Factors Affecting Equilibria

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 ${\mathrm{CO}}_2$?

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

Using Le Chatelier's principle, predict the effect of (i) decreasing the temperature and (ii) increasing the pressure on the given equilibria:
$2{\mathrm{CO}}_{\left(\mathrm{g}\right)}+{\mathrm{O}}_{2\left(\mathrm{g}\right)} \rightleftharpoons 2{\mathrm{CO}}_{2\left(\mathrm{g}\right)}+\mathrm{Heat}$

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

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.

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

Suitable conditions for melting of ice are:

In $\mathrm{N}{\mathrm{H}}_3$ solution of $\mathrm{Z}{\mathrm{n}}^{2+},\mathrm{ }\mathrm{Z}{\mathrm{n}}^{2+}$ form $\mathrm{Z}\mathrm{n}{\left(\mathrm{N}{\mathrm{H}}_3\right)}_{4^{2+}}$ . In this solution, to increases the concentration of $\mathrm{Z}{\mathrm{n}}^{2+}$ we are to add -

Consider the reaction $\mathrm{A}\mathrm{ }+\mathrm{ }\mathrm{B}\mathrm{ }\rightleftharpoons \mathrm{ }\mathrm{C}\mathrm{ }+\mathrm{ }\mathrm{D}$. If the blue solution decolourises on heating, then the reaction is:

The equilibrium constant for the reaction:

${\mathrm{N}}_{2\left(\mathrm{g}\right)}\mathrm{ }+\mathrm{ }{\mathrm{O}}_{2\left(\mathrm{g}\right)}\mathrm{ }\rightleftharpoons \mathrm{ }2\mathrm{N}{\mathrm{O}}_{\left(\mathrm{g}\right)}\mathrm{ }\mathrm{i}\mathrm{s}\mathrm{ }4\mathrm{ }\times \mathrm{ }{10}^{–4}\mathrm{ }\mathrm{a}\mathrm{t}\mathrm{ }200\mathrm{ }\mathrm{K}.$ In the presence of a catalyst, equilibrium is attained $10$ times faster. Therefore, the equilibrium constant in the presence of a catalyst at $200 \mathrm{K}$ is:

The equilibrium, ${\mathrm{S}\mathrm{O}}_2{\mathrm{C}\mathrm{l}}_2\mathrm{ }\left(\mathrm{g}\right)\mathrm{ }\rightleftarrows {\mathrm{S}\mathrm{O}}_2\mathrm{ }\left(\mathrm{g}\right)\mathrm{ }+\mathrm{ }{\mathrm{C}\mathrm{l}}_2\mathrm{ }\left(\mathrm{g}\right)$ is attained at $298\mathrm{ }\mathrm{K}$ in a closed container and an inert gas, He is introduced. Which of the following is/are correct ?

Ice and water are placed in a closed container at a pressure of $1\mathrm{ }\mathrm{a}\mathrm{t}\mathrm{m}$ and temperature $273\mathrm{ }\mathrm{K}$. If pressure of the system is increased to $2\mathrm{ }\mathrm{a}\mathrm{t}\mathrm{m}$ while keeping temperature constant, which of the following would be the correct observation ?

Mark out the correct statement for the following conversion



Reaction is usually catalysed by acid or base -