Question

# At 273K and 1atm $\alpha$ L of ${{N}_{2}}{{O}_{4}}(g)\to 2N{{O}_{2}}(g)$.To what extent has the decomposition proceeded when the original volume is 25% less than that of existing volume ?(A) $\alpha$ = 40%(B) $\alpha$ = 10%(C) $\alpha$ = 33%(D) $\alpha$ = 67%

Hint: The initial concentration of ${{N}_{2}}{{O}_{4}}$ could be taken as 100 to proceed with the solution. The conversion of ${{N}_{2}}{{O}_{4}}$ to $N{{O}_{2}}$ is exothermic, because ${{N}_{2}}{{O}_{4}}$ is more stable than $N{{O}_{2}}$, therefore it requires energy for conversion.

Let the initial volume of ${{N}_{2}}{{O}_{4}}$ be x , concentration of $N{{O}_{2}}$will be zero,
${{N}_{2}}{{O}_{4}}\to 2N{{O}_{2}}$
After time t at equilibrium, the concentration of ${{N}_{2}}{{O}_{4}}$ will be , $x(1-\alpha )$ and concentration of $N{{O}_{2}}$ will become, $2\alpha x$, where $\alpha$ is the de
Total equilibrium volume = $x(1-\alpha )$+$2\alpha x$=$x(1+\alpha )$
\begin{align} & x=75\times (1+\alpha ) \\ & \Rightarrow 100=75\times (1+\alpha ) \\ & \Rightarrow (1+\alpha )=1.33 \\ & \Rightarrow \alpha =0.33 \\ \end{align}
Note: Decomposition of ${{N}_{2}}{{O}_{4}}$ and hydrogen peroxide is a first order reaction. The conversion of $N{{O}_{2}}$ to ${{N}_{2}}{{O}_{4}}$ is endothermic. Nitrogen dioxide is a toxic gas with pungent odour, it is reddish brown in color. When cooled, the liquid freezes to form a colorless crystalline solid that consists almost entirely of the dimeric form, ${{N}_{2}}{{O}_{4}}$. Nitrogen tetroxide is used as an oxidizer in one of the most important rocket propellants because it can be stored as a liquid at room temperature.