The homogeneous reversible reaction, ${\mathrm{C}}_2{\mathrm{H}}_5\mathrm{OH}+{\mathrm{CH}}_3\mathrm{COOH}\rightleftharpoons {\mathrm{CH}}_3{\mathrm{COOC}}_2{\mathrm{H}}_5+{\mathrm{H}}_2\mathrm{O}$
is studied at various initial concentrations of the reactants at a constant temperature. Calculate the value of $\mathrm{X} \text{and} \mathrm{Y}$ if the initial concentration of both constituents is equal.

	Moles of acid per litre (initial)	Moles of alcohol per litre (initial)	Moles of ester per litre at equilibrium
$\left(\mathrm{i}\right)$	$1$	$1$	$0.667$
$\left(\mathrm{ii}\right)$	$\mathrm{X}$	$\mathrm{Y}$	$8/3$

Write the expressions for equilibrium constant ${\mathrm{K}}_{\mathrm{C}}$ and and  ${\mathrm{K}}_{\mathrm{p}}$. Classify in Homogeneous and Heterogeneous equilibrium:

${\mathrm{N}}_2{\mathrm{O}}_4\left(\mathrm{g}\right)\rightleftharpoons 2{\mathrm{NO}}_2\left(\mathrm{g}\right)$

Write the expressions for equilibrium constant ${\mathrm{K}}_{\mathrm{C}}$ and  ${\mathrm{K}}_{\mathrm{p}}$. Classify in Homogeneous and Heterogeneous equilibrium:

$3\mathrm{Fe}\left(\mathrm{s}\right)+4{\mathrm{H}}_2\mathrm{O}\left(\mathrm{g}\right)\rightleftharpoons {\mathrm{Fe}}_3{\mathrm{O}}_4\left(\mathrm{s}\right)+4{\mathrm{H}}_2\left(\mathrm{g}\right)$

Write the expressions for equilibrium constant ${\mathrm{K}}_{\mathrm{C}}$ and  ${\mathrm{K}}_{\mathrm{p}}$. Classify in Homogeneous and Heterogeneous equilibrium:

${\mathrm{NH}}_4\mathrm{HS}\left(\mathrm{s}\right)\rightleftharpoons {\mathrm{NH}}_3\left(\mathrm{g}\right)+{\mathrm{H}}_2\mathrm{S}\left(\mathrm{g}\right)$

Write the expressions for equilibrium constant ${\mathrm{K}}_{\mathrm{C}}$ and  ${\mathrm{K}}_{\mathrm{p}}$. Classify in Homogeneous and Heterogeneous equilibrium:

${\mathrm{CH}}_3\mathrm{COOH}\left(\mathrm{\ell }\right)+{\mathrm{C}}_2{\mathrm{H}}_5\mathrm{OH}\left(\mathrm{\ell }\right)\rightleftharpoons {\mathrm{CH}}_3{\mathrm{COOC}}_2{\mathrm{H}}_5\left(\mathrm{\ell }\right)+{\mathrm{H}}_2\mathrm{O}\left(\mathrm{\ell }\right)$

Write the expressions for equilibrium constant ${\mathrm{K}}_{\mathrm{C}}$ and  ${\mathrm{K}}_{\mathrm{p}}$. Classify in Homogeneous and Heterogeneous equilibrium:

${\mathrm{MgCO}}_3\left(\mathrm{s}\right)\rightleftharpoons \mathrm{MgO}\left(\mathrm{s}\right)+{\mathrm{CO}}_2\left(\mathrm{g}\right)$

Write the expressions for equilibrium constant ${\mathrm{K}}_{\mathrm{C}}$ and  ${\mathrm{K}}_{\mathrm{p}}$classify in homogeneous and heterogeneous equilibrium:

${\mathrm{NH}}_4{\mathrm{NO}}_2 \left(\mathrm{s}\right)\rightleftharpoons {\mathrm{N}}_2 \left(\mathrm{g}\right)+2{\mathrm{H}}_2\mathrm{O} \left(\mathrm{l}\right)$

For the given reaction at equilibrium:

${\mathrm{AgNO}}_3\left(\mathrm{s}\right)\rightleftharpoons \mathrm{Ag}\left(\mathrm{s}\right)+{\mathrm{NO}}_2\left(\mathrm{g}\right)+\frac{1}{2}{\mathrm{O}}_2\left(\mathrm{g}\right)$

If total pressure at equilibrium is $\mathrm{P}$, then calculate ${\mathrm{K}}_{\mathrm{p}}$ for the given reaction.