Law of Chemical Equilibrium and Equilibrium Constants

 An expression for the backward rate constant of the reaction, $\mathrm{aA}+\mathrm{bB}\stackrel{ }{\rightleftharpoons }\mathrm{cC}+\mathrm{dD}$ is

The reaction $\mathrm{A} \left(\mathrm{g}\right)+\mathrm{B} \left(\mathrm{g}\right)\rightleftharpoons \mathrm{C} \left(\mathrm{g}\right)+\mathrm{D} \left(\mathrm{g}\right)$ is elementary $2^{\mathrm{nd}}$ order reaction opposed by elementary secondary order reaction. When started with equimolar amounts of $\mathrm{A}$ and $\mathrm{B},$ at equilibrium, it is found that the concentration of $\mathrm{A}$ is twice that of $\mathrm{C} .$ Specific rate constant for forward reaction is $2\times {10}^{-3}{\mathrm{mol}}^{-1}{\mathrm{Lsec}}^{-1}.$ The specific rate constant for backward reaction is

For the reaction, $2\mathrm{S}{\mathrm{O}}_{2\left(\mathrm{g}\right)}+{\mathrm{O}}_{2\left(\mathrm{g}\right)}\leftrightharpoons 2\mathrm{S}{\mathrm{O}}_{3\left(\mathrm{g}\right)}$
What is ${\mathrm{K}}_{\mathrm{c}}$ when the equilibrium concentration of $\left[\mathrm{S}{\mathrm{O}}_2\right]=0.60\mathrm{M}, \left[{\mathrm{O}}_2\right]=0.82\mathrm{M}$ and $\left[\mathrm{S}{\mathrm{O}}_3\right]=1.90\mathrm{M}$?

The reaction

${\mathrm{CaCO}}_3\left(\mathrm{s}\right)\rightleftharpoons \mathrm{CaO}\left(\mathrm{s}\right)+{\mathrm{CO}}_2\left(\mathrm{g}\right)$

is in equilibrium in a closed vessel at $298 \mathrm{K}.$ The partial pressure (in atm) of ${\mathrm{CO}}_2\left(\mathrm{g}\right)$ in the reaction vessel is closest to:

[Given: The change in Gibbs energies of formation at $298 \mathrm{K}$ and $1$ bar for

$\mathrm{CaO}\left(\mathrm{s}\right)=-603.501 \mathrm{kJ} {\mathrm{mol}}^{-1}$

${\mathrm{CO}}_2\left(\mathrm{g}\right)=-394.389 \mathrm{kJ} {\mathrm{mol}}^{-1}$

${\mathrm{CaCO}}_3\left(\mathrm{s}\right)=-1128.79 \mathrm{kJ} {\mathrm{mol}}^{-1}$

Gas constant $\mathrm{R}=8.314 \mathrm{J} {\mathrm{K}}^{-1} {\mathrm{mol}}^{-1}$]

Calculate ${\mathrm{K}}_{\mathrm{c}}$ for the reaction, ${\mathrm{SO}}_2\left(\mathrm{g}\right)+\frac{1}{2}{\mathrm{O}}_2\left(\mathrm{g}\right)\rightleftharpoons {\mathrm{SO}}_3\left(\mathrm{g}\right)$

Given $: 2 \mathrm{NO}\left(\mathrm{g}\right)+{\mathrm{O}}_2\left(\mathrm{g}\right)\rightleftharpoons 2 {\mathrm{NO}}_2\left(\mathrm{g}\right), {\mathrm{K}}_{{\mathrm{c}}_1}=144$

$\mathrm{NO}\left(\mathrm{g}\right)+{\mathrm{SO}}_3\left(\mathrm{g}\right)\rightleftharpoons {\mathrm{NO}}_2\left(\mathrm{g}\right)+{\mathrm{SO}}_2\left(\mathrm{g}\right), {\mathrm{K}}_{{\mathrm{c}}_2}=3$

Given
$\mathrm{HF}+{\mathrm{H}}_2\mathrm{O}⟶{\mathrm{H}}_3{\mathrm{O}}^{+}+{\mathrm{F}}^{-}$
${\mathrm{F}}^{-}+{\mathrm{H}}_2\mathrm{O}⟶\mathrm{HF}+{\mathrm{OH}}^{-}$
Which relation is correct?

Find the number of reaction which will be favoured in backward direction:

$\left(\mathrm{A}\right)\mathrm{EtOH}+\mathrm{KOH}\rightleftharpoons \mathrm{EtOK}+{\mathrm{H}}_2\mathrm{O}$

$\left(\mathrm{B}\right)$

$\left(\mathrm{C}\right)$

$\left(\mathrm{D}\right)$

Active mass of $2$ mole pure water:

In which case does the reaction goes farthest to completion :

The mass ratio of steam and ${\mathrm{H}}_2$ gas at equilibrium is $1:2$. The value of equilibrium constant is : $3{\mathrm{Fe}}_{\left(s\right)}+4{\mathrm{H}}_2{\mathrm{O}}_{\left(\mathrm{g}\right)}\rightleftharpoons {\mathrm{Fe}}_3{\mathrm{O}}_{4( \mathrm{s})}+4{\mathrm{H}}_{2( \mathrm{g})}$

