Equilibrium Constants and its Significance

What is the equilibrium expression for the reaction,  ${\text{P}}_{\text{4}}{\text{(s) + 5O}}_{\text{2}}\text{(g) }\underset{}{\rightleftharpoons }{\text{ P}}_{\text{4}}{\text{O}}_{\text{10}}\text{(s) ?}$

At $27°\mathrm{C}$, $1 \mathrm{mol}$ of ${\mathrm{N}}_2{\mathrm{O}}_4\left(\mathrm{g}\right)$ placed in a container of volume $8.21 \mathrm{L}$, no dissociation takes place at this temperature. When the gas heated to $127°\mathrm{C}$, it is partially dissociated to ${\mathrm{NO}}_2\left(\mathrm{g}\right)$ and final pressure found to be $4.5 \mathrm{atm}$. Select the correct statement.

${\mathrm{COF}}_2$ gas passed over a catalyst at $1000 °\mathrm{C}$ comes to equilibrium:

$2{\mathrm{COF}}_2 \left(\mathrm{g}\right)\rightleftharpoons {\mathrm{CO}}_2 \left(\mathrm{g}\right)+{\mathrm{CF}}_4 \left(\mathrm{g}\right)$

Analysis of the equilibrium mixture (after quick cooling to freeze the equilibrium) shows that $500 \mathrm{mL}$ of the equilibrium mixture $\left(\mathrm{NTP}\right)$ contains $300 \mathrm{mL}$ $\left(\mathrm{NTP}\right)$ of ${\mathrm{COF}}_2$ and ${\mathrm{CO}}_2.$ Taking the total pressure to be $10 \mathrm{atm},$ calculate ${\mathrm{K}}_{\mathrm{p}}$.

The freezing point of an aqueous saturated solution of ${\mathrm{I}}_2$ is $-0.0024 °C$. More than this can dissolve in a $\mathrm{KI}$ solution because of the following equilibrium
${\mathrm{I}}_{2\left(\mathrm{aq}\right)} + {{\mathrm{I}}^{-}}_{\left(\mathrm{aq}\right)} \rightleftharpoons {\mathrm{I}}_{3\left(\mathrm{aq}\right)}^{-}$
0.1 M KI solution dissolves $12.5 \mathrm{g} {\mathrm{L}}^{-1} \mathrm{of} {\mathrm{I}}_2$. Calculate the equilibrium constant ${\mathrm{K}}_{\mathrm{c}}$ for the above equilibrium. Assume molarity to be equal to molality and also assume that concentration of I in all saturated solutions is same. (${\mathrm{K}}_{\mathrm{f}}$ of water is $1.86 \mathrm{K} {\mathrm{molal}}^{-1}$, Molecular weight of ${\mathrm{I}}_2 = 253.8 \mathrm{g}/\mathrm{mol}$ ) (Give answer upto nearest integer value.) 

If one-third of $\mathrm{HI}$ decomposes at a particular temperature, the value of equilibrium constant $\left({\mathrm{K}}_{\mathrm{c}}\right)$ for $2\mathrm{HI}\rightleftharpoons {\mathrm{H}}_2+{\mathrm{I}}_2$ is

A $1 \mathrm{L}$ vessel contains $2 \mathrm{mol}$ each of gases $\mathrm{A}, \mathrm{B}, \mathrm{C}$ and $\mathrm{D}$ at equilibrium. If $1 \mathrm{mol}$ each of $\mathrm{A}$ and $\mathrm{B}$ are removed, ${\mathrm{K}}_{\mathrm{c}}$ for $\mathrm{A}+\mathrm{B}\rightleftharpoons \mathrm{C}+\mathrm{D}$ will be

If the equilibrium constants of the following equilibriums ${\mathrm{SO}}_2+\frac{1}{2}{\mathrm{O}}_2\rightleftharpoons {\mathrm{SO}}_3$ and $2{\mathrm{SO}}_3\rightleftharpoons 2{\mathrm{SO}}_2+{\mathrm{O}}_2$ are given by ${\mathrm{K}}_1$ and ${\mathrm{K}}_2$, respectively, which of the following relations is correct?

For a reaction $\mathrm{N}{\mathrm{H}}_4\mathrm{C}\mathrm{O}\mathrm{O}\mathrm{N}{\mathrm{H}}_{2\left(\mathrm{s}\right)}\leftrightharpoons 2\mathrm{N}{\mathrm{H}}_{3\left(\mathrm{g}\right)}+\mathrm{C}{\mathrm{O}}_{2\left(\mathrm{g}\right)}$, the equilibrium pressure is $3 \mathrm{a}\mathrm{t}\mathrm{m}$. ${\mathrm{K}}_{\mathrm{p}}$ for the reaction will be _____${\mathrm{atm}}^3$.

$0.1 \mathrm{mole}$ of each of ethyl alcohol and acetic acid are allowed to react and at equilibrium, the acid was exactly neutralised by $100 \mathrm{mL}$ of $0.85 \mathrm{N}$ $\mathrm{NaOH}$. If no hydrolysis of an ester is supposed to have undergone, the equilibrium constant is $\mathrm{y}\times {10}^{-3}$. Calculate the value of y?

An air sample containing $21:79$ of ${\mathrm{O}}_2$ and ${\mathrm{N}}_2$ (mole ratio) is heated to $2400°\mathrm{C}$. If the mole percent of $\mathrm{NO}$ at equilibrium is $1.8\%,$ calculate ${\mathrm{K}}_{\mathrm{p}}$ for the reaction ${\mathrm{N}}_2+{\mathrm{O}}_2\rightleftharpoons 2\mathrm{NO}.$

Give your answer after multiplying by ${10}^5$ and round off up to nearest integer.