Exercise - Numericals

1. For the decomposition of dinitrogen oxide $({\mathrm{N}}_2\mathrm{O})$$(\mathrm{N}_{2}\mathrm{O})$ into nitrogen and oxygen reversible reaction takes place as follows

The concentration of ${\mathrm{N}}_2\mathrm{O}$$\mathrm{N}_2\mathrm{O}$ , ${\mathrm{N}}_2$$\mathrm{N}_2$ and ${\mathrm{O}}_2$$\mathrm{O}_2$ are $1.1\mathrm{m}\mathrm{o}\mathrm{l}{\mathrm{d}\mathrm{m}}^{-3}$$1.1 \mathrm{mol} \mathrm{dm}^{- 3}$ , $3.90\mathrm{m}\mathrm{o}\mathrm{l}{\mathrm{d}\mathrm{m}}^{-3}$$3.90 \mathrm{mol} \mathrm{dm}^{- 3}$ and $1.95\mathrm{m}\mathrm{o}\mathrm{l}{\mathrm{d}\mathrm{m}}^{-3}$$1.95 \mathrm{mol} \mathrm{dm}^{- 3}$ respectively at equilibrium. Find out ${\mathrm{K}}_c$$\mathrm{K}_c$ for this reaction.

2. Hydrogen iodide decomposes to form hydrogen and iodine. If the equilibrium concentration of HI is $0.078\mathrm{m}\mathrm{o}\mathrm{l}{\mathrm{d}\mathrm{m}}^{-3}$$0.078 \mathrm{mol} \mathrm{dm}^{-3}$ , ${\mathrm{H}}_2$$\mathrm{H}_2$ and ${\mathrm{I}}_2$$\mathrm{I}_2$ is same $0.011\mathrm{m}\mathrm{o}\mathrm{l}{\mathrm{d}\mathrm{m}}^{-3}$$0.011 \mathrm{mol} \mathrm{dm}^{-3}$ . Calculate the equilibrium constant value for this reversible reaction: