Homogeneous Equilibria

$2S{\mathrm{O}}_{2\left(\mathrm{g}\right)}+{\mathrm{O}}_{2\left(\mathrm{g}\right)}\leftrightharpoons 2\mathrm{S}{\mathrm{O}}_{3\left(\mathrm{g}\right)}$

It is an example of _____ (homogeneous/ heterogeneous) equilibrium?

For a reaction $\mathrm{A}\left(\mathrm{g}\right)\rightleftharpoons \mathrm{B}\left(\mathrm{g}\right)$ at equilibrium, the partial pressure of $\mathrm{B}$ is found to be one-fourth of the particle pressure of $\mathrm{A}$. The value of $\mathrm{\Delta G}°$ of the reaction $\mathrm{A}\to \mathrm{B}$ is

Which of the following is an example of homogeneous equilibrium?

Ratio of ${\mathrm{K}}_{\mathrm{p}}/{\mathrm{K}}_{\mathrm{c}}$ of the reaction $2{\mathrm{SO}}_2 + {\mathrm{O}}_2\rightleftharpoons 2{\mathrm{SO}}_3$ is equal to _____. (write the answer in the form of $\mathrm{a}/\mathrm{b}$).

Explain homogeneous equilibrium with the help of an example.

For the reaction, ${\mathrm{N}}_2{\mathrm{O}}_4\left(\mathrm{g}\right)\rightleftharpoons 2{\mathrm{NO}}_2\left(\mathrm{g}\right)$ the values of ${\mathrm{K}}_{\mathrm{p}}$ and ${\mathrm{K}}_{\mathrm{c}}$ are found to be $85.87 \mathrm{bar}$ and $2.6 \mathrm{mol} {\mathrm{L}}^{-1}$ respectively. Find the temperature at which the reaction is carried out.

For the reaction ${\mathrm{A}}_{\left(\mathrm{g}\right)}+ {\mathrm{B}}_{\left(\mathrm{s}\right)}\leftrightharpoons {\mathrm{C}}_{\left(\mathrm{g}\right)}+{\mathrm{D}}_{\left(\mathrm{g}\right)}$, ${\mathrm{K}}_{\mathrm{c}} = 42 \mathrm{mol} {\mathrm{dm}}^{-3}$ at $120°\mathrm{C}$. Calculate ${\mathrm{K}}_{\mathrm{p}}$

Explain homogeneous equilibrium with the help of an example.

${\mathrm{N}}_2{\mathrm{O}}_4$ is $25\%$ dissociated at ${37}^{°} \mathrm{C}$ and $1\mathrm{atm}$ pressure. Calculate ${\mathrm{K}}_{\mathrm{p}}$ for the reaction, ${\mathrm{N}}_2{\mathrm{O}}_4\left(\mathrm{g}\right)\stackrel{ }{\rightleftharpoons }2{\mathrm{NO}}_2\left(\mathrm{g}\right)$.

Give an example of a reaction, where ${\mathrm{K}}_{\mathrm{p}}={\mathrm{K}}_{\mathrm{c}}$.

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

${\mathrm{CH}}_3\mathrm{COOH}\left(\mathrm{aq}\right)+{\mathrm{CH}}_3\mathrm{OH}\left(\mathrm{aq}\right)\stackrel{ }{\rightleftharpoons }{\mathrm{CH}}_3{\mathrm{COOCH}}_3\left(\mathrm{aq}\right)+{\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right)$

What is a homogeneous equilibrium?

White solid balls of naphthalene $\left({\mathrm{C}}_{10}{\mathrm{H}}_8\right)$ used as moth balls were kept in a closed container at room temperature $({27}^0 \mathrm{C})$. The vapour pressure above the balls was found to be $0.10 \mathrm{mm} \mathrm{Hg}$. 

The value of ${\mathrm{K}}_{\mathrm{c}}$ for the sublimation equilibrium, ${\mathrm{C}}_{10}{\mathrm{H}}_{8 }\left(\mathrm{s}\right)\rightleftharpoons {\mathrm{C}}_{10}{\mathrm{H}}_8 \left(\mathrm{v}\right)$ is

In the following reaction, combustion of hot copper turnings can be used as an oxygen getter for inert gas supplies by slowly passing the gas over the turnings at a temperature of $600 \mathrm{K}$.

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

After equilibrium has reached, how many number of molecules of ${\mathrm{O}}_2$ per litre left?

Consider the equilibrium reaction  ${\mathrm{P}}_4\left(\mathrm{g}\right)\rightleftharpoons 2{\mathrm{P}}_2\left(\mathrm{g}\right)$where ${\mathrm{K}}_{\mathrm{P}} = 4$$atm$at $1325 \mathrm{K}.$In an experiment where ${\mathrm{P}}_4\left(\mathrm{g}\right)$was placed in a container at $1325 \mathrm{K}$, the equilibrium mixture of ${\mathrm{P}}_4\left(\mathrm{g}\right)$ and ${\mathrm{P}}_2\left(\mathrm{g}\right)$ has a total pressure of $1.0 \mathrm{atm}$. The equilibrium partial pressure of${\mathrm{P}}_2\left(\mathrm{g}\right)$ will be

For the following reaction; $2{\mathrm{NO}}_{2\left(\mathrm{g}\right)}\rightleftharpoons 2{\mathrm{NO}}_{\left(\mathrm{g}\right)}+{\mathrm{O}}_{2\left(\mathrm{g}\right)}, {\mathrm{K}}_{\mathrm{c}}=1.8\times {10}^{-6}$ at ${184}^{\mathrm{o}}\mathrm{C}$ and $\mathrm{R}=0.83 \mathrm{L} \mathrm{atm} {\mathrm{K}}^{-1}{\mathrm{mol}}^{-1}$ when ${\mathrm{K}}_{\mathrm{p}}$ and ${\mathrm{K}}_{\mathrm{c}}$ are compared at ${184}^{\mathrm{o}}\mathrm{C}.$ It is found that:

The density of an equilibrium mixture of ${\mathrm{N}}_2{\mathrm{O}}_4$ and ${\mathrm{NO}}_2$ at $1 \mathrm{atm}$  is $3.62 \mathrm{g}/\mathrm{litre}$ at $288 \mathrm{K}$ and $1.84 \mathrm{g}/\mathrm{litre}$ at $348 \mathrm{K}$. Calculate the enthalpy of reaction in calories.

Give an answer to the nearest integer value.