Factors Affecting Equilibrium

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 :–

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 –

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-

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

$0.6$ 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.

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 ${\mathrm{CO}}_2$?

For the following reversible reaction,

${\mathrm{N}}_2\left(\mathrm{g}\right)+3{\mathrm{H}}_2\left(\mathrm{g}\right)\leftrightharpoons 2{\mathrm{NH}}_3\left(\mathrm{g}\right); {\mathrm{\Delta H}}_{\mathrm{f}}=-92 \mathrm{kJ}/\mathrm{mol}.$

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

What would happen to a reversible dissociation reaction at equilibrium when an inert gas is added while the pressure remains unchanged? Here $∆\mathrm{n} >0$

The reaction ${\mathrm{N}}_2 \left(\mathrm{g}\right) + 3{\mathrm{H}}_2 \left(\mathrm{g}\right) \rightleftharpoons 2{\mathrm{NH}}_3 \left(\mathrm{g}\right)$ is in equilibrium. Now the reaction mixture is compressed to half the volume

By adding inert gas at a constant volume, which of the following equilibrium will not be affected?

For the equilibrium: ${\mathrm{PCl}}_5\left(\mathrm{g}\right)\rightleftharpoons {\mathrm{PCl}}_3\left(\mathrm{g}\right)+{\mathrm{Cl}}_2\left(\mathrm{g}\right)$ 

What will be the concentration of ${\mathrm{Cl}}_2\left(\mathrm{g}\right)$, if the equilibrium concentration of ${\mathrm{PCl}}_5\left(\mathrm{g}\right)$ is doubled?

Which of the following statements is incorrect with respect to the given spontaneous reaction?