number of signific $P_{{\mathrm{CO}}_2}=\mathrm{atm}$