The reaction $\mathrm{AB}_{2(\mathrm{~g})} \rightleftharpoons \mathrm{AB}_{(\mathrm{g})}+\mathrm{B}_

Question

The reaction $\mathrm{AB}_{2(\mathrm{~g})} ightleftharpoons \mathrm{AB}_{(\mathrm{g})}+\mathrm{B}_{(\mathrm{g})}$ was conducted in a closed vessel, starting with pure $\mathrm{AB}_{2}$. The initial pressure was 1000 mm . and total pressure, at equilibrium, was 1200 mm . The value of equilibrium constant ( mm ) is\

Professor PC Thomas Classes · Answer

$\mathrm{AB}_{2} ightarrow \mathrm{AB}+\mathrm{B}$
 $\begin{tabular}{lll} 1000 & 0 & 0 \ $1000-\mathrm{x}$ & x & x \ \end{tabular}$ \Total pressure , $1000+x=1200, x=200$\ So partial pressures are\ $\left[\mathrm{AB}_{2}ight]=800$,\ $[\mathrm{AB}]=200[\mathrm{~B}]=200$ $$ \mathrm{kp}=\frac{\mathrm{x}^{2}}{1000-\mathrm{x}}=\frac{200 	imes 200}{800}=50 $$