Equilibrium Constants (Kp, Kc or Kx)

For the system: $\mathrm{A} \left(\mathrm{g}\right)+2\mathrm{B} \left(\mathrm{g}\right)\to \mathrm{C} \left(\mathrm{g}\right)$, the equilibrium concentration is

$\mathrm{A}=0.06 \mathrm{moles}/\mathrm{l}, \mathrm{B}=0.12 \mathrm{moles}/\mathrm{l}, \mathrm{C}=0.216 \mathrm{moles}/\mathrm{l}$

The ${\mathrm{K}}_{\mathrm{eq}}$ for the reaction is:

The value of ${\mathrm{K}}_{\mathrm{c}}$ for the reaction:

$\mathrm{A}+3\mathrm{B}\rightleftharpoons 2\mathrm{C} \mathrm{at} 400 °\mathrm{C}$ is $0.5 \mathrm{mol} {\mathrm{L}}^{-1}.$ Calculate the value of ${\mathrm{K}}_{\mathrm{P}}$ in $\mathrm{atm}$.

For the reaction $2\mathrm{HI}\left(\mathrm{g}\right)\rightleftharpoons {\mathrm{H}}_2\left(\mathrm{g}\right)+{\mathrm{I}}_2\left(\mathrm{g}\right)$, the degree of dissociation $\left(\mathrm{\alpha }\right)$ of $\mathrm{HI}$ is related to the equilibrium constant ${\mathrm{K}}_{\mathrm{p}}$ by the expression

A reaction, $\mathrm{A}+2\mathrm{B}\rightleftharpoons 2\mathrm{C}+\mathrm{D}$ was studied using the initial concentrations, of which $\mathrm{B}$ was $1.5$ times that of $\mathrm{A}$. The equilibrium concentration of $\mathrm{A}$ and $\mathrm{B}$ were found to be equal. Then ${\mathrm{K}}_{\mathrm{c}}$ for the equilibrium is

Sulphide ions in alkaline solutions react with solid sulphur to form polyvalent sulphide ions. The equilibrium constant for the formation of ${{\mathrm{S}}_2}^{2-}$ and ${{\mathrm{S}}_3}^{2-}$ from $\mathrm{S}$ and${\mathrm{S}}^{2-}$ ions are $1.7$ and $5.3$, respectively. The equilibrium constant for the formation of ${{\mathrm{S}}_3}^{2-}$ from ${{\mathrm{S}}_2}^{2-}$ and $\mathrm{S}$ is

For the reaction equilibrium, $2\mathrm{NOBr}\left(\mathrm{g}\right)\rightleftharpoons 2\mathrm{NO}\left(\mathrm{g}\right)+{\mathrm{Br}}_2\left(\mathrm{g}\right),$ if ${\mathrm{P}}_{{\mathrm{Br}}_2}=\frac{\mathrm{P}}{9}$ at equilibrium and $\mathrm{P}$ is total pressure, then the ratio $\frac{{\mathrm{K}}_{\mathrm{P}}}{\mathrm{P}}$ is equal to: (assume that equilibrium was achieved starting with only $\mathrm{NOBr}$)

${\mathrm{X}}_2+{\mathrm{X}}^{-} \rightleftharpoons {\mathrm{X}}_3^{-} (\mathrm{X}=\mathrm{Iodine})$

This reaction is set up in an aqueous medium. The reaction started with $1 \mathrm{mol}$ of ${\mathrm{X}}_2$ and $0.5 \mathrm{mol}$ of ${\mathrm{X}}^{-}$ in a $1 \mathrm{L}$ flask. After equilibrium is reached, the excess ${\mathrm{AgNO}}_3$ gave $0.25 \mathrm{mol}$ of yellow precipitate. The equilibrium constant is:

At the temperature $\mathrm{T}$, a compound ${\mathrm{AB}}_2 \left(\mathrm{g}\right)$ dissociates, according to the reaction $2{\mathrm{AB}}_2 \left(\mathrm{g}\right)\rightleftharpoons 2\mathrm{AB} \left(\mathrm{g}\right)+{\mathrm{B}}_2 \left(\mathrm{g}\right)$ with a degree of dissociation $\mathrm{x}$, which is small compared with unity. The expression for ${\mathrm{K}}_{\mathrm{p}}$ in terms of $\mathrm{x}$ and the total pressure, $\mathrm{P}$ is

For the equilibrium reaction ${\mathrm{N}}_2{\mathrm{O}}_4\left(\mathrm{g}\right)\rightleftharpoons 2{\mathrm{NO}}_2\left(\mathrm{g}\right)$, the concentrations of ${\mathrm{N}}_2{\mathrm{O}}_4$ and ${\mathrm{NO}}_2$ at equilibrium are $4.8\times {10}^{-2}$ and $1.2\times {10}^{-2} \mathrm{mol} {\mathrm{L}}^{-1}$, respectively. What is the value of ${\mathrm{K}}_{\mathrm{c}}$ for the reaction?

For the reaction: $\mathrm{CO}\left(\mathrm{g}\right)+\frac{1}{2}{\mathrm{O}}_2\left(\mathrm{g}\right)\rightleftharpoons {\mathrm{CO}}_2\left(\mathrm{g}\right), \frac{{\mathrm{K}}_{\mathrm{p}}}{{\mathrm{K}}_{\mathrm{c}}}$ is

$\mathrm{X} +\mathrm{Y}\rightleftharpoons \mathrm{Z}$

If the concentrations of reactants in the given reaction are tripled, then what will be its equilibrium constant?

${\mathrm{PCl}}_5$ is dissociated to $40\%$ at $600 \mathrm{K}$. If ${\mathrm{K}}_{\mathrm{p}}= 2.4$, then what will be the total pressure at equilibrium?

Given that the equilibrium constant for the reaction $2S{O}_{2\left(g\right)}+O_{2\left(g\right)}\rightleftharpoons 2S{O}_{3\left(g\right)}$ has a value of 278 at a particular temperature. What is the value of the equilibrium constant for the following reaction at the same temperature?

$S{O}_{3\left(g\right)}\rightleftharpoons S{O}_{2\left(g\right)}+\frac{1}{2}{O}_{2\left(g\right)}$