Factors Affecting Equilibria

For the chemical reaction  $3\mathrm{X}\left(\mathrm{g}\right)+\mathrm{Y}\text{(g)}\rightleftharpoons {\mathrm{X}}_3\mathrm{Y}\left(\mathrm{g}\right)$ , the amount of  $X_{3}Y$ at equilibrium is affected by –

The plot of ${\mathrm{logk}}_{\mathrm{f}}$ versus $\frac{1}{\mathrm{T}}$ for a reversible reaction $\mathrm{A}\left(\mathrm{g}\right)\rightleftharpoons \mathrm{P}\left(\mathrm{g}\right)$ is shown.

Pre-exponential factors for the forward and backward reactions are ${10}^{15} {\mathrm{s}}^{-1}$ and ${10}^{11} {\mathrm{s}}^{-1}$, respectively. If the value of $\mathrm{logK}$ for the reaction at $500 \mathrm{K}$ is $6$, the value of $\left|{\mathrm{logk}}_{\mathrm{b}}\right|$ at $250 \mathrm{K}$ is
$\left[\mathrm{K}=\right.$equilibrium constant of the reaction, ${\mathrm{k}}_{\mathrm{f}}=$rate constant of forward reaction, ${\mathrm{K}}_{\mathrm{b}}=$rate constant of backward reaction]

The equilibrium constant for this reaction ${\mathrm{N}}_2+3{\mathrm{H}}_2\rightleftharpoons 2{\mathrm{NH}}_3$ at $400°\mathrm{C}$ is $1.64\times {10}^{-4}$ and at $500°\mathrm{C}$ is $0.144\times {10}^{-4}$. The mean heat of formation of $1$ mole of ammonia from its elements in the gives range of temp. is

For the reaction, $2\mathrm{A}\left(\mathrm{g}\right)+\mathrm{B}\left(\mathrm{g}\right)\rightleftharpoons 2\mathrm{C}\left(\mathrm{g}\right), \mathrm{\Delta H}=+13.6 \mathrm{kJ}$, which of the following will increase the extent of the reaction at equilibrium?

The thermal dissociation equilibrium reaction of ${\mathrm{CaCO}}_3\left(\mathrm{s}\right)$ is studied under different conditions
${\mathrm{CaCO}}_3\left(\mathrm{s}\right)\rightleftharpoons \mathrm{CaO}\left(\mathrm{s}\right)+{\mathrm{CO}}_2\left(\mathrm{g}\right)$

For this equilibrium reaction, the correct statement(s) is/ (are):

At the equilibrium of the reaction, $2 \mathrm{X} \left(\mathrm{g}\right) + \mathrm{Y} \left(\mathrm{g}\right)\rightleftharpoons {\mathrm{X}}_2\mathrm{Y} \left(\mathrm{g}\right)$, the number of moles of ${\mathrm{X}}_2\mathrm{Y}$ at equilibrium is affected by the

Which of the following reactions will not get affected on increasing the pressure?

Consider the following reaction ${\mathrm{CaCO}}_{3( \mathrm{s})}\rightleftharpoons {\mathrm{CaO}}_{\left(\mathrm{s}\right)}+{\mathrm{CO}}_{2\left(\mathrm{g}\right)}$ in closed container at equilibrium. What would be the effect of addition of ${\mathrm{CaCO}}_3$ on the equilibrium concentration of ${\mathrm{CO}}_2$?

Water freezes at $0°\mathrm{C}$ as ${\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}, \mathrm{d}=1 \mathrm{g}/{\mathrm{cm}}^3\right)\rightleftharpoons \underset{\left(\mathrm{s}, \mathrm{d}=0.92 \mathrm{g}/{\mathrm{cm}}^3\right)}{{\mathrm{H}}_2\mathrm{O}}$

Then by increasing pressure.

On applying pressure to the equilibrium,
$\mathrm{Ice}\rightleftharpoons \mathrm{Water}$
Which phenomenon will happen?

Glauber's salt, ${\mathrm{Na}}_2{\mathrm{SO}}_4·10{\mathrm{H}}_2\mathrm{O}$, was used by J.R.Glauber in the $17\mathrm{th}$ century as a medical agent. At $27°\mathrm{C}$

${\mathrm{Na}}_2{\mathrm{SO}}_4·10{\mathrm{H}}_2\mathrm{O}\left(\mathrm{s}\right)\rightleftharpoons {\mathrm{Na}}_2{\mathrm{SO}}_4\left(\mathrm{s}\right)+10{\mathrm{H}}_2\mathrm{O}\left(\mathrm{g}\right); {\mathrm{K}}_{\mathrm{P}}=4.08\times {10}^{-25}$

Which of the following change will take reaction in forward direction?

What is the effect of adding helium gas (at constant volume) to an equilibrium mixture of the reaction?
$\mathrm{CO}\left(\mathrm{g}\right)+{\mathrm{Cl}}_2\left(\mathrm{g}\right)\rightleftharpoons {\mathrm{COCl}}_2\left(\mathrm{g}\right)$

According to le-Chatelier's principle, adding heat to a solid and liquid in equilibrium will cause the

For a gas phase reaction:
$\mathrm{A}\left(\mathrm{g}\right)+2\mathrm{B}\left(\mathrm{g}\right)\rightleftharpoons \mathrm{C}\left(\mathrm{g}\right)+\mathrm{D}\left(\mathrm{g}\right)$

The backward reaction is favoured

$\left(\mathrm{i}\right)$ By introducing inert gas at constant volume

$\left(\mathrm{ii}\right)$ By introducing inert gas at constant pressure

$\left(\mathrm{iii}\right)$ By adding $\text{'}\mathrm{A}\left(\mathrm{g}\right)\text{'}$ at constant volume

$\left(\mathrm{iv}\right)$ By adding $\text{'}\mathrm{D}\left(\mathrm{g}\right)\text{'}$ at constant volume

The correct statements is/are

For the reaction ${\mathrm{PCl}}_5\left(\mathrm{g}\right)\rightleftharpoons {\mathrm{PCl}}_3\left(\mathrm{g}\right)+{\mathrm{Cl}}_2\left(\mathrm{g}\right)$, the forward reaction of constant temperature is favoured by

(1) Introducing an inert gas at constant volume

(2) Introducing chlorine gas at constant volume

(3) Introducing an inert gas at constant pressure

(4) Introducing ${\mathrm{PCl}}_5$ at constant volume

(5) Introducing ${\mathrm{PCl}}_3$ gas at constant volume

In which of the following reactions, an increase in the volume of the container will favour the formation of product?