Application of Equilibrium Constant

When two reactants, A and B are mixed to give products C and D, the reaction quotient $\mathrm{Q}$, at the initial stage of the reaction :–

When two reactants A and B are mixed to give products C and D, the reaction quotient Q at the initial stage of the reaction is best described by-

${\mathrm{COCl}}_2$ gas dissociates according to the equation, $\mathrm{COC}{\mathrm{l}}_2\underset{}{\rightleftharpoons }\mathrm{CO}\left(\mathrm{g}\right)+{\mathrm{Cl}}_2\left(\mathrm{g}\right)$. When heated to $700 \mathrm{K}$ the density of the gas mixture at $1.16 \mathrm{atm}$ and at equilibrium is $1.16 \mathrm{g}/\mathrm{litre}$. The degree of dissociation of ${\mathrm{CO}}_2$ at $700 \mathrm{K}$ is

When the reaction $\mathrm{A}+2\mathrm{B}\rightleftharpoons 2\mathrm{C}+\mathrm{D}$ was studied, it was observed that the initial concentration of $\mathrm{B}$ was $1.5$ times that of $\mathrm{A},$ and the equilibrium concentrations of $\mathrm{A}$ and $\mathrm{C}$ were equal. Then ${\mathrm{K}}_{\mathrm{c}}$ for the given equilibrium equals

Identify the correct expression for the equilibrium constant of the following reaction:
$2{\mathrm{X}}_{\left(\mathrm{g}\right)}+{\mathrm{Y}}_{\left(\mathrm{g}\right)}\rightleftharpoons 3{\mathrm{Z}}_{\left(\mathrm{g}\right)}$

Predict the extent of a reaction, ${\mathrm{N}}_2\left(\mathrm{g}\right)+{\mathrm{O}}_2\left(\mathrm{g}\right)\rightleftharpoons 2\mathrm{NO}\left(\mathrm{g}\right)$ at $298 \mathrm{K}$ has $\mathrm{Kc}=4.8\times {10}^{-31}$.

${\mathrm{N}}_2{\mathrm{O}}_4\left(\mathrm{g}\right)\rightleftharpoons 2{\mathrm{NO}}_2\left(\mathrm{g}\right); \mathrm{Kc}=5.7\times {10}^{-9}$ at $298 \mathrm{K}$. At equilibrium

If $\mathrm{Kc}$ is very large 

Explain the classification of chemical equilibrium based on the extent of completion.

A sample of pure ${\mathrm{PCl}}_5$ was introduced into an evacuated vessel at $473 \mathrm{K}$. After equilibrium was attained, the concentration of ${\mathrm{PCl}}_5$ was found to be $0.05 \mathrm{mol} {\mathrm{L}}^{-1}$. If the value of ${\mathrm{K}}_{\mathrm{c}}$ is $8.3\times {10}^{-3}$, what is the concentrations of ${\mathrm{Cl}}_2$ at equilibrium?

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

The equilibrium:

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

is allowed  to set-up at $127°\mathrm{C}$ in a closed vessel. The total pressure at equilibrium was $20 \mathrm{atm}$. The ${\mathrm{K}}_{\mathrm{c}}$ for the reaction is

In an aqueous solution of volume $500 \mathrm{mL}$, when the reaction of $2{\text{Ag}}^{+}+\text{Cu}\rightleftharpoons {\text{Cu}}^{2+}+2\text{Ag}$ is reached equilibrium the $\left[{\mathrm{Cu}}^{2+}\right]$, was $\mathrm{x} \mathrm{M}$. When $500 \mathrm{mL}$ of water is further added, at the equilibrium $\left[{\mathrm{Cu}}^{2+}\right]$ will be

The degree of dissociation is $0.4 \text{at} 420 \mathrm{K} \text{and} 1.0 \mathrm{atm}$ for the gaseous reaction

${\mathrm{PCl}}_5\left(\mathrm{g}\right)⟶{\mathrm{PCl}}_3\left(\mathrm{g}\right)+{\mathrm{Cl}}_2\left(\mathrm{g}\right)$

Assuming ideal behaviour of all gases, calculate the density of equilibrium mixture of equilibrium mixture at $420 \mathrm{K} \text{and} 1.0 \mathrm{atm}. (\mathrm{P} = 31, \mathrm{Cl} = 35.5)$

$40\%$ of a mixture of $2$ moles of ${\mathrm{N}}_2$ and $6$ moles of ${\mathrm{H}}_2$ react to give ${\mathrm{NH}}_3$ according to the equation ${\mathrm{N}}_2 \left(\mathrm{g}\right)+3{\mathrm{H}}_2 \left(\mathrm{g}\right)\rightleftharpoons 2{\mathrm{NH}}_3 \left(\mathrm{g}\right)$ at constant temperature and pressure. Then the ratio of the final volume to the initial volume of gases are

The degree of dissociation of acetic acid in a $0.1 \mathrm{N}$ solution is $1.32\times {10}^{-2}$. At what concentration of nitrous acid will its degree of dissociation be the same as that of acetic acid?

${\mathrm{K}}_{\mathrm{a}} \mathrm{for} {\mathrm{HNO}}_2 = 4 \times {10}^{-4}$

(Report your answer by multiplying the value with 10)

At what concentration of the solution will the degree of dissociation of nitrous acid be $0.2$?

 (${\mathrm{K}}_{\mathrm{a}}$ for ${\mathrm{HNO}}_2$ is $4\times {10}^{-4}$)

Report the value by multiplying with 1000 and rounding off to one significant figure.

$5$ moles of ${\mathrm{S}\mathrm{O}}_2$ and $5$ moles of ${\mathrm{O}}_2$ react in a closed vessel. At equilibrium $60\mathrm{\%}$ of the ${\mathrm{S}\mathrm{O}}_2$ is consumed. The total number of gaseous moles $(\mathrm{S}{\mathrm{O}}_2, {\mathrm{O}}_2\mathrm{ }\mathrm{a}\mathrm{n}\mathrm{d}\mathrm{ }\mathrm{S}{\mathrm{O}}_3)$ in the vessel is:

$0.6$ mole of ${\mathrm{P}\mathrm{C}\mathrm{l}}_5,\mathrm{ }0.3$ mole of ${\mathrm{P}\mathrm{C}\mathrm{l}}_3$ and $0.5$ mole of ${\mathrm{C}\mathrm{l}}_2$ are taken in a $1\mathrm{L}$ flask to obtain the following equilibrium:
$\mathrm{P}\mathrm{C}{\mathrm{l}}_{5\left(\mathrm{g}\right)}\leftrightharpoons \mathrm{P}\mathrm{C}{\mathrm{l}}_{3\left(\mathrm{g}\right)}+\mathrm{C}{\mathrm{l}}_{2\left(\mathrm{g}\right)}$
If the equilibrium constant ${\mathrm{K}}_{\mathrm{c}}$ for the reaction is $0.2$. Predict the direction of the reaction.

Explain the classification of chemical equilibrium on the basis of extent of completion.