When \( \mathrm{N}_{2} \mathrm{O}_{5} \) is heated at certain temperature, it dissociates as \( ...
0When \( \mathrm{N}_{2} \mathrm{O}_{5} \) is heated at certain temperature, it dissociates as
\( \mathrm{N}_{2} \mathrm{O}_{5}(g) \rightleftharpoons \mathrm{N}_{2} \mathrm{O}_{3}(g)+\mathrm{O}_{2}(g) ; \mathrm{K}_{c}=2.5 \). At the same time \( \mathrm{N}_{2} \mathrm{O}_{3} \) also decomposes as :
\( \mathrm{N}_{2} \mathrm{O}_{3}(g) \rightleftharpoons \mathrm{N}_{2} \mathrm{O}(g)+\mathrm{O}_{2}(g) \). If initially \( 4.0 \) moles of \( \mathrm{N}_{2} \mathrm{O}_{5} \) are taken in \( 1.0 \) litre flask and
allowed to dissociate. Concentration of \( \mathrm{O}_{2} \) at equilibrium is \( 2.5 \mathrm{M} \). Equilibrium concentration
of \( \mathrm{N}_{2} \mathrm{O}_{5} \) is:
\( \begin{array}{llll}\text { (a) } 1.0 \mathrm{M} & \text { (b) } 1.5 \mathrm{M} & \text { (c) } 2.166 M & \text { (d) } 1.846 M\end{array} \)
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