Chapter 14, Problem

Nitrous oxide, ${\text{N}}_{\text{2}}\text{O}$, is a gas used as an anesthetic; ir is sometimes called “laughing gas." This compound has a strong tendency to decompose into nitrogen and oxygen following the equation

${\text{2N}}_{\text{2}}\text{O}\left(g\right)\stackrel{}{\rightleftarrows }{\text{ 2N}}_{\text{2}}\left(g\right){\text{+ O}}_{\text{2}}\left(g\right)$

but the reaction is so slow that the gas appears to be stable at room temperature $\left(\text{25 °C}\right)$. The decomposition reaction has $Kc=7.3\times {10}^{34}$. What is the value of $K_p$ for this reaction at $\text{25 °C}$? (Hint: Be careful in calculating $\Delta n_g$)