Law of Chemical Equilibrium and Equilibrium Constants

State and explain the law of mass action. Apply it to the following equilibria: ${\mathrm{PCl}}_5\left(\mathrm{s}\right)\rightleftharpoons {\mathrm{PCl}}_3\left(\mathrm{l}\right)+{\mathrm{Cl}}_2\left(\mathrm{g}\right)$.

State and explain the law of mass action. Apply it to the following equilibria: ${\mathrm{NH}}_4\mathrm{HS}\left(\mathrm{s}\right)\rightleftharpoons {\mathrm{NH}}_3\left(\mathrm{g}\right)+{\mathrm{H}}_2\mathrm{S}\left(\mathrm{g}\right)$.

State and explain the law of mass action. Apply it to the following equilibria: ${\mathrm{H}}_2\left(\mathrm{g}\right)+{\mathrm{F}}_2\left(\mathrm{g}\right)\rightleftharpoons 2\mathrm{HF}\left(\mathrm{g}\right)$.

One mole of ${\mathrm{PCl}}_5$ is subjected to heating in a $1 \mathrm{L}$ vessel. The number of moles of ${\mathrm{PCl}}_3$ formed at equilibrium is $0.6$. Calculate the equilibrium constant for the dissociation of ${\mathrm{PCl}}_5$.

Calculate ${\mathrm{K}}_{\mathrm{p}}$ if the partial pressures of reactants and products in the dissociation of $1$ mole of phosphorous pentachloride are $0.3 \mathrm{atm}, 0.4 \mathrm{atm}$, and $0.2 \mathrm{atm}$ respectively.

Give the units of ${\mathrm{K}}_{\mathrm{c}}$ for the formation of $1$ mole of ${\mathrm{NH}}_3$ from its constituents.

Write the equilibrium constant for the dissociation of ${\mathrm{CaCO}}_3$.

Active mass of a solid is taken as _____.

The value of ${\mathrm{K}}_{\mathrm{c}}$ is $64$ at $800 \mathrm{K}$ for the reaction

${{\mathrm{N}}_2}_{\left(\mathrm{g}\right)}+3{{\mathrm{H}}_2}_{\left(\mathrm{g}\right)}\iff 2{{\mathrm{NH}}_3}_{\left(\mathrm{g}\right)}$

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

${{\mathrm{NH}}_3}_{\left(\mathrm{g}\right)}\iff \frac{1}{2}{{\mathrm{N}}_2}_{\left(\mathrm{g}\right)}+\frac{3}{2}{{\mathrm{H}}_2}_{\left(\mathrm{g}\right)}$

The value of${\mathrm{K}}_{\mathrm{c}}$ for the reaction $3\mathrm{A}\to 2\mathrm{B}+2\mathrm{C}$ is $3\times {10}^{-5}$ At a given composition of reaction mixture is $\left[\mathrm{A}\right] =\left[\mathrm{B}\right] =\left[\mathrm{C}\right]=2\times {10}^{-4}\mathrm{M}$. In which direction the reaction will proceed?

What is ${\mathrm{K}}_{\mathrm{a}}, {\mathrm{K}}_{\mathrm{b}}, {\mathrm{K}}_{\mathrm{w}}$?

For which of the following reaction, the degree of dissociation $\left(\mathrm{\alpha }\right)$ and equilibrium constant $({\mathrm{K}}_{\mathrm{p}})$ are related as ${\mathrm{K}}_{\mathrm{p}}=\frac{4{\mathrm{\alpha }}^2\mathrm{P}}{(1-{\mathrm{\alpha }}^2)}?$

Which of the following is irreversible reaction?

The value of ${\mathrm{K}}_{\mathrm{c}} = 4.24$ at $800 \mathrm{K}$ for the reaction,

${\mathrm{CO}}_{\left(\mathrm{g}\right)} + {\mathrm{H}}_2{\mathrm{O}}_{ \left(\mathrm{g}\right) }$$\to {\mathrm{CO}}_{2\left(\mathrm{g}\right)} + {\mathrm{H}}_{2\left(\mathrm{g}\right)}$

Calculate equilibrium concentrations of ${\mathrm{CO}}_2, {\mathrm{H}}_2, \mathrm{CO} \mathrm{and} {\mathrm{H}}_2\mathrm{O} \mathrm{at} 800 \mathrm{K}$, if only $\mathrm{CO} \mathrm{and} {\mathrm{H}}_2\mathrm{O}$ are present initially at concentration of $0.10 \mathrm{M}$ each ?

$0.1$ mole of ${\mathrm{N}}_2{\mathrm{O}}_4\left(\mathrm{g}\right)$ was sealed in a tube under one atmospheric conditions at ${25}^{\circ }\mathrm{C}$. Calculate the number of moles of ${\mathrm{NO}}_2\left(\mathrm{g}\right)$ present, if the equilibrium 

${\mathrm{N}}_2{\mathrm{O}}_4\left(\mathrm{g}\right)\leftrightharpoons 2{\mathrm{NO}}_2\left(\mathrm{g}\right) \left({\mathrm{K}}_{\mathrm{p}}=0.14\right)$ is reached after some time.

In a reversible gaseous system, molar concentrations (active masses) of reactants or products are proportional to:

The equilibrium constant for the reaction ${\mathrm{H}}_2{\mathrm{O}}_{\left(\mathrm{l}\right)}+{\mathrm{CO}}_{\left(\mathrm{g}\right)}\leftrightharpoons {{\mathrm{H}}_2}_{\left(\mathrm{g}\right)}+{{\mathrm{CO}}_2}_{\left(\mathrm{g}\right)}$ is $64$. If the rate constant for the forward reaction is $160$, the rate constant for the backward reaction is 

From equation (i) and (ii)

$$\begin{gathered} {\mathrm{CO}}_2\left(\mathrm{g}\right)\leftrightharpoons \mathrm{CO}\left(\mathrm{g}\right)+\frac{1}{2}{\mathrm{O}}_{2 }\left(\mathrm{g}\right)\left[{\mathrm{K}}_{{\mathrm{C}}_1}=9.0\times {10}^{-12} \mathrm{at} {1000}^{\circ }\mathrm{C}\right]---\left(\mathrm{i}\right) \\ {\mathrm{H}}_2\mathrm{O}\left(\mathrm{g}\right)\leftrightharpoons {\mathrm{H}}_2\left(\mathrm{g}\right)+\frac{1}{2}{\mathrm{O}}_{2 }\left(\mathrm{g}\right)\left[{\mathrm{K}}_{{\mathrm{C}}_2}=7.0\times {10}^{-12} \mathrm{at} {1000}^{\circ }\mathrm{C}\right]---\left(\mathrm{ii}\right) \end{gathered}$$

The equilibrium constant for the following reaction

${\mathrm{CO}}_2+{\mathrm{H}}_2\rightleftharpoons \mathrm{CO}+{\mathrm{H}}_2\mathrm{O}$

at the same temperature is 

The equilibrium constant for the reaction, ${\mathrm{H}}_2\mathrm{O}\left(\mathrm{g}\right)+\mathrm{CO}\left(\mathrm{g}\right)\rightleftharpoons {\mathrm{H}}_2\left(\mathrm{g}\right)+{\mathrm{CO}}_2\left(\mathrm{g}\right)$ is $64$. If the rate constant for the forward reaction is $160$, the rate constant for the backward reaction is :

Define the following:
 Law of mass action.