Applications of Law of Mass Action and Law of Equilibrium

Answer the following questions :

Explain the effect of (x) pressure and (y) continuous removal of HI at constant temperature on the position of equilibrium of the following reaction :

${\mathrm{H}}_2\left(\mathrm{g}\right)+{\mathrm{I}}_2\left(\mathrm{g}\right)\rightleftharpoons 2\mathrm{HI}\left(\mathrm{g}\right)$

Reaction between nitrogen and oxygen takes place as follows:

$2{\mathrm{N}}_2\left(\mathrm{g}\right)+{\mathrm{O}}_2\left(\mathrm{g}\right)\rightleftharpoons 2{\mathrm{N}}_2\mathrm{O}\left(\mathrm{g}\right)$

If a mixture of $0.482 \mathrm{mol} \mathrm{of} {\mathrm{N}}_2 \mathrm{and} 0.933 \mathrm{mol} \mathrm{of} {\mathrm{O}}_2$ is placed in a reaction vessel of volume $10 \mathrm{L}$ and allowed to form ${\mathrm{N}}_2\mathrm{O}$ at a temperature for which ${\mathrm{K}}_{\mathrm{c}}=2.0\times {10}^{-37}.$ Determine the composition of equilibrium.

$3.00$ ml of ${\mathrm{PCl}}_5$ kept in $1\mathrm{L}$ closed reaction vessel was allowed to attain equilibrium at $380 \mathrm{K}$. Calculate the composition of the mixture at equilibrium. ${\mathrm{K}}_{\mathrm{c}}=1.80.$

The following concentrations were obtained for the formation of ${\mathrm{NH}}_3 \mathrm{from} {\mathrm{N}}_2 \mathrm{and} {\mathrm{H}}_2$ at equilibrium at 500 K:$\left[{\mathrm{N}}_2\right]=1.5\times {10}^{-2}\mathrm{M},\left[{\mathrm{H}}_2\right]=3.0\times {10}^{-2}\mathrm{M} \mathrm{and} \left[{\mathrm{NH}}_3\right]=1.2\times {10}^{-2}\mathrm{M}$

Calculate equilibrium constant.

One mole of nitrogen is mixed with three moles of hydrogen in a $4$ litre container. If $0.0025$ mole of nitrogen is converted to ammonia by the following reaction:

${\mathrm{N}}_2\left(\mathrm{g}\right)+3{\mathrm{H}}_2\left(\mathrm{g}\right)\rightleftharpoons 2{\mathrm{NH}}_3\left(\mathrm{g}\right)$

Calculate the equilibrium constant $\left({\mathrm{K}}_{\mathrm{c}}\right)$ in concentration units. What will be the value of ${\mathrm{K}}_{\mathrm{c}}$ for the following equilibrium?

$\frac{1}{2}{\mathrm{N}}_2\left(\mathrm{g}\right)+\frac{3}{2}{\mathrm{H}}_2\left(\mathrm{g}\right)\rightleftharpoons {\mathrm{NH}}_3\left(\mathrm{g}\right)$

Two moles of ${\mathrm{NH}}_3$ are introduced into one litre flask in which it dissociates at high temperature as follows:

$2{\mathrm{NH}}_3\left(\mathrm{g}\right)\rightleftharpoons {\mathrm{N}}_2\left(\mathrm{g}\right)+3{\mathrm{H}}_2\left(\mathrm{g}\right)$

Determine ${\mathrm{K}}_{\mathrm{c}}$ if at equilibrium one mole of ammonia remains.