Applications of Equilibrium Constant

$5$ 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:

$2\mathrm{A}+\mathrm{B}\rightleftharpoons 3\mathrm{C}, {\mathrm{K}}_{\mathrm{C}}=49$

For the above reaction, $3$ $\mathrm{L}$ vessel contains $2, 1$ and $3$ moles of $\mathrm{A}, \mathrm{B}$ and $\mathrm{C}$ respectively. Then, what will happen to the reaction?

The reaction quotient $\left(\mathrm{Q}\right)$ predicts:

For a reaction $\mathrm{A}\to$ products, the value of equilibrium constant $\text{'}\mathrm{K}\text{'}$, when the reaction reaches completion, would be close to which among the following?

The equilibrium constant for the reaction between ${\mathrm{CH}}_4 \left(\mathrm{g}\right)$ and ${\mathrm{H}}_2\mathrm{S} \left(\mathrm{g}\right)$ to form ${\mathrm{CS}}_2 \left(\mathrm{g}\right)$ and ${\mathrm{H}}_2 \left(\mathrm{g}\right)$, at $1173 \mathrm{K}$ is $3.6$. For the following composition of the reaction mixture, decide which of the following option is correct?
$$\begin{gathered} \left[{\mathrm{CH}}_4\right]=1.07 \mathrm{M}, \left[{\mathrm{H}}_2\mathrm{S}\right]=1.20 \mathrm{M}, \\ \left[{\mathrm{CS}}_2\right]=0.90 \mathrm{M} , \left[{\mathrm{H}}_2\right]=1.78 \mathrm{M} \end{gathered}$$

A mixture of ${\mathrm{NO}}_2$ and ${\mathrm{N}}_2{\mathrm{O}}_4$ has a vapour density of $38.3$ at $300 \mathrm{K}$. What is the number of moles of ${\mathrm{NO}}_2$ in $100 \mathrm{g}$ of the mixture?

The equilibrium constant for the reaction between ${\mathrm{CH}}_4 \left(\mathrm{g}\right)$ and ${\mathrm{H}}_2\mathrm{S} \left(\mathrm{g}\right)$ to form ${\mathrm{CS}}_2 \left(\mathrm{g}\right)$ and ${\mathrm{H}}_2 \left(\mathrm{g}\right)$, at $1173 \mathrm{K}$ is $3.6$. For the following composition of the reaction mixture, decide which of the following option is correct?
$$\begin{gathered} \left[{\mathrm{CH}}_4\right]=1.07 \mathrm{M}, \left[{\mathrm{H}}_2\mathrm{S}\right]=1.20 \mathrm{M}, \\ \left[{\mathrm{CS}}_2\right]=0.90 \mathrm{M} , \left[{\mathrm{H}}_2\right]=1.78 \mathrm{M} \end{gathered}$$

Value of ${\mathrm{K}}_{\mathrm{p}}$ for the reaction ${{\text{SO}}_2}_{\left(\text{g}\right)}+{{\text{NO}}_2}_{\left(\text{g}\right)}\rightleftharpoons {{\text{SO}}_3}_{\left(\text{g}\right)}+{\text{NO}}_{\left(\text{g}\right)}$  is 25 at cartain temperature and 4atm pressure.
Initially if we take 2 moles of each of the four gases and 2 moles of inert gas, what would be the equilibrium partial pressure of SO₂ ? 

Consider the following reaction equilibrium:

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

Initially in $2 \mathrm{L}$ flask $1$ mole of ${\mathrm{N}}_2$ and $3$ mole of ${\mathrm{H}}_2$ are kept. If equilibrium state the number of moles of ${\mathrm{N}}_2 \mathrm{is} 0.6$, then the total number of moles of all gases present in the flask is

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

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

$\mathrm{\alpha }$ is the degree of dissociation, ${\mathrm{P}}_1$, ${\mathrm{T}}_1$, ${\mathrm{P}}_2$ and ${\mathrm{T}}_2$ are the initial pressure, initial temperature, equilibrium pressure and temperature, respectively. What is the value of $\mathrm{\alpha }$ $\left(\mathrm{constant} \mathrm{V}\right)$?

