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-

The vapour density of a sample ${\mathrm{N}}_2{{\mathrm{O}}_4}_{\left(\mathrm{g}\right)}$ is $40$ at $10 \mathrm{atm}$. Calculate the ${\mathrm{K}}_{\mathrm{P}}$ for the reaction.

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.

Calculate the percentage degree of ionisation of $0.4 \mathrm{M}$ acetic acid in water. Dissociation constant of acetic acid is $1.8\times {10}^{-5}$.

Give your answer by multiplying the value with 1000.

$\mathrm{HI}$ is introduced into three identical $500 \mathrm{mL}$ bulbs at $350°\mathrm{C}$. Each bulb is opened at different time intervals and analysed for ${\mathrm{I}}_2$ by titrating with $0.015 \mathrm{M}$ hypo solution.

$\left({\mathrm{I}}_2+2{\mathrm{Na}}_2{\mathrm{S}}_2{\mathrm{O}}_3\to {\mathrm{Na}}_2{\mathrm{S}}_4{\mathrm{O}}_6+2\mathrm{NaI}\right)$

 ${\mathrm{K}}_{\mathrm{c}}$ for $2\mathrm{HI}\rightleftharpoons {\mathrm{H}}_2+{\mathrm{I}}_2$ at $350°\mathrm{C}$ is $\frac{\mathrm{y}}{2}\times {10}^{-2}$

Express the $\mathrm{y}$ value after rounding off up to nearest integer.

$5$ 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.

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

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?

In an aqueous solution of volume $500 \mathrm{mL},$ when the reaction of $2{\mathrm{Ag}}^{+}+{\mathrm{Cu}}_{\left(\mathrm{s}\right)}\rightleftharpoons {\mathrm{Cu}}^{2+}+2{\mathrm{Ag}}_{\left(\mathrm{s}\right)}$ reached equilibrium the $\left[{\mathrm{Cu}}^{2+}\right]$ was $\mathrm{x}\hspace{0.17em}\mathrm{M}$. When $500 \mathrm{mL}$ of water is further added, at the new equilibrium $\left[{\mathrm{Cu}}^{+2}\right]$ will be :-

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?
$$\begin{gathered} \left[{\mathrm{CH}}_4\right]=1.07 \mathrm{M}, \left[{\mathrm{H}}_2\mathrm{S}\right]=1.20 \mathrm{M}, \\ \left[{\mathrm{CS}}_2\right]=0.90 \mathrm{M} , \left[{\mathrm{H}}_2\right]=1.78 \mathrm{M} \end{gathered}$$

The equilibrium constant for the reaction, $\mathrm{A}+2\mathrm{B}\rightleftharpoons \mathrm{C}+\mathrm{D},$ is $1.0\times {10}^8.$

Calculate the equilibrium concentration of $\mathrm{A}$, if $1.0$ mole of $\mathrm{A}$ and $3.0$ mole of $\mathrm{B}$ are placed in $1\mathrm{L}$ flask and allowed to attain the equilibrium.

The equilibrium constant(K) for the reaction Cyclohexane $\rightleftharpoons$ Hex-1-ene is 10732. At the given condition in a closed one litre vessel 2 moles of cyclohexane are mixed with 2 moles of hex-1-ene then