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 exothermic formation of ${\mathrm{ClF}}_3$ is represented by the reaction
${\mathrm{Cl}}_2( \mathrm{g})+3{ \mathrm{F}}_2( \mathrm{g}) \rightleftharpoons 2{\mathrm{ClF}}_3 \left(\mathrm{g}\right); ∆\mathrm{H}=-329 \mathrm{kJ}$
Which of the following will increase the quantity of ${\mathrm{ClF}}_3$ in an equilibrium mixture of  ${\mathrm{Cl}}_2,{ \mathrm{F}}_2$ and ${\mathrm{ClF}}_3?$

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 exothermic and reversible. A mixture of ${\mathrm{N}}_{2\left(\mathrm{g}\right)}, {\mathrm{H}}_{2\left(\mathrm{g}\right)}$ and ${\mathrm{NH}}_{3\left(\mathrm{g}\right)}$ is at equilibrium in a closed container. When a certain quantity of extra ${\mathrm{H}}_{2( \mathrm{g})}$ is introduced into the container, while keeping the volume constant, then which statement among the following is true?

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 ${\mathrm{CO}}_2$?

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

From the following graph represents:

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?

The ionisation constant of ${\mathrm{NH}}_4^{+}$ in water is $5.6\times {10}^{-10}$ at $25°\mathrm{C}$. The rate constant for the reaction of ${\mathrm{NH}}_4^{+}$ and ${\mathrm{OH}}^{-}$ to form ${\mathrm{NH}}_3$ and ${\mathrm{H}}_2\mathrm{O}$ at $25°\mathrm{C}$ is $3.4\times {10}^{10} \mathrm{L} {\mathrm{mol}}^{-1}{\sec }^{-1}$. If dissociation constant of water at $25°\mathrm{C}$ is $1.8\times {10}^{-16}$. If ${\mathrm{K}}_{\mathrm{w}}$ of water at $60°\mathrm{C}$ is $9.5\times {10}^{-14},$ then the heat of neutralisation is:

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

In the given diagram, a cylinder is divided by partition $\mathrm{P}$. In compartment $\mathrm{A},$ two gases ${\mathrm{O}}_2$ and ${\mathrm{O}}_3$are in equilibrium with each other.

The reversible reaction
$\left[\mathrm{C}\mathrm{u}\right(\mathrm{N}{\mathrm{H}}_3{)}_4{]}^{2+}+\mathrm{S}{{\mathrm{O}}_3}^{2-}\rightleftharpoons \left[\mathrm{C}\mathrm{u}\right(\mathrm{N}{\mathrm{H}}_3{)}_3\mathrm{S}{\mathrm{O}}_3]+\mathrm{N}{\mathrm{H}}_3$
is at equilibrium. What would not happen if ammonia is added –

Dissociation of phosphorus pentachloride is favoured by –