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 ${\mathrm{ClF}}_3?$

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 ${\mathrm{CO}}_2$?

Which of the following statements are correct for the reaction ${\mathrm{SO}}_2{\mathrm{Cl}}_{2\left(\mathrm{g}\right)}\rightleftharpoons {\mathrm{SO}}_{2\left(\mathrm{g}\right)}+{\mathrm{Cl}}_{2\left(\mathrm{g}\right)},$ at $500 \mathrm{K} ?$
a) ${\mathrm{K}}_{\mathrm{p}}>{\mathrm{K}}_{\mathrm{c}}$. 
b) Rate of the forward reaction increases with increasing pressure. 
c) Rate of the forward reaction increases on removing ${\mathrm{Cl}}_2$ gas. 
d) Rate of the forward reaction increases with decreasing pressure. 

For the following reversible reaction,

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

Aqueous solution of ferric nitrate when mixed with aqueous solution of potassium thiocyanate gives red colour solution. The intensity of red colour becomes constant on attaining equilibrium.

Choose the correct statement when the following chemical is added to the above solution at equilibrium
($\mathrm{i}$) Oxalic acid
($\mathrm{ii}$) Mercuric chloride

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?

In a closed vessel, ${\mathrm{NaNO}}_3$ is heated. ${\mathrm{O}}_2$ is liberated and ${\mathrm{NaNO}}_2$ is left behind. At equilibrium

(i) Addition of ${\mathrm{NaNO}}_3$, favours forward reaction.

(ii) Addition of ${\mathrm{NaNO}}_2$, favours backward reaction.

(iii) Increasing pressure favours reverse reaction.

(iv) Increasing temperature favours forward reaction.

Which one of the following is the correct option?

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:

Match the following (There may be one or more correct choices)