Consider the equilibrium ${\mathrm{CO}}_{2\left(\mathrm{g}\right)}\rightleftharpoons {\mathrm{CO}}_{\left(\mathrm{g}\right)}+\frac{1}{2}{\mathrm{O}}_{2\left(\mathrm{g}\right)}$ .The equilibrium constant $\mathrm{K}$ is given by (when $\mathrm{\alpha }<<1)$

At constant temperature and $1$ atm pressure, ${\mathrm{PCl}}_5$ dissociate $2\%$ then at what pressure ${\mathrm{PCl}}_5$ dissociate $4\%$ :-
(Use ${\mathrm{PCl}}_5( \mathrm{g})\rightleftharpoons {\mathrm{PCl}}_3( \mathrm{g})+{\mathrm{Cl}}_2( \mathrm{g})$)

For gaseous reactions values of equilibrium constants are given:

$2\mathrm{NO}+{\mathrm{O}}_2\rightleftharpoons 2{\mathrm{NO}}_2;{\mathrm{K}}_1$

${\mathrm{NO}}_2+{\mathrm{SO}}_2\rightleftharpoons {\mathrm{SO}}_3+\mathrm{NO};{\mathrm{K}}_2$

$2{\mathrm{SO}}_3\rightleftharpoons 2{\mathrm{SO}}_2+{\mathrm{O}}_2;{\mathrm{K}}_3$

The correct relation is:-

The equilibrium constant expression for a gaseous reaction is:-

${\mathrm{K}}_{\mathrm{c}}=\frac{{\left[{\mathrm{NH}}_3\right]}^4{\left[{\mathrm{O}}_2\right]}^5}{[\mathrm{NO}{]}^4{\left[{\mathrm{H}}_2\mathrm{O}\right]}^6}$

The correct reaction would be :-

$2{\mathrm{ICl}}_{\left(\mathrm{g}\right)}\rightleftharpoons {\mathrm{I}}_{2\left(\mathrm{g}\right)}+{\mathrm{Cl}}_{2\left(\mathrm{g}\right)};{\mathrm{K}}_{\mathrm{C}}=2.5\times {10}^{-5}$ Initial concentration of $\mathrm{ICl}$ is $0.1 \mathrm{M}$. What will be the equilibrium concentration of ${\mathrm{Cl}}_2$?

Select the correct graph for rate versus time. $({\mathrm{r}}_{\mathrm{f}}=$ rate of forward reaction and ${\mathrm{r}}_{\mathrm{b}}=$ rate of backward reaction)

Consider the following equilibrium :

${\mathrm{CaCO}}_3\left(\mathrm{s}\right)\rightleftharpoons \mathrm{CaO}\left(\mathrm{s}\right)+{\mathrm{CO}}_2\left(\mathrm{g}\right)$

Find the approximate value of ${\mathrm{K}}_{\mathrm{c}}$ for the given equilibrium reaction, when $2$ moles of ${\mathrm{SO}}_2$ and $1$ mole of ${\mathrm{O}}_2$ are allowed to react in a container of capacity $2 \mathrm{L}$ and the following equilibrium is established:

$2{\mathrm{SO}}_2\left(\mathrm{g}\right)+{\mathrm{O}}_2\left(\mathrm{g}\right)\rightleftharpoons 2{\mathrm{SO}}_3\left(\mathrm{g}\right)$, given that the equilibrium mixture requires $200 \mathrm{mL}$ of $0.1 \mathrm{M}$ acidified ${\mathrm{K}}_2{\mathrm{Cr}}_2{\mathrm{O}}_7$ solution.

At $550 \mathrm{K},$ the ${\mathrm{K}}_{\mathrm{c}}$ for the following reaction is ${10}^4 \mathrm{mol} {\mathrm{L}}^{-1}$

$\mathrm{X}\left(\mathrm{g}\right)+\mathrm{Y}\left(\mathrm{g}\right)\rightleftharpoons \mathrm{Z}\left(\mathrm{g}\right)$

At equilibrium, it was observed that:

$\left[\mathrm{X}\right]=\frac{1}{2}\left[\mathrm{Y}\right]=\frac{1}{2}\left[\mathrm{Z}\right]$ 

Find the value of $\left[\mathrm{Z}\right]$ at equilibrium.

A one-litre vessel containing $0.015 \mathrm{moles} \mathrm{of} {\mathrm{N}}_{2\left(\mathrm{g}\right)}$ and $0.02 \mathrm{moles} \mathrm{of} {\mathrm{PCl}}_{5\left(\mathrm{g}\right)}$ are heated at $227^{\circ }\text{C}$, where the total pressure was found to be $1.843 \mathrm{atm}$. Assuming nitrogen to be inert, determine ${\mathrm{K}}_{\mathrm{p}}$ for the following decomposition reaction:

${\mathrm{PCl}}_{5\left(\mathrm{g}\right)}\rightleftharpoons {\mathrm{PCl}}_{3\left(\mathrm{g}\right)}+{\mathrm{Cl}}_{2\left(\mathrm{g}\right)}$

(Put your answer by multiplying with $100$ and round off to the nearest integer)

What will be the value of active mass taken for solids?