Heterogeneous Equilibria

The molar concentrations of a pure solid or liquid are not considered, while writing the equilibrium expressions.

Write the expression for the equilibrium constant ${\mathrm{K}}_{\mathrm{c}}$ for the following reaction:

${\mathrm{CO}}_2\left(\mathrm{g}\right)+\mathrm{C}\left(\mathrm{s}\right)\stackrel{ }{\rightleftharpoons }2\mathrm{CO}\left(\mathrm{g}\right)$

Write the expression for the equilibrium constant, ${\mathrm{K}}_{\mathrm{c}}$ for the following reaction, ${\mathrm{Br}}_2\left(\mathrm{l}\right) \rightleftharpoons {\mathrm{Br}}_2\left(\mathrm{g}\right)$.

Write the expression for the equilibrium constant ${\mathrm{K}}_{\mathrm{c}}$ for the following reaction:

${\mathrm{PCl}}_3\left(\mathrm{l}\right)+{\mathrm{Cl}}_2\left(\mathrm{g}\right)\stackrel{ }{\rightleftharpoons }{\mathrm{PCl}}_5\left(\mathrm{s}\right)$

Write the expression for the equilibrium constant, ${\mathrm{K}}_{\mathrm{c}}$ for the following reaction:
$\mathrm{Cu}\left(\mathrm{s}\right)+2{\mathrm{Ag}}^{+}\left(\mathrm{aq}\right) \stackrel{ }{\rightleftharpoons } {\mathrm{Cu}}^{2+}\left(\mathrm{aq}\right)+2\mathrm{Ag}\left(\mathrm{s}\right)$

Explain heterogeneous equilibrium with the help of an example.

Write the expression for the equilibrium constant ${\mathrm{K}}_{\mathrm{c}}$ for the following reaction:

${{\mathrm{CrO}}_4}^{2-}\left(\mathrm{aq}\right)+{\mathrm{Pb}}^{2+}\left(\mathrm{aq}\right)\stackrel{ }{\rightleftharpoons }{\mathrm{PbCrO}}_4\left(\mathrm{s}\right)$

What is a heterogeneous equilibrium?

Explain why pure solids and liquids can be ignored while writing the equilibrium constant expression ?

The molar concentration of a pure solid or liquid is constant.

Cotyledons are also called-

The partial pressure of carbon dioxide from the following is :

$\mathrm{C}\mathrm{a}\mathrm{C}{{\mathrm{O}}_3}_{\left(\mathrm{s}\right)}\mathrm{ }\rightleftharpoons \mathrm{ }\mathrm{C}\mathrm{a}{\mathrm{O}}_{\left(\mathrm{s}\right)\mathrm{ }}+\mathrm{ }\mathrm{C}{{\mathrm{O}}_2}_{\left(\mathrm{g}\right)}\mathrm{ };\mathrm{ }{\mathrm{K}}_{\mathrm{p}}=8\mathrm{ }\times \mathrm{ }{10}^{–2}$

Partial pressure of ${\mathrm{O}}_2$ in the reaction

$2\mathrm{A}{\mathrm{g}}_2\mathrm{O}\left(s\right)\rightleftharpoons 4\mathrm{A}\mathrm{g}\left(s\right)+{\mathrm{O}}_2\left(\mathrm{g}\right)$ is

Hot copper turnings can be used as oxygen getter for inert gas supplies by slowly passing the gas over the turnings at 600 K.

$2{\text{Cu}}_{\left(\text{s}\right)}+\frac{1}{2}{\text{O}}_{2\left(\text{g}\right)}\rightleftharpoons {\text{Cu}}_2{\text{O}}_{\left(\text{s}\right)};K_{\text{P}}=\text{7.5}\times 10^{10}{\text{atm}}^{-1/2}$

The number of molecules of O₂ per litre left after equilibrium has reached are :

The dissociation equilibrium pressure of ${\mathrm{NH}}_4\mathrm{HS}\left(\mathrm{s}\right)$ is $60 \mathrm{cm}$ of $\mathrm{Hg}$ at $27°\mathrm{C}$. The total pressure at equilibrium when ${\mathrm{NH}}_4\mathrm{HS}$ is dissociated in the presence of $45 \mathrm{cm}$ of $\mathrm{Hg}$ of ${\mathrm{NH}}_3$ is

K_p for the reaction
${\mathrm{CuSO}}_4·3{\mathrm{H}}_2{\mathrm{O}}_{\left(\mathrm{s}\right)}+2{\mathrm{H}}_2{\mathrm{O}}_{\left(\mathrm{g}\right)}\to {\mathrm{CuSO}}_4·5{\mathrm{H}}_2{\mathrm{O}}_{\left(\mathrm{s}\right)}$   is $1·0\times 10^4 {\text{atm}}^{-2}$  at certain  temperature. What lowest relative humidity of air can be achieved using $CuS{O}_4.3H_{2}O$ as drying agent at that temperature ?
Aqueous tension at the given temperature = 16 torr