Consider the following equilibrium in a closed container $PC{l}_5\left(g\right)\rightleftharpoons PC{l}_3\left(g\right)+C{l}_2\left(g\right)PC{l}_5$. Gas at a certain pressure is introduced in the container at ${27}^{°}C$. However, the total pressure at equilibrium at ${207}^{°}C$ was found to be double the initial value. The $\%$ dissociation of $PC{l}_5$ at ${207}^{°}C$ is:

For the reaction ${\mathrm{N}}_2{\mathrm{O}}_{4\left(\mathrm{g}\right)}\rightleftharpoons 2{\mathrm{NO}}_{2\left(\mathrm{g}\right)}$, the correct relationship between degree of dissociation $\left(\mathrm{\alpha }\right)$ and equilibrium constant $\left({\mathrm{K}}_{\mathrm{p}}\right)$ is:

$(\mathrm{P}=$equilibrium total pressure$)$

A vessel contains ${\mathrm{H}}_2$ and ${\mathrm{H}}_2\mathrm{S}$ gases at partial pressures of $1$ and $2 \mathrm{atm}$, respectively, at a certain temperature the reaction, $8{\mathrm{H}}_2{\mathrm{S}}^{}\left(\mathrm{g}\right)\rightleftharpoons 8{\mathrm{H}}_2\left(\mathrm{g}\right)+{\mathrm{S}}_8\left(\mathrm{s}\right)$ occurs. It is found that ${\left[\frac{{\mathrm{n}}_{{\mathrm{H}}_2}}{{\mathrm{n}}_{{\mathrm{H}}_2\mathrm{S}}}\right]}_{\mathrm{at}\mathrm{equilibrium}}={\left[\frac{{\mathrm{n}}_{{\mathrm{H}}_2\mathrm{S}}}{{\mathrm{n}}_{{\mathrm{H}}_2}}\right]}_{\mathrm{at}\mathrm{time},\mathrm{t}=0}$  ($\mathrm{n}$ represents no. of moles). Identify the correct value of the given property.

At a certain temperature, 2 moles of $CO$ and 3 moles of $C{l}_2$ were mixed and allowed to reach equilibrium in a $5.0 L$ vessel according to the reaction $C{O}_{\left(g\right)} + C{l}_{2\left(g\right)} \rightleftharpoons COC{l}_{2 \left(g\right)}$.

At equilibrium, if 1 mole of $CO$ is present, then equilibrium constant $\left(K_c\right)$ for the reaction is:

$\underset{\left(S\right)}{MgS{O}_4\cdot 7H_{2}O}\stackrel{}{\rightleftharpoons }\underset{\left(S\right)}{MgS{O}_4.5H_{2}O}+\underset{\left(g\right)}{2H_{2}O}$

The above equilibrium is reached in a closed contained initially having dry inert gases. At equilibrium relative humidity of the mixture is $0.4$. What is $Kp$ if aqueous tension at the same temperature is $50 mm Hg$ ?

${\mathrm{A}}_2{\mathrm{B}}_5$ (gas) decomposes in presence of Helium with total initial pressure of $100 \mathrm{mm} \mathrm{of} \mathrm{Hg}$ in a closed flask. After $50\%$ of ${\mathrm{A}}_2{\mathrm{B}}_5$ decomposed equilibrium is reached with a net pressure of $140 mm of Hg$. What is ${\mathrm{K}}_{\mathrm{p}}$ for ${\mathrm{A}}_2{\mathrm{B}}_5\left(\mathrm{g}\right)\stackrel{}{\rightleftharpoons }{\mathrm{A}}_2\mathrm{B}\left(\mathrm{g}\right)+2{\mathrm{B}}_2\left(\mathrm{g}\right)$

Equilibrium $A_4\left(g\right)\rightleftharpoons 4A\left(g\right)$  is established in a close container. A very tiny pinhole is made and very-very little amount of equilibrium mixture (equilibrium not altered) is effused out, in which mass percentage of atomic A is $40\%$. Hence degree of dissociation of$A_4$ is -