Applications of Equilibrium Constant

$240 \mathrm{ml}, 0.1\mathrm{M}$ solution of weak acid ${\mathrm{H}}_{\mathrm{A}}$, is mixed with $0.2\mathrm{M} \mathrm{NaOH}$. Calculate the volume of $\mathrm{NaOH}$ in ml required when $\mathrm{pH}$ of solution is $5.4$.

$({\mathrm{K}}_{\mathrm{a}} \mathrm{of} {\mathrm{H}}_{\mathrm{A}} \mathrm{is} 2\mathrm{x}{{10}^{-}}^6,{\log }_2=0.3)$

$\mathrm{A}\left(\mathrm{g}\right)\rightleftharpoons 2 \mathrm{B}( \mathrm{g})+\mathrm{C}\left(\mathrm{g}\right)$

For the given reaction, if the initial pressure is $450 \mathrm{mmHg}$ and the pressure at time $\mathrm{t}$ is $720 \mathrm{mmHg}$ at a constant temperature$\mathrm{T}$ and constant volume $\mathrm{V}$. The fraction of $\mathrm{A}\left(\mathrm{g}\right)$ decomposed under these conditions is $\mathrm{x}\times {10}^{-1}$. The value of $\mathrm{x}$ is (nearest integer)

Carbonic acid $\left({\mathrm{H}}_2{\mathrm{CO}}_3\right)$, a diprotic acid has ${\mathrm{K}}_{{\mathrm{a}}_1}=4.0\times {10}^{-7} \mathrm{and} {\mathrm{K}}_{{\mathrm{a}}_2}=7.0\times {10}^{-11}$. What is the $\left[{{\mathrm{CO}}_3}^{2-}\right]$ of a $0.025 \mathrm{M}$ solution of carbonic acid?

${\mathrm{X}}_2+{\mathrm{Y}}_2\rightleftharpoons 2\mathrm{XY}$ reaction was studied at a certain temperature. In the beginning $1 \mathrm{mole}$ of ${\mathrm{X}}_2$​ was taken in a one litre flask and $2 \mathrm{moles}$ of ${\mathrm{Y}}_2$was taken in another $2 \mathrm{litre}$ flask. What is the equilibrium concentration of ${\mathrm{X}}_2$​ and ${\mathrm{Y}}_2$​, respectively?(Given equilibrium concentration of $\left[\mathrm{XY}\right]=0.6{\mathrm{molL}}^{\mathbf{-}\mathbf{1}}$)

For a chemical reaction $\mathrm{A}+\mathrm{B}\to$products, the order is one with respect to each A and B. The sum of x and y from the following data is

The equilibrium constant for the reaction

 ${\mathrm{CO}}_{\left(\mathrm{g}\right)}+{\mathrm{H}}_2{\mathrm{O}}_{\left(\mathrm{g}\right)}\iff {\mathrm{CO}}_{2\left(\mathrm{g}\right)}+{\mathrm{H}}_{2\left(\mathrm{g}\right)}$ is $4.0$ at $1000\mathrm{K}$. When equimolar mixtures of $\mathrm{CO} \mathrm{and} {\mathrm{H}}_2\mathrm{O}$ are heated to $1000\mathrm{K}$ the percentage of ${\mathrm{CO}}_2$ formed at equilibrium is 

In a ten litre container $92 \mathrm{gram}$ of ${\mathrm{N}}_2{\mathrm{O}}_4$ is taken when it is heated up to $327° \mathrm{C}, 25\%$ of ${\mathrm{N}}_2{\mathrm{O}}_4$ is dissociated at equilibrium into ${\mathrm{NO}}_2$. Calculate total pressure inside the container. .

$102 \mathrm{g}$ of solid ${\mathrm{NH}}_4\mathrm{HS}$ is taken in the $2 \mathrm{L}$ evacuated flask at $57°\mathrm{C}$. Following two equilibrium exist simultaneously.

$$\begin{gathered} {\mathrm{NH}}_4\mathrm{HS}\left(\mathrm{s}\right) \rightleftharpoons {\mathrm{NH}}_3\left(\mathrm{g}\right) + {\mathrm{H}}_2\mathrm{S}\left(\mathrm{g}\right) \\ {\mathrm{NH}}_3\left(\mathrm{g}\right) \rightleftharpoons \frac{1}{2}{\mathrm{N}}_2\left(\mathrm{g}\right) + \frac{3}{2}{\mathrm{H}}_2\left(\mathrm{g}\right) \end{gathered}$$

One mole of the solid decomposes to maintain both the equilibrium and $0.75 \mathrm{mol}$ of ${\mathrm{H}}_2$ was found at the equilibrium then find the equilibrium concentration of all the species and ${\mathrm{K}}_{\mathrm{c}}$ for both the reaction.

The equilibrium constant ${\mathrm{K}}_{\mathrm{C}}$ of the following reaction is $9$ at a temperature $\mathrm{T}$.

$\mathrm{A}\left(\mathrm{g}\right)+\mathrm{B}\left(\mathrm{g}\right)\rightleftharpoons \mathrm{C}\left(\mathrm{g}\right)+\mathrm{D}\left(\mathrm{g}\right)$

Assuming that the initial concentration of all the gases is $1$ mole, what will be the concentration of $\mathrm{A}$ and $\mathrm{C}$, respectively, at equilibrium?

Some of the reactions and their equilibrium constants ${\mathrm{K}}_{\mathrm{c}}$ are given. Choose the reaction which proceeds rarely at the given temperature.

${\mathrm{NH}}_4\mathrm{HS}\left(\mathrm{s}\right) \rightleftharpoons {\mathrm{NH}}_3\left(\mathrm{g}\right) + {\mathrm{H}}_2\mathrm{S}\left(\mathrm{g}\right); \mathrm{Kp} = 1200 \mathrm{torr}². \mathrm{In} \mathrm{a} \mathrm{vessel} {\mathrm{NH}}_3\left(\mathrm{g}\right) \mathrm{and} {\mathrm{H}}_2\mathrm{S}\left(\mathrm{g}\right)$ are mixed at partial pressure of 50 torr and 20 torr respectively. After a long time, the total pressure in vessel will be?

Write any three applications of equilibrium constant ${\mathrm{K}}_{\mathrm{c}}$ or ${\mathrm{K}}_{\mathrm{p}}$.

What happens to equilibrium when the temperature is increased ?

What is an equilibrium mixture?

What happens when ${\mathrm{K}}_{\mathrm{c}}$ is very large?

How can we predict the extent of the reaction from the ${\mathrm{K}}_{\mathrm{c}}$ values ?

How will you find the direction of reaction on the basis of the value of reaction quotient $\left({\mathrm{Q}}_{\mathrm{c}}\right)$ and equilibrium constant $\left({\mathrm{K}}_{\mathrm{c}}\right)$?

What factors help in determining the direction of a reaction?

Why is water ignored in equilibrium constant ?